Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + O₂(g) → NO₂ (g) + O (g) k₁ 2 NO (g) + O(g) → NO₂ (g) k₂ Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = &

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**Reaction Mechanism for Nitric Oxide and Oxygen**

Suppose the reaction between nitric oxide (NO) and oxygen (O₂) proceeds by the following mechanism:

| Step | Elementary Reaction                       | Rate Constant |
|------|-------------------------------------------|---------------|
| 1    | NO(g) + O₂(g) → NO₂(g) + O(g)             | k₁            |
| 2    | NO(g) + O(g) → NO₂(g)                     | k₂            |

Assume that \( k_1 \ll k_2 \), meaning the first step is much slower than the second.

**Task 1: Balanced Chemical Equation**

Write the balanced chemical equation for the overall reaction:

\[ \; \]

**Task 2: Rate Law**

Write the experimentally-observable rate law for the overall chemical reaction.

Note: Your answer should not contain the concentrations of any intermediates.

Rate = \( k \; \)
Transcribed Image Text:**Reaction Mechanism for Nitric Oxide and Oxygen** Suppose the reaction between nitric oxide (NO) and oxygen (O₂) proceeds by the following mechanism: | Step | Elementary Reaction | Rate Constant | |------|-------------------------------------------|---------------| | 1 | NO(g) + O₂(g) → NO₂(g) + O(g) | k₁ | | 2 | NO(g) + O(g) → NO₂(g) | k₂ | Assume that \( k_1 \ll k_2 \), meaning the first step is much slower than the second. **Task 1: Balanced Chemical Equation** Write the balanced chemical equation for the overall reaction: \[ \; \] **Task 2: Rate Law** Write the experimentally-observable rate law for the overall chemical reaction. Note: Your answer should not contain the concentrations of any intermediates. Rate = \( k \; \)
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