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13 Dec 2019

At temperatures below 500 K, the reaction between carbon monoxide and nitrogen dioxide
CO (g) + NO2 (g) ? CO2 (g) + NO (g)
has the following rate equation: Rate = k[NO2]2. Which of the three mechanisms suggested here agrees with the experimentally observed rate equation?
Mechanism 1: Step 1 Slow NO2 + NO2 ? NO3 + NO
Step 2 Fast NO3 + CO ? NO2 + CO2
Mechanism 2: Step 1 Fast NO2 + NO2 ? N2O3 + O
Step 2 Slow N2O3 + O + CO ? CO2 + NO2 + NO
Mechanism 3: CO + NO2 ? CO2 + NO

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Patrina Schowalter
Patrina SchowalterLv2
17 Dec 2019

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Related questions

In the lower troposphere, ozone is one of the components ofphotochemical smog. It is generated in air when nitrogen dioxide,formed by the oxidation of nitrogen monoxide from car exhaust,reacts by the following mechanism.
(1) NO2(g) NO(g) + O(g)
(2) O(g) + O2(g) O3(g)
Assuming the rate of formation of atomic oxygen in step 1 equalsthe rate of its consumption in step 2, use the data below tocalculate the following quantities.
k1 = 8.0 10-3 s-1; [NO2] = 4.0 10-9 M
k2 = 1.0 106 L/mol

In the lower troposphere, ozone is one of the components ofphotochemical smog. It is generated in air when nitrogen dioxide,formed by the oxidation of nitrogen monoxide from car exhaust,reacts by the following mechanism.
(1) NO2(g) NO(g) + O(g)
(2) O(g) + O2(g) O3(g)
Assuming the rate of formation of atomic oxygen in step 1 equalsthe rate of its consumption in step 2, use the data below tocalculate the following quantities.
k1 = 7.0 10-3 s-1; [NO2] = 4.0 10-9 M
k2 = 1.0 106 L/mol

Part A

The reaction between nitrogen dioxide and carbon monoxide is

NO2(g)+CO(g)→NO(g)+CO2(g)

The rate constant at 701 K is measured as 2.57 M−1⋠s−1 and that at 895 K is measured as 567 M−1⋠s−1. The activation energy is 1.5×102 kJ/mol.

Predict the rate constant at 525 K .

Express the rate constant in liters per mole-second to three significant figures.

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