This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in $$ \text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3 $$, the coefficients 1, 3, and 2 mean that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia. This ratio is the fundamental relationship—it means for every 3 moles of $\text{H}_2$ consumed, exactly 1 mole of $\text{N}_2$ is consumed and 2 moles of $\text{NH}_3$ are produced. The ratio stays constant no matter how much you scale it: 2 moles of $\text{N}_2$ with 6 moles of $\text{H}_2$ makes 4 moles of $\text{NH}_3$ (doubled), or 0.5 moles of $\text{N}_2$ with 1.5 moles of $\text{H}_2$ makes 1 mole of $\text{NH}_3$ (halved)—the 1:3:2 ratio is preserved! In this equation, the mole ratio of $\text{NH}_3$ to $\text{H}_2$ is extracted from their coefficients: $\text{NH}_3$ has 2 and $\text{H}_2$ has 3, so it's 2:3, meaning 2 moles of $\text{NH}_3$ per 3 moles of $\text{H}_2$. Choice A correctly interprets the coefficients as the mole ratio between $\text{NH}_3$ and $\text{H}_2$, stating 2:3. A distractor like choice B (3:2) might swap the order, but the question specifies $\text{NH}_3$ to $\text{H}_2$, which is 2:3—pay attention to which comes first. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio.

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in $$2H2 + O2 \rightarrow 2H2O$$, the coefficients 2, 1, and 2 mean that 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water. This ratio is the fundamental relationship—it means for every 1 mole of O2 consumed, exactly 2 moles of H2 are consumed and exactly 2 moles of H2O are produced. The ratio stays constant no matter how much you scale it: 4 moles H2 with 2 moles O2 makes 4 moles H2O (doubled), or 1 mole H2 with 0.5 moles O2 makes 1 mole H2O (halved)—the 2:1:2 ratio is preserved! In the given equation $$N2 + 3H2 \rightarrow 2NH3$$, the coefficient for H2 is 3 and for N2 is 1, so per 1 mole of N2, 3 moles of H2 react, directly from the 1:3 ratio of N2 to H2. Choice C correctly interprets the coefficients as the mole ratio between the specified substances. A distractor like choice B might misread the ratio as 2 moles from the product side, but focus on the reactant coefficients and the 'per 1 mole of N2' phrasing to avoid confusing it with the NH3 coefficient. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio—they're not just decorative numbers, they're the mathematical relationship between substances in the reaction!

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in 2H2 + O2 → 2H2O, the coefficients 2, 1, and 2 mean that 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water. This ratio is the fundamental relationship—it means for every 1 mole of O2 consumed, exactly 2 moles of H2 are consumed and exactly 2 moles of H2O are produced. The ratio stays constant no matter how much you scale it: 4 moles H2 with 2 moles O2 makes 4 moles H2O (doubled), or 1 mole H2 with 0.5 moles O2 makes 1 mole H2O (halved)—the 2:1:2 ratio is preserved! In the given equation 2KClO3 → 2KCl + 3O2, the coefficient for KClO3 is 2 and for O2 is 3, so the mole ratio of KClO3 to O2 is 2:3, meaning 2 moles of KClO3 produce 3 moles of O2. Choice B correctly interprets the coefficients as the mole ratio between the specified substances. A distractor like choice A might reverse to 3:2, but always use the order asked—KClO3 to O2 means coefficient of KClO3 first (2) to O2 (3). Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio—they're not just decorative numbers, they're the mathematical relationship between substances in the reaction!

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in CH₄ + 2O₂ → CO₂ + 2H₂O, the coefficients 1, 2, 1, and 2 mean that 1 mole of methane reacts with 2 moles of oxygen gas to produce 1 mole of carbon dioxide and 2 moles of water. From the equation CH₄ + 2O₂ → CO₂ + 2H₂O, the coefficient of CH₄ is 1 (when no number is shown, it's 1) and the coefficient of O₂ is 2, so the ratio is 1:2, meaning 1 mole of CH₄ requires exactly 2 moles of O₂. Choice B correctly states that 2 mol O₂ are required per 1 mol CH₄, directly matching the 1:2 ratio from the coefficients. The other choices suggest incorrect amounts (1 mol, 4 mol) or incorrectly claim the ratio depends on temperature rather than the balanced equation coefficients. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. The beauty of mole ratios is their scalability: if you have 5 moles of CH₄, you need 10 moles of O₂ (5 × 2 = 10), and if you have only 0.5 moles of CH₄, you need 1 mole of O₂ (0.5 × 2 = 1)—the 1:2 ratio always holds!

