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AP Chemistry Flashcards: Calculating The Equilibrium Constant

Study Calculating The Equilibrium Constant in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.

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What this deck covers

This deck focuses on Calculating The Equilibrium Constant, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

AP Chemistry Flashcards: Calculating The Equilibrium Constant

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QUESTION

Identify the correct $K_c$ for $\text{CaCO}_3(s)\rightleftharpoons\text{CaO}(s)+\text{CO}_2(g)$ .

Tap or drag to reveal answer

ANSWER

$K_c=[\text{CO}_2]$ . Solids omitted; only gaseous CO₂ appears in the expression.

Swipe Right = I Know It! 🎉

Swipe Left = Still Learning

All flashcards

Flashcard 1: Identify the correct $K_c$ for $\text{CaCO}_3(s)\rightleftharpoons\text{CaO}(s)+\text{CO}_2(g)$ .

Answer: $K_c=[\text{CO}_2]$ . Solids omitted; only gaseous CO₂ appears in the expression.

Flashcard 2: Identify the correct $K_c$ for $\text{N}_2(g)+3\text{H}_2(g)\rightleftharpoons^2\text{NH}_3(g)$ .

Answer: $K_c=\frac{[\text{NH}_3]^2}{[\text{N}_2][\text{H}_2]^3}$ . Products over reactants with coefficients: $2$ for NH₃, $3$ for H₂.

Flashcard 3: Which temperature unit must be used in $K_p=K_c(RT)^{\Delta n}$ calculations?

Answer: $T$ must be in kelvin $(\text{K})$ . Absolute temperature required for ideal gas calculations.

Flashcard 4: What is $\Delta n_{\text{gas}}$ for $K_p=K_c(RT)^{\Delta n_{\text{gas}}}$ ?

Answer: $\Delta n_{\text{gas}}=\sum \nu_{\text{prod,gas}}-\sum \nu_{\text{react,gas}}$ . Change in moles of gas: product coefficients minus reactant coefficients.

Flashcard 5: What is the value of $K$ for any reaction written as $X\rightleftharpoons X$ ?

Answer: $K=1$ . Same species on both sides cancel out, leaving unity.

Flashcard 6: Which species are omitted from $K$ expressions: pure solids, pure liquids, gases, or aqueous solutes?

Answer: Pure solids and pure liquids are omitted. Their activities equal 1, so they don't affect the equilibrium constant.

Flashcard 7: What is the general expression for $K_p$ for $aA+bB\rightleftharpoons cC+dD$ (gases)?

Answer: $K_p=\frac{(P_C)^c(P_D)^d}{(P_A)^a(P_B)^b}$ . Uses partial pressures instead of concentrations for gas-phase equilibria.

Flashcard 8: What is the general expression for $K_c$ for $aA+bB\rightleftharpoons cC+dD$ ?

Answer: $K_c=\frac{[C]^c[D]^d}{[A]^a[B]^b}$ . Products over reactants, each raised to their stoichiometric coefficients.

Flashcard 9: Calculate $K_c$ for $A\rightleftharpoons^2B$ if $[A]=0.50\,\text{M}$ and $[B]=0.20\,\text{M}$ at equilibrium.

Answer: $K_c=0.080$ . $K_c = [B]^2/[A] = (0.20)^2/0.50 = 0.040/0.50 = 0.080$

Flashcard 10: What is $K$ for the reaction if the given reaction has $K=3.0$ and all coefficients are doubled?

Answer: $K_{\text{new}}=9.0$ . Doubling coefficients squares $K$ : $3.0^2 = 9.0$

Flashcard 11: What is $K$ for the reverse reaction if $K=4.0\times10^{-3}$ for the forward reaction?

Answer: $K_{\text{reverse}}=2.5\times10^2$ . $K_{reverse} = 1 ÷ (4.0×10^{-3}) = 2.5×10^2$

Flashcard 12: Find $K_c$ if $K_p=2.0$ , $\Delta n_{\text{gas}}=-2$ , $T=400\,\text{K}$ , and $R=0.0821$ .

Answer: $K_c=2.15\times10^3$ . $K_c = 2.0 ÷ (0.0821 × 400)^{-2} = 2.0 × 1079 = 2.15×10^3$

Flashcard 13: Find $K_p$ if $K_c=0.50$ , $\Delta n_{\text{gas}}=1$ , $T=300\,\text{K}$ , and $R=0.0821$ .

Answer: $K_p=12.3$ . $K_p = 0.50 × (0.0821 × 300)^1 = 0.50 × 24.63 = 12.3$

Flashcard 14: State the relationship between $K_p$ and $K_c$ using $\Delta n_{\text{gas}}$ .

Answer: $K_p=K_c(RT)^{\Delta n_{\text{gas}}}$ . Relates pressure and concentration constants via ideal gas law.

