A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O 3 (g) + NO (g) ⟶ O 2 (g) + NO 2 (g) The rate law for this reaction is rate of reaction = k [ O 3 ] [ NO ] Given that k = 2.55 * 10 6 M - 1 ⋅ s - 1 at a certain temperature, calculate the initial reaction rate when [ O 3 ] and [ NO ] remain essentially constant at the values [ O 3 ] 0 = 7.34 * 10 - 6 M and [ NO ] 0 = 6.99 * 10 - 5 M, owing to continuous production from separate sources.

Question

Tommy Greene

Chemistry

29 December, 04:04

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O 3 (g) + NO (g) ⟶ O 2 (g) + NO 2 (g) The rate law for this reaction is rate of reaction = k [ O 3 ] [ NO ] Given that k = 2.55 * 10 6 M - 1 ⋅ s - 1 at a certain temperature, calculate the initial reaction rate when [ O 3 ] and [ NO ] remain essentially constant at the values [ O 3 ] 0 = 7.34 * 10 - 6 M and [ NO ] 0 = 6.99 * 10 - 5 M, owing to continuous production from separate sources.

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Answers (1)

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Kayden Glass · Answer 1

1.31 * 10⁻¹⁵ M/s

Explanation:

Let's consider the following reaction.

O₃ (g) + NO (g) ⟶ O₂ (g) + NO₂ (g)

The rate law is:

rate = 2.55 * 10⁻⁶ M⁻¹s⁻¹ [O₃].[NO]

where,

2.55 * 10⁻⁶ M⁻¹s⁻¹ is the rate constant (k)

[O₃] is the concentration of O₃ raised to the reaction order 1

[NO] is the concentration of NO raised to the reaction order 1

When [O₃] = 7.34 * 10⁻⁶ M and [NO] = 6.99 * 10⁻⁵ M, the rate of the reaction is:

rate = 2.55 * 10⁻⁶ M⁻¹s⁻¹ (7.34 * 10⁻⁶ M). (6.99 * 10⁻⁵ M) = 1.31 * 10⁻¹⁵ M/s