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When the rate of disappearance of O2 is 0.28 M s1, the rate of appearance of CO2 is s-1 M

When the rate of disappearance of O2 is 0.28 M s1, the rate of appearance of CO2 is s-1 M

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Combustion Reaction of Ethylene and Rate of Product Formation** The combustion of ethylene (C₂H₄) proceeds by the following chemical reaction: \[ \text{C}_2\text{H}_4\text{(g)} + 3 \text{O}_2\text{(g)} \rightarrow 2 \text{CO}_2\text{(g)} + 2 \text{H}_2\text{O(g)} \] --- ### Problem Statement: When the rate of disappearance of \(\text{O}_2\) is \(0.28 \, \text{M s}^{-1}\), calculate the rate of appearance of \(\text{CO}_2\) in \(\text{M s}^{-1}\). ### Answer Choices: - \( \mathbf{0.42} \) - \( \mathbf{0.19} \) - \( \mathbf{0.56} \) - \( \mathbf{0.093} \) - \( \mathbf{0.84} \) ### Explanation: To solve this problem, we need to use the stoichiometric relationship between \(\text{O}_2\) and \(\text{CO}_2\) based on the given balanced chemical equation. From the equation: \[ \text{C}_2\text{H}_4\text{(g)} + 3 \text{O}_2\text{(g)} \rightarrow 2 \text{CO}_2\text{(g)} + 2 \text{H}_2\text{O(g)} \] We see that 3 moles of \(\text{O}_2\) yield 2 moles of \(\text{CO}_2\). To find the rate of appearance of \(\text{CO}_2\) from the rate of disappearance of \(\text{O}_2\), we use the stoichiometric ratio: \[ \text{Rate of disappearance of O}_2 : 3 = \text{Rate of appearance of CO}_2 : 2 \] Given that the rate of disappearance of \(\text{O}_2\) is \(0.28 \, \text{M s}^{-1}\), we can set up the following proportion: \[ \frac{0.28}{3} = \frac{\text{Rate of
Transcribed Image Text:**Combustion Reaction of Ethylene and Rate of Product Formation** The combustion of ethylene (C₂H₄) proceeds by the following chemical reaction: \[ \text{C}_2\text{H}_4\text{(g)} + 3 \text{O}_2\text{(g)} \rightarrow 2 \text{CO}_2\text{(g)} + 2 \text{H}_2\text{O(g)} \] --- ### Problem Statement: When the rate of disappearance of \(\text{O}_2\) is \(0.28 \, \text{M s}^{-1}\), calculate the rate of appearance of \(\text{CO}_2\) in \(\text{M s}^{-1}\). ### Answer Choices: - \( \mathbf{0.42} \) - \( \mathbf{0.19} \) - \( \mathbf{0.56} \) - \( \mathbf{0.093} \) - \( \mathbf{0.84} \) ### Explanation: To solve this problem, we need to use the stoichiometric relationship between \(\text{O}_2\) and \(\text{CO}_2\) based on the given balanced chemical equation. From the equation: \[ \text{C}_2\text{H}_4\text{(g)} + 3 \text{O}_2\text{(g)} \rightarrow 2 \text{CO}_2\text{(g)} + 2 \text{H}_2\text{O(g)} \] We see that 3 moles of \(\text{O}_2\) yield 2 moles of \(\text{CO}_2\). To find the rate of appearance of \(\text{CO}_2\) from the rate of disappearance of \(\text{O}_2\), we use the stoichiometric ratio: \[ \text{Rate of disappearance of O}_2 : 3 = \text{Rate of appearance of CO}_2 : 2 \] Given that the rate of disappearance of \(\text{O}_2\) is \(0.28 \, \text{M s}^{-1}\), we can set up the following proportion: \[ \frac{0.28}{3} = \frac{\text{Rate of
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