Question

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.

Answer 1

Answer:

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