Ammonia is manufactured in large amounts by the reaction
N₂(g) + 3 H₂(g) → 2 NH₃(g)
(a) How is the rate of consumption of H₂ related to the rate of consumption of N₂?

검증된 단계별 안내

Step 1: Understand the reaction. The balanced chemical equation given is N₂(g) + 3 H₂(g) → 2 NH₃(g). This tells us that one molecule of nitrogen reacts with three molecules of hydrogen to form two molecules of ammonia.

Step 2: Understand the concept of reaction rate. The rate of a reaction is the speed at which reactants are consumed or products are formed. It is usually expressed in terms of change in concentration of a reactant or product per unit time.

Step 3: Relate the rate of consumption of reactants. The stoichiometry of the reaction tells us that for every one molecule of N₂ that reacts, three molecules of H₂ are consumed. Therefore, the rate of consumption of H₂ is three times the rate of consumption of N₂.

Step 4: Express the relationship mathematically. If we denote the rate of consumption of N₂ as -d[N₂]/dt and the rate of consumption of H₂ as -d[H₂]/dt, then according to the stoichiometry of the reaction, -d[H₂]/dt = 3(-d[N₂]/dt).

Step 5: Interpret the result. This means that for every unit of time, the amount of H₂ consumed is three times the amount of N₂ consumed.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. In the given reaction, the coefficients indicate that one mole of nitrogen (N₂) reacts with three moles of hydrogen (H₂) to produce two moles of ammonia (NH₃). This relationship allows us to determine how the consumption rates of the reactants are related.

Reaction Rates

The rate of a chemical reaction refers to the speed at which reactants are converted into products. It can be expressed in terms of the change in concentration of a reactant or product over time. In this case, understanding how the rate of consumption of H₂ relates to N₂ involves applying the stoichiometric coefficients to express their rates in a proportional manner.

Rate Law

The rate law is an equation that relates the rate of a reaction to the concentration of its reactants. While the question focuses on stoichiometric relationships, knowing that the rate of consumption of H₂ is three times that of N₂ (due to the coefficients in the balanced equation) is essential for understanding how changes in concentration affect the overall reaction rate.

Ammonia is manufactured in large amounts by the reactionN2(g) + 3 H2(g) → 2 NH3(g)(a) How is the rate of consumption of H2 related to the rate of consumption of N2?