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in $2\text{Fe} + 3\text{Cl}_2 \rightarrow 2\text{FeCl}_3$, the coefficients 2, 3, and 2 mean that 2 moles of $\text{Fe}$ react with 3 moles of $\text{Cl}_2$ to produce 2 moles of $\text{FeCl}_3$. This ratio is the fundamental relationship—it means for every 2 moles of $\text{Fe}$ consumed, exactly 3 moles of $\text{Cl}_2$ are consumed and 2 moles of $\text{FeCl}_3$ are produced. The ratio stays constant no matter how much you scale it: 4 moles $\text{Fe}$ with 6 moles $\text{Cl}_2$ makes 4 moles $\text{FeCl}_3$ (doubled), or 1 mole $\text{Fe}$ with 1.5 moles $\text{Cl}_2$ makes 1 mole $\text{FeCl}_3$ (halved)—the $2:3:2$ ratio is preserved! In this equation, the mole ratio of $\text{Fe}$ to $\text{Cl}_2$ is extracted from their coefficients: $\text{Fe}$ has 2 and $\text{Cl}_2$ has 3, so it's $2:3$, meaning 2 moles of $\text{Fe}$ per 3 moles of $\text{Cl}_2$. Choice B correctly interprets the coefficients as the mole ratio between $\text{Fe}$ and $\text{Cl}_2$, stating $2:3$. A distractor like choice A ($3:2$) might reverse the substances, but confirm the order: it's $\text{Fe}$ to $\text{Cl}_2$, which is $2:3$, not $3:2$. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio.

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in N₂ + 3H₂ → 2NH₃, the coefficients 1, 3, and 2 mean that 1 mole of nitrogen gas reacts with 3 moles of hydrogen gas to produce 2 moles of ammonia. This ratio is the fundamental relationship—it means for every 1 mole of N₂ consumed, exactly 3 moles of H₂ are consumed and exactly 2 moles of NH₃ are produced. The ratio stays constant no matter how much you scale it: 2 moles N₂ with 6 moles H₂ makes 4 moles NH₃ (doubled), or 0.5 moles N₂ with 1.5 moles H₂ makes 1 mole NH₃ (halved)—the 1:3:2 ratio is preserved! In this equation, the mole ratio of H₂ to N₂ is extracted from their coefficients: H₂ has 3 and N₂ has 1 (implied), so per 1 mole of N₂, 3 moles of H₂ react. Choice C correctly interprets the coefficients by stating 3 mol H₂ react per 1 mol N₂. A distractor like choice B (2 mol H₂) might confuse the product coefficient with the reactant, but remember, we're focusing on reactants here—check the equation sides carefully. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio.

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in $$4 \mathrm{Fe} + 3 \mathrm{O}_2 \rightarrow 2 \mathrm{Fe}_2\mathrm{O}_3$$, the coefficients 4, 3, and 2 mean that 4 moles of iron react with 3 moles of oxygen to produce 2 moles of iron(III) oxide. This ratio is the fundamental relationship—it means for every 4 moles of $\mathrm{Fe}$ consumed, exactly 3 moles of $\mathrm{O}_2$ are consumed and 2 moles of $\mathrm{Fe}_2\mathrm{O}_3$ are produced. The ratio stays constant no matter how much you scale it: 8 moles of $\mathrm{Fe}$ with 6 moles of $\mathrm{O}_2$ makes 4 moles of $\mathrm{Fe}_2\mathrm{O}_3$ (doubled), or 2 moles of $\mathrm{Fe}$ with 1.5 moles of $\mathrm{O}_2$ makes 1 mole of $\mathrm{Fe}_2\mathrm{O}_3$ (halved)—the 4:3:2 ratio is preserved! In this equation, the mole ratio of $\mathrm{Fe}_2\mathrm{O}_3$ to $\mathrm{Fe}$ is extracted from their coefficients: $\mathrm{Fe}_2\mathrm{O}_3$ has 2 and $\mathrm{Fe}$ has 4, so it's 2:4 (or simplified 1:2, but the question uses unsimplified). Choice A correctly interprets the coefficients as the mole ratio between $\mathrm{Fe}_2\mathrm{O}_3$ and $\mathrm{Fe}$, stating 2:4. A distractor like choice B (4:2) reverses the order, but the question asks for $\mathrm{Fe}_2\mathrm{O}_3$ to $\mathrm{Fe}$, which is 2:4—always match the sequence. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio.

