Chapter 13, Problem 13.152QP

Nitrogen monoxide reacts with hydrogen as follows:

$2\text{NO}(g)+{\text{H}}_2(g)\stackrel{}{\to }{\text{N}}_2\text{O}(g)+{\text{H}}_2\text{O}(g)$

The rate law is −Δ[H₂]/Δt = k[NO]²[H₂], where k is 1.10 × 10⁻⁷ L²/(mol² · s) at 826°C. A vessel contains NO and H₂ at 826°C. The partial pressures of NO and H₂ are 144 mmHg and 315 mmHg, respectively. What is the rate of decrease of partial pressure of NO? See Problem 13.151.