**Reaction Mechanism and Rate Law Analysis: An Educational Overview**The given reaction: \[ 2 \text{CO}(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) \]is described by the following rate law:\[ \text{rate} = k[\text{CO}]^2[\text{O}_2] \]To determine which of the following mechanisms are consistent with this rate law, consider the step-by-step reaction processes and their respective speeds.**Mechanisms:**(a) \[ \text{CO} + \text{O}_2 \rightarrow \text{CO}_2 + \text{O} \quad (\text{Slow}) \]\[ \text{O} + \text{CO} \rightarrow \text{CO}_2 \quad (\text{Fast}) \](b) \[ \text{CO} + \text{O}_2 \rightarrow \text{CO}_3 \quad (\text{Fast equilibrium}) \]\[ \text{CO}_3 + \text{CO} \rightarrow 2 \text{CO}_2 \quad (\text{Slow}) \](c) \[ 2 \text{CO} \rightarrow \text{C}_2\text{O}_2 \quad (\text{Slow}) \]\[ \text{C}_2\text{O}_2 + \text{O}_2 \rightarrow \text{C}_2\text{O}_4 \quad (\text{Fast}) \]\[ \text{C}_2\text{O}_4 \rightarrow 2 \text{CO}_2 \quad (\text{Fast}) \](d) \[ 2 \text{CO} \rightarrow \text{C}_2\text{O}_2 \quad (\text{Fast equilibrium}) \]\[ \text{C}_2\text{O}_2 \rightarrow \text{CO}_2 + \text{O} \quad (\text{Slow}) \]\[ \text{O} + \text{CO} \rightarrow \text{CO}_2 \quad (\text{Fast}) \]**Analysis:**To determine which mechanism corresponds to the given rate law (\( \text{rate} = k[\text{CO}]^2[\text{O}_2] \)), we need to identify

Given : Rate law of reaction is : Rate = k[CO]2[O2]

The reaction 2 CO(g) + O₂(g) → 2 CO2(g) is described by this rate law: rate = k[CO]²[0₂] Which of the following mechanisms are consistent with this rate law? (Think carefully.) (a) CO+O₂ CO₂ + O Slow O + CO - CO₂ Fast (b) CO+O2CO3 Fast equilibrium CO3 + CO2 CO2 Slow Slow C202 +02 C204 Fast C204-2 CO2 Fast (d) 2 CO→ C₂02 Fast equilibrium (c) 2 CO-C₂02 C₂O2 CO2 + O Slow

The reaction 2 CO(g) + O₂(g) → 2 CO2(g) is described by this rate law: rate = k[CO]²[0₂] Which of the following mechanisms are consistent with this rate law? (Think carefully.) (a) CO+O₂ CO₂ + O Slow O + CO - CO₂ Fast (b) CO+O2CO3 Fast equilibrium CO3 + CO2 CO2 Slow Slow C202 +02 C204 Fast C204-2 CO2 Fast (d) 2 CO→ C₂02 Fast equilibrium (c) 2 CO-C₂02 C₂O2 CO2 + O Slow

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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