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in $2\text{H}_2\text{O}_2 \rightarrow 2\text{H}_2\text{O} + \text{O}_2$, the coefficients 2, 2, and 1 mean that 2 moles of hydrogen peroxide decompose to produce 2 moles of water and 1 mole of oxygen. This ratio is the fundamental relationship—it means for every 2 moles of $\text{H}_2\text{O}_2$ decomposed, exactly 2 moles of $\text{H}_2\text{O}$ and 1 mole of $\text{O}_2$ are produced. The ratio stays constant no matter how much you scale it: 4 moles $\text{H}_2\text{O}_2$ makes 4 moles $\text{H}_2\text{O}$ and 2 moles $\text{O}_2$ (doubled), or 1 mole $\text{H}_2\text{O}_2$ makes 1 mole $\text{H}_2\text{O}$ and 0.5 moles $\text{O}_2$ (halved)—the 2:2:1 ratio is preserved! In this equation, the mole ratio of $\text{H}_2\text{O}$ to $\text{O}_2$ is extracted from their coefficients: $\text{H}_2\text{O}$ has 2 and $\text{O}_2$ has 1 (implied), so it's 2:1, meaning 2 moles of $\text{H}_2\text{O}$ per 1 mole of $\text{O}_2$. Choice A correctly interprets the coefficients as the mole ratio between $\text{H}_2\text{O}$ and $\text{O}_2$, stating 2:1. A distractor like choice B (1:2) could result from swapping the order, but always state the ratio as asked—$\text{H}_2\text{O}$ to $\text{O}_2$ is 2:1, not reversed. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio.

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in $2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}$, the coefficients 2, 1, and 2 mean that $2$ moles of $\text{H}_2$ react with $1$ mole of $\text{O}_2$ to produce $2$ moles of $\text{H}_2\text{O}$. This ratio is the fundamental relationship—it means for every $1$ mole of $\text{O}_2$ consumed, exactly $2$ moles of $\text{H}_2$ are consumed and exactly $2$ moles of $\text{H}_2\text{O}$ are produced. The ratio stays constant no matter how much you scale it: $4$ moles of $\text{H}_2$ with $2$ moles of $\text{O}_2$ makes $4$ moles of $\text{H}_2\text{O}$ (doubled), or $1$ mole of $\text{H}_2$ with $0.5$ moles of $\text{O}_2$ makes $1$ mole of $\text{H}_2\text{O}$ (halved)—the $2:1:2$ ratio is preserved! In this equation, the mole relationship between $\text{O}_2$ and $\text{H}_2\text{O}$ is that $1$ mole of $\text{O}_2$ produces $2$ moles of $\text{H}_2\text{O}$, as their coefficients are 1 and 2. Choice C correctly interprets the coefficients by stating 1 mol $\text{O}_2$ produces 2 mol $\text{H}_2\text{O}$. A distractor like choice A (1 mol $\text{O}_2$ produces 1 mol $\text{H}_2\text{O}$) might ignore the coefficients, but remember, the numbers show the proportion—$\text{O}_2$'s 1 to $\text{H}_2\text{O}$'s 2 means twice as much water is produced. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio.

This question tests your understanding that coefficients in balanced chemical equations represent mole ratios—the proportional relationships between amounts of reactants consumed and products formed in a chemical reaction. The coefficients in a balanced equation (the numbers in front of chemical formulas) tell you the ratio of MOLES of each substance involved in the reaction: in 2H₂O₂ → 2H₂O + O₂, the coefficients 2, 2, and 1 mean that 2 moles of hydrogen peroxide decompose to produce 2 moles of water and 1 mole of oxygen. This ratio is the fundamental relationship—it means for every 2 moles of H₂O₂ decomposed, exactly 1 mole of O₂ is produced (along with 2 moles of H₂O). The ratio stays constant no matter how much you scale it: 4 moles H₂O₂ makes 4 moles H₂O and 2 moles O₂ (doubled), or 1 mole H₂O₂ makes 1 mole H₂O and 0.5 moles O₂ (halved)—the 2:2:1 ratio is preserved! In this equation, the comparison of moles of H₂O₂ reacted to moles of O₂ formed is that 2 moles of H₂O₂ form 1 mole of O₂, based on coefficients 2 and 1. Choice C correctly interprets the coefficients by stating 2 mol H₂O₂ form 1 mol O₂. A distractor like choice A (2 mol H₂O₂ form 2 mol O₂) might confuse O₂ with H₂O's coefficient, but O₂ has a 1—always verify the specific substance. Reading mole ratios from balanced equations: (1) Locate the two substances you're comparing in the equation. (2) Read their coefficients (the numbers in front—if no number is written, the coefficient is 1). (3) Write the ratio: [coefficient of first substance] : [coefficient of second substance]. Using mole ratios as conversion factors: mole ratios let you predict amounts! If you know how many moles of one substance you have, you can calculate moles of another using the ratio.