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AP Chemistry Flashcards: Magnitude Of The Equilibrium Constant

Study Magnitude Of 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 Magnitude Of The Equilibrium Constant, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

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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: Magnitude Of The Equilibrium Constant

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QUESTION

What is true about the equilibrium constant when a reaction reaches equilibrium?

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ANSWER

The rate of the forward and reverse reactions are equal. At equilibrium, the equilibrium constant value remains constant.

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Flashcard 1: What is true about the equilibrium constant when a reaction reaches equilibrium?

Answer: The rate of the forward and reverse reactions are equal. At equilibrium, the equilibrium constant value remains constant.

Flashcard 2: What is the expression for the equilibrium constant KcK_cKc​ for the reaction aA+bB⇌cC+dDaA + bB \rightleftharpoons cC + dDaA+bB⇌cC+dD?

Answer: Kc=[C]c[D]d[A]a[B]bK_c = \frac{[C]^c[D]^d}{[A]^a[B]^b}Kc​=[A]a[B]b[C]c[D]d​. Products raised to coefficients over reactants raised to coefficients.

Flashcard 3: If the equilibrium constant KKK for a reaction is 0.010.010.01, what does this suggest?

Answer: The reaction is reactant-favored. K<1K < 1K<1 means reactants predominate at equilibrium.

Flashcard 4: What does a large KcK_cKc​ value indicate about the position of equilibrium?

Answer: The equilibrium favors products. Large KKK means products are more abundant at equilibrium.

Flashcard 5: For N2(g)+O2(g)⇌2NO(g)N_2(g) + O_2(g) \rightleftharpoons 2NO(g)N2​(g)+O2​(g)⇌2NO(g), write the KcK_cKc​ expression.

Answer: Kc=[NO]2[N2][O2]K_c = \frac{[NO]^2}{[N_2][O_2]}Kc​=[N2​][O2​][NO]2​. Products over reactants, raised to stoichiometric coefficients.

Flashcard 6: What is the effect on KcK_cKc​ if the temperature increases for an endothermic reaction?

Answer: KcK_cKc​ increases. Higher temperature favors endothermic direction (products).

Flashcard 7: For the reaction 2A(g)⇌B(g)+C(g)2A(g) \rightleftharpoons B(g) + C(g)2A(g)⇌B(g)+C(g), write the KpK_pKp​ expression.

Answer: Kp=PBPCPA2K_p = \frac{P_B P_C}{P_A^2}Kp​=PA2​PB​PC​​. Partial pressures of products over reactants, raised to coefficients.

Flashcard 8: What does a small KcK_cKc​ value indicate about the position of equilibrium?

Answer: The equilibrium favors reactants. Small KKK means reactants are more abundant at equilibrium.

Flashcard 9: Determine the KcK_cKc​ expression for 2NO2(g)⇌N2O4(g)2NO_2(g) \rightleftharpoons N_2O_4(g)2NO2​(g)⇌N2​O4​(g).

Answer: Kc=[N2O4][NO2]2K_c = \frac{[N_2O_4]}{[NO_2]^2}Kc​=[NO2​]2[N2​O4​]​. Products over reactants, with each raised to stoichiometric coefficients.

Flashcard 10: Identify the equilibrium constant expression KpK_pKp​ for the reaction aA(g)+bB(g)⇌cC(g)+dD(g)aA(g) + bB(g) \rightleftharpoons cC(g) + dD(g)aA(g)+bB(g)⇌cC(g)+dD(g).

Answer: Kp=(PC)c(PD)d(PA)a(PB)bK_p = \frac{(P_C)^c(P_D)^d}{(P_A)^a(P_B)^b}Kp​=(PA​)a(PB​)b(PC​)c(PD​)d​. Uses partial pressures instead of concentrations in the expression.

Flashcard 11: State the relationship between KcK_cKc​ and the rate constants kfk_fkf​ and krk_rkr​ for a reaction.

Answer: Kc=kfkrK_c = \frac{k_f}{k_r}Kc​=kr​kf​​. Ratio of forward to reverse rate constants equals equilibrium constant.

Flashcard 12: What is the effect on KcK_cKc​ if the temperature decreases for an endothermic reaction?

Answer: KcK_cKc​ decreases. Lower temperature shifts endothermic equilibrium toward reactants.

Flashcard 13: What is the equilibrium constant KcK_cKc​ for the reverse reaction if the forward reaction has Kc=10K_c = 10Kc​=10?

Answer: Kc=0.1K_c = 0.1Kc​=0.1. Reverse reaction constant equals 1/Kforward1/K_{forward}1/Kforward​.

Flashcard 14: If Kc=1000K_c = 1000Kc​=1000 for a reaction, is it product or reactant favored?

Answer: Product favored. K>1K > 1K>1 indicates products are favored at equilibrium.

Flashcard 15: For the equilibrium PCl5(g)⇌PCl3(g)+Cl2(g)PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)PCl5​(g)⇌PCl3​(g)+Cl2​(g), write the KcK_cKc​ expression.

Answer: Kc=[PCl3][Cl2][PCl5]K_c = \frac{[PCl_3][Cl_2]}{[PCl_5]}Kc​=[PCl5​][PCl3​][Cl2​]​. Products over reactants, raised to stoichiometric coefficients.

