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Chapter 2: Problem 10

\(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)\) 2.0 mol of \(\mathrm{CO}(g)\) and 2.0 mol of \(\mathrm{O}_{2}(g)\) are pumped into a rigid, evacuated \(4.0-\mathrm{L}\) container, where they react to form \(\mathrm{CO}_{2}(g) .\) Which of the following values does NOT represent a potential set of concentrations for each gas at a given point during the reaction? (A) 0.5 0.5 0 (B) 0 0.25 0.5 (C) 0.25 0.25 0.5 (D) 0.25 0.38 0.25

Short Answer

Expert verified
The set of concentrations that does not represent a potential set during the reaction is (D) 0.25 0.38 0.25.

Step by step solution

01

Analyzing the Chemical Reaction

From the chemical equation \(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)\), for every 2 moles of CO (Carbon Monoxide), 1 mole of O2 (Oxygen) is used to give 2 moles of CO2 (Carbon Dioxide). The total number of moles initially is 4.0 moles (2.0 moles of CO and 2.0 moles of O2) within a 4.0 L volume. Therefore, the initial concentration for each reactant is 0.5 M.
02

Checking Option A

In option A, the concentrations are 0.5M for CO, 0.5M for O2, and 0 for CO2. This could be an initial moment when the reaction has just started, but no CO2 gas has been produced yet. So this set of concentrations can occur.
03

Checking Option B

In option B, the concentrations are 0M for CO, 0.25M for O2, and 0.5M for CO2. Considering the reaction, when all CO gas has reacted, it must have formed 0.5M of CO2 gas and used up 0.25M of O2 gas. This leaves no CO, 0.25M of O2 and 0.5M of CO2. So this set of concentrations is also possible.
04

Checking Option C

In option C, the concentrations are 0.25M for CO, 0.25M for O2, and 0.5M for CO2. Here, half of the original CO has reacted, using up half the original O2, and formed 0.5M of CO2 gas. This matches the stoichiometry of the reaction, so this is another potential set of concentrations.
05

Checking Option D

In option D, the concentrations are 0.25M for CO, 0.38M for O2, and 0.25M for CO2. Half of the original CO has reacted, but the concentration of O2 left is not 0.25M as the reaction ratios demand. Instead, it's more (0.38M). This suggests that not enough O2 has reacted to form CO2, which means this set of concentrations does not represent a valid point during the reaction.

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Most popular questions from this chapter

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