Rate Law from Initial Rates: NO Reacting with Ozone

Question

For NO(g) + O₃(g) \to NO₂(g) + O₂(g), use the following laboratory initial-rate data at 25 °C to determine the rate law and rate constant. The measured rate is the formation rate of NO₂ in mol L⁻¹ s⁻¹. Trial [NO] (mol/L) [O₃] (mol/L) Initial rate (mol L⁻¹ s⁻¹) 1 1.00 \times 10⁻⁶ 3.00 \times 10⁻⁶ 6.60 \times 10⁻⁵ 2 1.00 \times 10⁻⁶ 6.00 \times 10⁻⁶ 1.32 \times 10⁻⁴ 3 1.00 \times 10⁻⁶ 9.00 \times 10⁻⁶ 1.98 \times 10⁻⁴ 4 2.00 \times 10⁻⁶ 9.00 \times 10⁻⁶ 3.96 \times 10⁻⁴ 5 3.00 \times 10⁻⁶ 9.00 \times 10⁻⁶ 5.94 \times 10⁻⁴

Trial	[NO] (mol/L)	[O₃] (mol/L)	Initial rate (mol L⁻¹ s⁻¹)
1	1.00 × 10⁻⁶	3.00 × 10⁻⁶	6.60 × 10⁻⁵
2	1.00 × 10⁻⁶	6.00 × 10⁻⁶	1.32 × 10⁻⁴
3	1.00 × 10⁻⁶	9.00 × 10⁻⁶	1.98 × 10⁻⁴
4	2.00 × 10⁻⁶	9.00 × 10⁻⁶	3.96 × 10⁻⁴
5	3.00 × 10⁻⁶	9.00 × 10⁻⁶	5.94 × 10⁻⁴

Explore the full answer and supporting references to better understand this question.

Verla BasicBest value

$19.99/month

Study Pass

$0.99/month

The rate is the measured NO₂ formation rate in OpenStax Example 12.4 at 25 °C. The fitted law applies to the supplied experimental conditions. The reaction orders come from the rate comparisons, rather than an assumption that equation coefficients determine the exponents.