Flashcard 15: What is $K$ for an overall reaction made by adding reactions with constants $K_1$ and $K_2$ ?

Answer: $K_{\text{overall}}=K_1K_2$ . When reactions add, their equilibrium constants multiply.

Flashcard 16: What happens to $K$ when all coefficients in the reaction are multiplied by $n$ ?

Answer: $K_{\text{new}}=K^n$ . Each concentration term gets raised to $n$ , so $K$ is raised to $n$ .

Flashcard 17: What happens to $K$ when the reaction is reversed?

Answer: $K_{\text{reverse}}=\frac{1}{K_{\text{forward}}}$ . Reversing swaps products and reactants, inverting the fraction.

Flashcard 18: Calculate $K_p$ for $2A(g)\rightleftharpoons B(g)$ if $P_A=0.50\,\text{atm}$ and $P_B=2.0\,\text{atm}$ at equilibrium.

Answer: $K_p=8.0$ . $K_p = P_B/(P_A)^2 = 2.0/(0.50)^2 = 2.0/0.25 = 8.0$

Flashcard 19: What is $\Delta n_{\text{gas}}$ for $2\text{SO}_2(g)+\text{O}_2(g)\rightleftharpoons^2\text{SO}_3(g)$ ?

Answer: $\Delta n_{\text{gas}}=-1$ . $2$ moles gas products minus $3$ moles gas reactants equals $-1$ .

Flashcard 20: Identify the correct $K_c$ for $\text{CH}_3\text{COOH}(aq)\rightleftharpoons\text{H}^+(aq)+\text{CH}_3\text{COO}^-(aq)$ .

Answer: $K_c=\frac{[\text{H}^+][\text{CH}_3\text{COO}^-]}{[\text{CH}_3\text{COOH}]}$ . Weak acid dissociation: products over undissociated acid.

Flashcard 21: What is $K$ for the overall reaction if two steps have constants $K_1$ and $K_2$ and are added?

Answer: $K_\text{overall}=K_1K_2$ . When reactions add, equilibrium constants multiply.

Flashcard 22: Calculate $K_c$ if at equilibrium $[A]=0.20\,M$ , $[B]=0.30\,M$ , $[C]=0.40\,M$ for $A+B\rightleftharpoons C$ .

Answer: $K_c=\frac{0.40}{(0.20)(0.30)}=6.7$ . Substitute equilibrium concentrations into $K_c$ expression.

Flashcard 23: Which species are omitted from $K$ for a heterogeneous equilibrium involving pure solids and liquids?

Answer: Pure solids and pure liquids are omitted (activity $=1$ ). Their concentrations remain constant during reaction.

Flashcard 24: What is the effect on $K$ when a reaction is reversed?

Answer: $K_\text{rev}=\frac{1}{K}$ . Reversing flips the fraction, giving the reciprocal.

Flashcard 25: What is the relationship between $K_c$ and $K_p$ using $\Delta n$ and $R,T$ ?

Answer: $K_p=K_c(RT)^{\Delta n}$ . Relates concentration and pressure equilibrium constants.

Flashcard 26: What is $\Delta n$ (used in $K_p=K_c(RT)^{\Delta n}$ ) for gas-phase equilibria?

Answer: $\Delta n=\text{mol gas products}-\text{mol gas reactants}$ . Change in moles of gas from reactants to products.

Flashcard 27: What is the equilibrium constant expression $K_c$ for $2NO_2(g)\rightleftharpoons N_2O_4(g)$ ?

Answer: $K_c=\frac{[N_2O_4]}{[NO_2]^2}$ . Products over reactants with stoichiometric exponents.

Flashcard 28: What is the equilibrium constant expression $K_p$ for $N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)$ ?

Answer: $K_p=\frac{(P_{NH_3})^2}{P_{N_2}(P_{H_2})^3}$ . Partial pressures raised to stoichiometric coefficients.

Flashcard 29: What is $K_c$ for $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ?

Answer: $K_c=[CO_2]$ . Solids omitted; only gas concentration appears.

Flashcard 30: What is $K_p$ for $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ?

Answer: $K_p=P_{CO_2}$ . Solids omitted; only gas pressure appears.

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AP Chemistry Flashcards: Calculating The Equilibrium Constant

Study Calculating The Equilibrium Constant in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.

← Back to flashcard decks

What this deck covers

This deck focuses on Calculating The Equilibrium Constant, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

AP Chemistry Flashcards: Calculating The Equilibrium Constant

/ 30

0 reviewed

0% Complete

0 reviewing

QUESTION

Identify the correct $K_c$ for $\text{CaCO}_3(s)\rightleftharpoons\text{CaO}(s)+\text{CO}_2(g)$ .

Tap or drag to reveal answer

ANSWER

$K_c=[\text{CO}_2]$ . Solids omitted; only gaseous CO₂ appears in the expression.

