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Chapter 1: Problem 8

$$2 \mathrm{NOCl} \rightarrow 2 \mathrm{NO}+\mathrm{Cl}_{2}$$ The reaction above takes place with all of the reactants and products in the gaseous phase. Which of the following is true of the relative rates of disappearance of the reactants and appearance of the products? (A) NO appears at twice the rate that NOCl disappears. (B) NO appears at the same rate that NOCl disappears. (C) NO appears at half the rate that NOCl disappears. (D) \(\mathrm{Cl}_{2}\) appears at the same rate that NOCl disappears.

Short Answer

Expert verified
The correct answer is B. NO appears at the same rate that NOCl disappears.

Step by step solution

01

Analyze the stoichiometry of the reaction

The stoichiometric coefficients in the provided chemical reaction are 2 for NOCl and NO, and 1 for Cl2. This means that for every 2 moles of NOCl that disappears, 2 moles of NO appear and 1 mole of Cl2 appears.
02

Relate the disappearance and appearance rates

Based on the stoichiometry, the disappearance rate of NOCl equates to the appearance rate of NO. As such, every mole of NOCl that vanishes would result in the appearanc of one mole of NO. On the other hand, the appearance rate of Cl2 would be half the disappearance rate of NOCl.
03

Determine the correct answer

Reviewing the options, Option A states that NO appears at twice the rate NOCl disappears, which contradicts our analysis. Option B suggests NO appears at the same rate that NOCl disappears, which matches our reasoning. Option C and D also contradict the analysis. Therefore, option B is the correct answer.

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