14. The reaction 2 H2(g) + 2 NO(g) ® N2(g) + 2 H2O(g) is proposed to...
14. The reaction 2 H2(g) + 2 NO(g) ® N2(g) + 2 H2O(g) is proposed to have the alternate mechanism:
2 NO(g) ® N2O2(g) FAST
N2O2(g) + H2(g) ® N2O(g) + H2O(g) SLOW
N2O(g) + H2(g) ® N2(g) + H2O(g) FAST
If the rate law is found to be Rate = k[H2][NO]2, could this support the proposed mechanism? Does the rate law indicate that the reaction is termolecular?
Homework Answers
Ans :
The rate law for the reaction is given by the slowest step of reaction mechanism. Here the slowest step is the second step of the reaction , where N2O2 and H2 are the reactants. Since N2O2 is the intermediate that is formed in the step 1 of the reaction , so it will be replaced by NO.
So the rate law will be : Rate = k[H2] [NO]2
This rate law correctly supports the proposed mechanism.
The order of H2 in the rate law is 1 and that of NO is 2 , so the overall order of reaction = 1 + 2 = 3. This indicates that the reaction is termolecular.
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14. The reaction 2 H2(g) + 2 NO(g) ®
N2(g) + 2 H2O(g) is proposed to...
QUESTION 9 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1:...
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QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1:...
QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) →...
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
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The experimental rate law for the reaction 2H2(g) + 2 NO(g) → N2(g) +2 H2O(g) is d[N2) = kods[Hz][NO] Below is a proposed mechanism: H2(g) + NO(g) + NO(g) = N2O(g) + H2O(g) H2(g) + N2O(g) = N2(g) + H2O(g) ki k2 (a) Under what conditions does this mechanism give the observed rate law? Express kobs in terms of the rate constants for the individual steps of the mechanism. A second proposed mechanism is: NO(g) + NO(g) = N2O2(g) N2O2(g)...
Please answer each part with work shown. Thank you. 6. The following three mechanisms have been proposed for a particular reaction. Mechanism II Mechanism III Mechanisml H2 +NO-H2O+N (slow) N +...
Please answer each part with work shown. Thank you.
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1)
2)
3)
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8. Consider the following reaction where nitrogen monoxide reacts with hydrogen gas to create nitrogen gas...
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Please answer each part with work shown. Thank you.
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2)
3)
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