Swipe Right = I Know It! 🎉

Swipe Left = Still Learning

All flashcards

Flashcard 1: Identify the correct $K_c$ for $\text{CaCO}_3(s)\rightleftharpoons\text{CaO}(s)+\text{CO}_2(g)$ .

Answer: $K_c=[\text{CO}_2]$ . Solids omitted; only gaseous CO₂ appears in the expression.

Flashcard 2: Identify the correct $K_c$ for $\text{N}_2(g)+3\text{H}_2(g)\rightleftharpoons^2\text{NH}_3(g)$ .

Answer: $K_c=\frac{[\text{NH}_3]^2}{[\text{N}_2][\text{H}_2]^3}$ . Products over reactants with coefficients: $2$ for NH₃, $3$ for H₂.

Flashcard 3: Which temperature unit must be used in $K_p=K_c(RT)^{\Delta n}$ calculations?

Answer: $T$ must be in kelvin $(\text{K})$ . Absolute temperature required for ideal gas calculations.

Flashcard 4: What is $\Delta n_{\text{gas}}$ for $K_p=K_c(RT)^{\Delta n_{\text{gas}}}$ ?

Answer: $\Delta n_{\text{gas}}=\sum \nu_{\text{prod,gas}}-\sum \nu_{\text{react,gas}}$ . Change in moles of gas: product coefficients minus reactant coefficients.

Flashcard 5: What is the value of $K$ for any reaction written as $X\rightleftharpoons X$ ?

Answer: $K=1$ . Same species on both sides cancel out, leaving unity.

Flashcard 6: Which species are omitted from $K$ expressions: pure solids, pure liquids, gases, or aqueous solutes?

Answer: Pure solids and pure liquids are omitted. Their activities equal 1, so they don't affect the equilibrium constant.

Flashcard 7: What is the general expression for $K_p$ for $aA+bB\rightleftharpoons cC+dD$ (gases)?

Answer: $K_p=\frac{(P_C)^c(P_D)^d}{(P_A)^a(P_B)^b}$ . Uses partial pressures instead of concentrations for gas-phase equilibria.

Flashcard 8: What is the general expression for $K_c$ for $aA+bB\rightleftharpoons cC+dD$ ?

Answer: $K_c=\frac{[C]^c[D]^d}{[A]^a[B]^b}$ . Products over reactants, each raised to their stoichiometric coefficients.

Flashcard 9: Calculate $K_c$ for $A\rightleftharpoons^2B$ if $[A]=0.50\,\text{M}$ and $[B]=0.20\,\text{M}$ at equilibrium.

Answer: $K_c=0.080$ . $K_c = [B]^2/[A] = (0.20)^2/0.50 = 0.040/0.50 = 0.080$

Flashcard 10: What is $K$ for the reaction if the given reaction has $K=3.0$ and all coefficients are doubled?

Answer: $K_{\text{new}}=9.0$ . Doubling coefficients squares $K$ : $3.0^2 = 9.0$

Flashcard 11: What is $K$ for the reverse reaction if $K=4.0\times10^{-3}$ for the forward reaction?

Answer: $K_{\text{reverse}}=2.5\times10^2$ . $K_{reverse} = 1 ÷ (4.0×10^{-3}) = 2.5×10^2$

Flashcard 12: Find $K_c$ if $K_p=2.0$ , $\Delta n_{\text{gas}}=-2$ , $T=400\,\text{K}$ , and $R=0.0821$ .

Answer: $K_c=2.15\times10^3$ . $K_c = 2.0 ÷ (0.0821 × 400)^{-2} = 2.0 × 1079 = 2.15×10^3$

Flashcard 13: Find $K_p$ if $K_c=0.50$ , $\Delta n_{\text{gas}}=1$ , $T=300\,\text{K}$ , and $R=0.0821$ .

Answer: $K_p=12.3$ . $K_p = 0.50 × (0.0821 × 300)^1 = 0.50 × 24.63 = 12.3$

Flashcard 14: State the relationship between $K_p$ and $K_c$ using $\Delta n_{\text{gas}}$ .

Answer: $K_p=K_c(RT)^{\Delta n_{\text{gas}}}$ . Relates pressure and concentration constants via ideal gas law.

Flashcard 15: What is $K$ for an overall reaction made by adding reactions with constants $K_1$ and $K_2$ ?

Answer: $K_{\text{overall}}=K_1K_2$ . When reactions add, their equilibrium constants multiply.

Flashcard 16: What happens to $K$ when all coefficients in the reaction are multiplied by $n$ ?

Answer: $K_{\text{new}}=K^n$ . Each concentration term gets raised to $n$ , so $K$ is raised to $n$ .

Flashcard 17: What happens to $K$ when the reaction is reversed?

Answer: $K_{\text{reverse}}=\frac{1}{K_{\text{forward}}}$ . Reversing swaps products and reactants, inverting the fraction.