Flashcard 16: Determine the KcK_cKc​ expression for CH4(g)+2O2(g)⇌CO2(g)+2H2O(g)CH_4(g) + 2O_2(g) \rightleftharpoons CO_2(g) + 2H_2O(g)CH4​(g)+2O2​(g)⇌CO2​(g)+2H2​O(g).

Answer: Kc=[CO2][H2O]2[CH4][O2]2K_c = \frac{[CO_2][H_2O]^2}{[CH_4][O_2]^2}Kc​=[CH4​][O2​]2[CO2​][H2​O]2​. Products over reactants, each raised to their stoichiometric coefficients.

Flashcard 17: How does KcK_cKc​ change if a catalyst is added to a reaction?

Answer: KcK_cKc​ remains unchanged. Catalysts affect reaction rate but not equilibrium position.

Flashcard 18: Predict how KcK_cKc​ will shift if pressure is increased for N2(g)+3H2(g)⇌2NH3(g)N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)N2​(g)+3H2​(g)⇌2NH3​(g).

Answer: KcK_cKc​ does not change. Equilibrium constant depends only on temperature, not pressure.

Flashcard 19: What is the expression for KcK_cKc​ for the decomposition of H2O(g)H_2O(g)H2​O(g) into H2(g)H_2(g)H2​(g) and O2(g)O_2(g)O2​(g)?

Answer: Kc=[H2]2[O2][H2O]2K_c = \frac{[H_2]^2[O_2]}{[H_2O]^2}Kc​=[H2​O]2[H2​]2[O2​]​. Decomposition: 2H2O(g)⇌2H2(g)+O2(g)2H_2O(g) \rightleftharpoons 2H_2(g) + O_2(g)2H2​O(g)⇌2H2​(g)+O2​(g).

Flashcard 20: What is the equilibrium expression for KcK_cKc​ for the reaction 2SO3(g)⇌2SO2(g)+O2(g)2SO_3(g) \rightleftharpoons 2SO_2(g) + O_2(g)2SO3​(g)⇌2SO2​(g)+O2​(g)?

Answer: Kc=[SO2]2[O2][SO3]2K_c = \frac{[SO_2]^2[O_2]}{[SO_3]^2}Kc​=[SO3​]2[SO2​]2[O2​]​. Products over reactants, raised to stoichiometric coefficients.

Flashcard 21: For 2NO(g)+O2(g)⇌2NO2(g)2NO(g) + O_2(g) \rightleftharpoons 2NO_2(g)2NO(g)+O2​(g)⇌2NO2​(g), provide the KcK_cKc​ expression.

Answer: Kc=[NO2]2[NO]2[O2]K_c = \frac{[NO_2]^2}{[NO]^2[O_2]}Kc​=[NO]2[O2​][NO2​]2​. Products over reactants, raised to stoichiometric coefficients.

Flashcard 22: For 2SO2(g)+O2(g)⇌2SO3(g)2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)2SO2​(g)+O2​(g)⇌2SO3​(g), write the KcK_cKc​ expression.

Answer: Kc=[SO3]2[SO2]2[O2]K_c = \frac{[SO_3]^2}{[SO_2]^2[O_2]}Kc​=[SO2​]2[O2​][SO3​]2​. Products over reactants, raised to stoichiometric coefficients.

Flashcard 23: Calculate KpK_pKp​ from Kc=50K_c = 50Kc​=50 for H2(g)+I2(g)⇌2HI(g)H_2(g) + I_2(g) \rightleftharpoons 2HI(g)H2​(g)+I2​(g)⇌2HI(g) at 300 K.

Answer: Kp=50K_p = 50Kp​=50. Δn=0\Delta n = 0Δn=0, so Kp=KcK_p = K_cKp​=Kc​.

Flashcard 24: What will happen to KcK_cKc​ if the equation coefficients are doubled?

Answer: KcK_cKc​ is squared. When coefficients are multiplied by nnn, KKK is raised to the nnnth power.

Flashcard 25: What happens to KcK_cKc​ if the equation is reversed?

Answer: KcK_cKc​ becomes 1/Kc1/K_c1/Kc​. Reversing the equation inverts the equilibrium constant.

Flashcard 26: What is the effect on KpK_pKp​ if the temperature increases for an exothermic reaction?

Answer: KpK_pKp​ decreases. Le Chatelier's principle: heat shifts equilibrium toward reactants.

Flashcard 27: If the equilibrium constant KKK for a reaction is 0.010.010.01, what does this suggest?

Answer: The reaction is reactant-favored. K<1K < 1K<1 means reactants predominate at equilibrium.

Flashcard 28: What is true about the equilibrium constant when a reaction reaches equilibrium?

Answer: The rate of the forward and reverse reactions are equal. At equilibrium, the equilibrium constant value remains constant.

Flashcard 29: For the reaction A⇌BA \rightleftharpoons BA⇌B, if Kc=1K_c = 1Kc​=1, what does this indicate?

Answer: The concentrations of products and reactants are equal. Kc=1K_c = 1Kc​=1 means equal concentrations of A and B at equilibrium.

Flashcard 30: State how KcK_cKc​ is affected by a change in concentration.

Answer: KcK_cKc​ is unaffected. Equilibrium constant is independent of concentration changes.