Nitrogen monoxide reacts with hydrogen as follows: 2NO(g)+ H2(g) N2O(g) + H2O(g) The rate law is [H2]/ t
2NO(g)+ H2(g) → N2O(g) + H2O(g)
The rate law is Δ[H2]/ Δt = k[NO]2[H2], where k is 1.10 × 107 L2/(mol2∙s) at 826oC. A vessel contains NO and H2 at 826oC. The partial pressures of NO and H2 are 144 mmHg and 324 mmHg, respectively. What is the rate of decrease of partial pressure of NO? See Problem 13.145.
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Chapter # 13- Rates of Reaction
Section: Review Questions
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Question Posted: March 01, 2016 04:32:00