Flashcard 18: Calculate $K_p$ for $2A(g)\rightleftharpoons B(g)$ if $P_A=0.50\,\text{atm}$ and $P_B=2.0\,\text{atm}$ at equilibrium.

Answer: $K_p=8.0$ . $K_p = P_B/(P_A)^2 = 2.0/(0.50)^2 = 2.0/0.25 = 8.0$

Flashcard 19: What is $\Delta n_{\text{gas}}$ for $2\text{SO}_2(g)+\text{O}_2(g)\rightleftharpoons^2\text{SO}_3(g)$ ?

Answer: $\Delta n_{\text{gas}}=-1$ . $2$ moles gas products minus $3$ moles gas reactants equals $-1$ .

Flashcard 20: Identify the correct $K_c$ for $\text{CH}_3\text{COOH}(aq)\rightleftharpoons\text{H}^+(aq)+\text{CH}_3\text{COO}^-(aq)$ .

Answer: $K_c=\frac{[\text{H}^+][\text{CH}_3\text{COO}^-]}{[\text{CH}_3\text{COOH}]}$ . Weak acid dissociation: products over undissociated acid.

Flashcard 21: What is $K$ for the overall reaction if two steps have constants $K_1$ and $K_2$ and are added?

Answer: $K_\text{overall}=K_1K_2$ . When reactions add, equilibrium constants multiply.

Flashcard 22: Calculate $K_c$ if at equilibrium $[A]=0.20\,M$ , $[B]=0.30\,M$ , $[C]=0.40\,M$ for $A+B\rightleftharpoons C$ .

Answer: $K_c=\frac{0.40}{(0.20)(0.30)}=6.7$ . Substitute equilibrium concentrations into $K_c$ expression.

Flashcard 23: Which species are omitted from $K$ for a heterogeneous equilibrium involving pure solids and liquids?

Answer: Pure solids and pure liquids are omitted (activity $=1$ ). Their concentrations remain constant during reaction.

Flashcard 24: What is the effect on $K$ when a reaction is reversed?

Answer: $K_\text{rev}=\frac{1}{K}$ . Reversing flips the fraction, giving the reciprocal.

Flashcard 25: What is the relationship between $K_c$ and $K_p$ using $\Delta n$ and $R,T$ ?

Answer: $K_p=K_c(RT)^{\Delta n}$ . Relates concentration and pressure equilibrium constants.

Flashcard 26: What is $\Delta n$ (used in $K_p=K_c(RT)^{\Delta n}$ ) for gas-phase equilibria?

Answer: $\Delta n=\text{mol gas products}-\text{mol gas reactants}$ . Change in moles of gas from reactants to products.

Flashcard 27: What is the equilibrium constant expression $K_c$ for $2NO_2(g)\rightleftharpoons N_2O_4(g)$ ?

Answer: $K_c=\frac{[N_2O_4]}{[NO_2]^2}$ . Products over reactants with stoichiometric exponents.

Flashcard 28: What is the equilibrium constant expression $K_p$ for $N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)$ ?

Answer: $K_p=\frac{(P_{NH_3})^2}{P_{N_2}(P_{H_2})^3}$ . Partial pressures raised to stoichiometric coefficients.

Flashcard 29: What is $K_c$ for $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ?

Answer: $K_c=[CO_2]$ . Solids omitted; only gas concentration appears.

Flashcard 30: What is $K_p$ for $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ?

Answer: $K_p=P_{CO_2}$ . Solids omitted; only gas pressure appears.

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AP Chemistry Flashcards: Calculating The Equilibrium Constant

What this deck covers

How to use these flashcards

AP Chemistry Flashcards: Calculating The Equilibrium Constant

All flashcards

Flashcard 1: Identify the correct KcK_cKc​ for CaCO3(s)⇌CaO(s)+CO2(g)\text{CaCO}_3(s)\rightleftharpoons\text{CaO}(s)+\text{CO}_2(g)CaCO3​(s)⇌CaO(s)+CO2​(g).

Flashcard 2: Identify the correct KcK_cKc​ for N2(g)+3H2(g)⇌2NH3(g)\text{N}_2(g)+3\text{H}_2(g)\rightleftharpoons^2\text{NH}_3(g)N2​(g)+3H2​(g)⇌2NH3​(g).

Flashcard 3: Which temperature unit must be used in Kp=Kc(RT)ΔnK_p=K_c(RT)^{\Delta n}Kp​=Kc​(RT)Δn calculations?

Flashcard 4: What is Δngas\Delta n_{\text{gas}}Δngas​ for Kp=Kc(RT)ΔngasK_p=K_c(RT)^{\Delta n_{\text{gas}}}Kp​=Kc​(RT)Δngas​?

Flashcard 5: What is the value of KKK for any reaction written as X⇌XX\rightleftharpoons XX⇌X?

