For the reaction: 2 H2 + 2 NO → N2 + 2 H2O the observed rate expression, under some conditions, is: rate = k[H2][NO]2 Which of the following mechanisms are consistent with these data? Select all that are True. step 1 H2 + 2 NO → N2O + H2O (slow) step 2 N2O + H2 → N2 + H2O (fast) step 1 2 H2 + 2 NO → N2 + H2O step 1 NO + NO ⇌ N2O2 (fast) step 2 N2O2 + H2 → N2 + H2O + O (slow) step 3 O + H2 → H2O (fast) step 1 H2 + NO ⇌ H2ON (fast) step 2 H2ON + NO → N2 + H2O2 (slow) step 3 H2O2→ H2O + O (fast) step 4 O + H2 → H2O (fast)

Step 1 H2 + 2 NO → N2O + H2O (slow)

step 2 N2O + H2 → N2 + H2O (fast)

Explanation:

It is known that the slowest step in a reaction is the rate determining step in a sequence of reactions (reaction mechanism).

We have two important pieces of information in the question to guide our decision making process.

The overall reaction equation, and the rate expression. The two;

2 H2 + 2 NO → N2 + 2 H2O and rate = k[H2][NO]2 all support the answer given above.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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