Flashcard 6: Which species are omitted from KKK expressions: pure solids, pure liquids, gases, or aqueous solutes?

Flashcard 7: What is the general expression for KpK_pKp​ for aA+bB⇌cC+dDaA+bB\rightleftharpoons cC+dDaA+bB⇌cC+dD (gases)?

Flashcard 8: What is the general expression for KcK_cKc​ for aA+bB⇌cC+dDaA+bB\rightleftharpoons cC+dDaA+bB⇌cC+dD?

Flashcard 9: Calculate KcK_cKc​ for A⇌2BA\rightleftharpoons^2BA⇌2B if [A]=0.50 M[A]=0.50\,\text{M}[A]=0.50M and [B]=0.20 M[B]=0.20\,\text{M}[B]=0.20M at equilibrium.

Flashcard 10: What is KKK for the reaction if the given reaction has K=3.0K=3.0K=3.0 and all coefficients are doubled?

Flashcard 11: What is KKK for the reverse reaction if K=4.0×10−3K=4.0\times10^{-3}K=4.0×10−3 for the forward reaction?

Flashcard 12: Find KcK_cKc​ if Kp=2.0K_p=2.0Kp​=2.0, Δngas=−2\Delta n_{\text{gas}}=-2Δngas​=−2, T=400 KT=400\,\text{K}T=400K, and R=0.0821R=0.0821R=0.0821.

Flashcard 13: Find KpK_pKp​ if Kc=0.50K_c=0.50Kc​=0.50, Δngas=1\Delta n_{\text{gas}}=1Δngas​=1, T=300 KT=300\,\text{K}T=300K, and R=0.0821R=0.0821R=0.0821.

Flashcard 14: State the relationship between KpK_pKp​ and KcK_cKc​ using Δngas\Delta n_{\text{gas}}Δngas​.

Flashcard 15: What is KKK for an overall reaction made by adding reactions with constants K1K_1K1​ and K2K_2K2​?

Flashcard 16: What happens to KKK when all coefficients in the reaction are multiplied by nnn?

Flashcard 17: What happens to KKK when the reaction is reversed?

Flashcard 18: Calculate KpK_pKp​ for 2A(g)⇌B(g)2A(g)\rightleftharpoons B(g)2A(g)⇌B(g) if PA=0.50 atmP_A=0.50\,\text{atm}PA​=0.50atm and PB=2.0 atmP_B=2.0\,\text{atm}PB​=2.0atm at equilibrium.

Flashcard 19: What is Δngas\Delta n_{\text{gas}}Δngas​ for 2SO2(g)+O2(g)⇌2SO3(g)2\text{SO}_2(g)+\text{O}_2(g)\rightleftharpoons^2\text{SO}_3(g)2SO2​(g)+O2​(g)⇌2SO3​(g)?

Flashcard 20: Identify the correct KcK_cKc​ for CH3COOH(aq)⇌H+(aq)+CH3COO−(aq)\text{CH}_3\text{COOH}(aq)\rightleftharpoons\text{H}^+(aq)+\text{CH}_3\text{COO}^-(aq)CH3​COOH(aq)⇌H+(aq)+CH3​COO−(aq).

Flashcard 21: What is KKK for the overall reaction if two steps have constants K1K_1K1​ and K2K_2K2​ and are added?

Flashcard 22: Calculate KcK_cKc​ if at equilibrium [A]=0.20 M[A]=0.20\,M[A]=0.20M, [B]=0.30 M[B]=0.30\,M[B]=0.30M, [C]=0.40 M[C]=0.40\,M[C]=0.40M for A+B⇌CA+B\rightleftharpoons CA+B⇌C.

Flashcard 23: Which species are omitted from KKK for a heterogeneous equilibrium involving pure solids and liquids?

Flashcard 24: What is the effect on KKK when a reaction is reversed?

Flashcard 25: What is the relationship between KcK_cKc​ and KpK_pKp​ using Δn\Delta nΔn and R,TR,TR,T?

Flashcard 26: What is Δn\Delta nΔn (used in Kp=Kc(RT)ΔnK_p=K_c(RT)^{\Delta n}Kp​=Kc​(RT)Δn) for gas-phase equilibria?

Flashcard 27: What is the equilibrium constant expression KcK_cKc​ for 2NO2(g)⇌N2O4(g)2NO_2(g)\rightleftharpoons N_2O_4(g)2NO2​(g)⇌N2​O4​(g)?

Flashcard 28: What is the equilibrium constant expression KpK_pKp​ for N2(g)+3H2(g)⇌2NH3(g)N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)N2​(g)+3H2​(g)⇌2NH3​(g)?

Flashcard 29: What is KcK_cKc​ for CaCO3(s)⇌CaO(s)+CO2(g)CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)CaCO3​(s)⇌CaO(s)+CO2​(g)?

Flashcard 30: What is KpK_pKp​ for CaCO3(s)⇌CaO(s)+CO2(g)CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)CaCO3​(s)⇌CaO(s)+CO2​(g)?

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AP Chemistry Flashcards: Calculating The Equilibrium Constant

What this deck covers

How to use these flashcards

AP Chemistry Flashcards: Calculating The Equilibrium Constant

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Flashcard 1: Identify the correct KcK_cKc​ for CaCO3(s)⇌CaO(s)+CO2(g)\text{CaCO}_3(s)\rightleftharpoons\text{CaO}(s)+\text{CO}_2(g)CaCO3​(s)⇌CaO(s)+CO2​(g).

Flashcard 2: Identify the correct KcK_cKc​ for N2(g)+3H2(g)⇌2NH3(g)\text{N}_2(g)+3\text{H}_2(g)\rightleftharpoons^2\text{NH}_3(g)N2​(g)+3H2​(g)⇌2NH3​(g).

Flashcard 3: Which temperature unit must be used in Kp=Kc(RT)ΔnK_p=K_c(RT)^{\Delta n}Kp​=Kc​(RT)Δn calculations?

Flashcard 4: What is Δngas\Delta n_{\text{gas}}Δngas​ for Kp=Kc(RT)ΔngasK_p=K_c(RT)^{\Delta n_{\text{gas}}}Kp​=Kc​(RT)Δngas​?

Flashcard 5: What is the value of KKK for any reaction written as X⇌XX\rightleftharpoons XX⇌X?

Flashcard 6: Which species are omitted from KKK expressions: pure solids, pure liquids, gases, or aqueous solutes?

Flashcard 7: What is the general expression for KpK_pKp​ for aA+bB⇌cC+dDaA+bB\rightleftharpoons cC+dDaA+bB⇌cC+dD (gases)?

Flashcard 8: What is the general expression for KcK_cKc​ for aA+bB⇌cC+dDaA+bB\rightleftharpoons cC+dDaA+bB⇌cC+dD?

Flashcard 9: Calculate KcK_cKc​ for A⇌2BA\rightleftharpoons^2BA⇌2B if [A]=0.50 M[A]=0.50\,\text{M}[A]=0.50M and [B]=0.20 M[B]=0.20\,\text{M}[B]=0.20M at equilibrium.

Flashcard 10: What is KKK for the reaction if the given reaction has K=3.0K=3.0K=3.0 and all coefficients are doubled?

Flashcard 11: What is KKK for the reverse reaction if K=4.0×10−3K=4.0\times10^{-3}K=4.0×10−3 for the forward reaction?

Flashcard 12: Find KcK_cKc​ if Kp=2.0K_p=2.0Kp​=2.0, Δngas=−2\Delta n_{\text{gas}}=-2Δngas​=−2, T=400 KT=400\,\text{K}T=400K, and R=0.0821R=0.0821R=0.0821.

Flashcard 13: Find KpK_pKp​ if Kc=0.50K_c=0.50Kc​=0.50, Δngas=1\Delta n_{\text{gas}}=1Δngas​=1, T=300 KT=300\,\text{K}T=300K, and R=0.0821R=0.0821R=0.0821.

Flashcard 14: State the relationship between KpK_pKp​ and KcK_cKc​ using Δngas\Delta n_{\text{gas}}Δngas​.

Flashcard 15: What is KKK for an overall reaction made by adding reactions with constants K1K_1K1​ and K2K_2K2​?

Flashcard 16: What happens to KKK when all coefficients in the reaction are multiplied by nnn?

Flashcard 17: What happens to KKK when the reaction is reversed?

Flashcard 18: Calculate KpK_pKp​ for 2A(g)⇌B(g)2A(g)\rightleftharpoons B(g)2A(g)⇌B(g) if PA=0.50 atmP_A=0.50\,\text{atm}PA​=0.50atm and PB=2.0 atmP_B=2.0\,\text{atm}PB​=2.0atm at equilibrium.

Flashcard 19: What is Δngas\Delta n_{\text{gas}}Δngas​ for 2SO2(g)+O2(g)⇌2SO3(g)2\text{SO}_2(g)+\text{O}_2(g)\rightleftharpoons^2\text{SO}_3(g)2SO2​(g)+O2​(g)⇌2SO3​(g)?

Flashcard 20: Identify the correct KcK_cKc​ for CH3COOH(aq)⇌H+(aq)+CH3COO−(aq)\text{CH}_3\text{COOH}(aq)\rightleftharpoons\text{H}^+(aq)+\text{CH}_3\text{COO}^-(aq)CH3​COOH(aq)⇌H+(aq)+CH3​COO−(aq).

Flashcard 21: What is KKK for the overall reaction if two steps have constants K1K_1K1​ and K2K_2K2​ and are added?

Flashcard 22: Calculate KcK_cKc​ if at equilibrium [A]=0.20 M[A]=0.20\,M[A]=0.20M, [B]=0.30 M[B]=0.30\,M[B]=0.30M, [C]=0.40 M[C]=0.40\,M[C]=0.40M for A+B⇌CA+B\rightleftharpoons CA+B⇌C.

Flashcard 23: Which species are omitted from KKK for a heterogeneous equilibrium involving pure solids and liquids?

Flashcard 24: What is the effect on KKK when a reaction is reversed?

Flashcard 25: What is the relationship between KcK_cKc​ and KpK_pKp​ using Δn\Delta nΔn and R,TR,TR,T?

Flashcard 26: What is Δn\Delta nΔn (used in Kp=Kc(RT)ΔnK_p=K_c(RT)^{\Delta n}Kp​=Kc​(RT)Δn) for gas-phase equilibria?

Flashcard 27: What is the equilibrium constant expression KcK_cKc​ for 2NO2(g)⇌N2O4(g)2NO_2(g)\rightleftharpoons N_2O_4(g)2NO2​(g)⇌N2​O4​(g)?

Flashcard 28: What is the equilibrium constant expression KpK_pKp​ for N2(g)+3H2(g)⇌2NH3(g)N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)N2​(g)+3H2​(g)⇌2NH3​(g)?

Flashcard 29: What is KcK_cKc​ for CaCO3(s)⇌CaO(s)+CO2(g)CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)CaCO3​(s)⇌CaO(s)+CO2​(g)?

Flashcard 30: What is KpK_pKp​ for CaCO3(s)⇌CaO(s)+CO2(g)CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)CaCO3​(s)⇌CaO(s)+CO2​(g)?

Flashcard 1: Identify the correct $K_c$ for $\text{CaCO}_3(s)\rightleftharpoons\text{CaO}(s)+\text{CO}_2(g)$ .

Flashcard 2: Identify the correct $K_c$ for $\text{N}_2(g)+3\text{H}_2(g)\rightleftharpoons^2\text{NH}_3(g)$ .

Flashcard 3: Which temperature unit must be used in $K_p=K_c(RT)^{\Delta n}$ calculations?

Flashcard 4: What is $\Delta n_{\text{gas}}$ for $K_p=K_c(RT)^{\Delta n_{\text{gas}}}$ ?

Flashcard 5: What is the value of $K$ for any reaction written as $X\rightleftharpoons X$ ?

Flashcard 6: Which species are omitted from $K$ expressions: pure solids, pure liquids, gases, or aqueous solutes?

Flashcard 7: What is the general expression for $K_p$ for $aA+bB\rightleftharpoons cC+dD$ (gases)?

Flashcard 8: What is the general expression for $K_c$ for $aA+bB\rightleftharpoons cC+dD$ ?

Flashcard 9: Calculate $K_c$ for $A\rightleftharpoons^2B$ if $[A]=0.50\,\text{M}$ and $[B]=0.20\,\text{M}$ at equilibrium.

Flashcard 10: What is $K$ for the reaction if the given reaction has $K=3.0$ and all coefficients are doubled?

Flashcard 11: What is $K$ for the reverse reaction if $K=4.0\times10^{-3}$ for the forward reaction?

Flashcard 12: Find $K_c$ if $K_p=2.0$ , $\Delta n_{\text{gas}}=-2$ , $T=400\,\text{K}$ , and $R=0.0821$ .

Flashcard 13: Find $K_p$ if $K_c=0.50$ , $\Delta n_{\text{gas}}=1$ , $T=300\,\text{K}$ , and $R=0.0821$ .

Flashcard 14: State the relationship between $K_p$ and $K_c$ using $\Delta n_{\text{gas}}$ .

Flashcard 15: What is $K$ for an overall reaction made by adding reactions with constants $K_1$ and $K_2$ ?

Flashcard 16: What happens to $K$ when all coefficients in the reaction are multiplied by $n$ ?

Flashcard 17: What happens to $K$ when the reaction is reversed?

Flashcard 18: Calculate $K_p$ for $2A(g)\rightleftharpoons B(g)$ if $P_A=0.50\,\text{atm}$ and $P_B=2.0\,\text{atm}$ at equilibrium.

Flashcard 19: What is $\Delta n_{\text{gas}}$ for $2\text{SO}_2(g)+\text{O}_2(g)\rightleftharpoons^2\text{SO}_3(g)$ ?

Flashcard 20: Identify the correct $K_c$ for $\text{CH}_3\text{COOH}(aq)\rightleftharpoons\text{H}^+(aq)+\text{CH}_3\text{COO}^-(aq)$ .

Flashcard 21: What is $K$ for the overall reaction if two steps have constants $K_1$ and $K_2$ and are added?

Flashcard 22: Calculate $K_c$ if at equilibrium $[A]=0.20\,M$ , $[B]=0.30\,M$ , $[C]=0.40\,M$ for $A+B\rightleftharpoons C$ .

Flashcard 23: Which species are omitted from $K$ for a heterogeneous equilibrium involving pure solids and liquids?

Flashcard 24: What is the effect on $K$ when a reaction is reversed?

Flashcard 25: What is the relationship between $K_c$ and $K_p$ using $\Delta n$ and $R,T$ ?

Flashcard 26: What is $\Delta n$ (used in $K_p=K_c(RT)^{\Delta n}$ ) for gas-phase equilibria?

Flashcard 27: What is the equilibrium constant expression $K_c$ for $2NO_2(g)\rightleftharpoons N_2O_4(g)$ ?

Flashcard 28: What is the equilibrium constant expression $K_p$ for $N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)$ ?

Flashcard 29: What is $K_c$ for $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ?

Flashcard 30: What is $K_p$ for $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ?

Flashcard 1: Identify the correct $K_c$ for $\text{CaCO}_3(s)\rightleftharpoons\text{CaO}(s)+\text{CO}_2(g)$ .

Flashcard 2: Identify the correct $K_c$ for $\text{N}_2(g)+3\text{H}_2(g)\rightleftharpoons^2\text{NH}_3(g)$ .

Flashcard 3: Which temperature unit must be used in $K_p=K_c(RT)^{\Delta n}$ calculations?

Flashcard 4: What is $\Delta n_{\text{gas}}$ for $K_p=K_c(RT)^{\Delta n_{\text{gas}}}$ ?

Flashcard 5: What is the value of $K$ for any reaction written as $X\rightleftharpoons X$ ?

Flashcard 6: Which species are omitted from $K$ expressions: pure solids, pure liquids, gases, or aqueous solutes?

Flashcard 7: What is the general expression for $K_p$ for $aA+bB\rightleftharpoons cC+dD$ (gases)?

Flashcard 8: What is the general expression for $K_c$ for $aA+bB\rightleftharpoons cC+dD$ ?

Flashcard 9: Calculate $K_c$ for $A\rightleftharpoons^2B$ if $[A]=0.50\,\text{M}$ and $[B]=0.20\,\text{M}$ at equilibrium.

Flashcard 10: What is $K$ for the reaction if the given reaction has $K=3.0$ and all coefficients are doubled?

Flashcard 11: What is $K$ for the reverse reaction if $K=4.0\times10^{-3}$ for the forward reaction?

Flashcard 12: Find $K_c$ if $K_p=2.0$ , $\Delta n_{\text{gas}}=-2$ , $T=400\,\text{K}$ , and $R=0.0821$ .

Flashcard 13: Find $K_p$ if $K_c=0.50$ , $\Delta n_{\text{gas}}=1$ , $T=300\,\text{K}$ , and $R=0.0821$ .

Flashcard 14: State the relationship between $K_p$ and $K_c$ using $\Delta n_{\text{gas}}$ .

Flashcard 15: What is $K$ for an overall reaction made by adding reactions with constants $K_1$ and $K_2$ ?

Flashcard 16: What happens to $K$ when all coefficients in the reaction are multiplied by $n$ ?

Flashcard 17: What happens to $K$ when the reaction is reversed?

Flashcard 18: Calculate $K_p$ for $2A(g)\rightleftharpoons B(g)$ if $P_A=0.50\,\text{atm}$ and $P_B=2.0\,\text{atm}$ at equilibrium.

Flashcard 19: What is $\Delta n_{\text{gas}}$ for $2\text{SO}_2(g)+\text{O}_2(g)\rightleftharpoons^2\text{SO}_3(g)$ ?

Flashcard 20: Identify the correct $K_c$ for $\text{CH}_3\text{COOH}(aq)\rightleftharpoons\text{H}^+(aq)+\text{CH}_3\text{COO}^-(aq)$ .

Flashcard 21: What is $K$ for the overall reaction if two steps have constants $K_1$ and $K_2$ and are added?

Flashcard 22: Calculate $K_c$ if at equilibrium $[A]=0.20\,M$ , $[B]=0.30\,M$ , $[C]=0.40\,M$ for $A+B\rightleftharpoons C$ .

Flashcard 23: Which species are omitted from $K$ for a heterogeneous equilibrium involving pure solids and liquids?

Flashcard 24: What is the effect on $K$ when a reaction is reversed?

Flashcard 25: What is the relationship between $K_c$ and $K_p$ using $\Delta n$ and $R,T$ ?

Flashcard 26: What is $\Delta n$ (used in $K_p=K_c(RT)^{\Delta n}$ ) for gas-phase equilibria?

Flashcard 27: What is the equilibrium constant expression $K_c$ for $2NO_2(g)\rightleftharpoons N_2O_4(g)$ ?

Flashcard 28: What is the equilibrium constant expression $K_p$ for $N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)$ ?

Flashcard 29: What is $K_c$ for $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ?

Flashcard 30: What is $K_p$ for $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ?