What is the rate law for the reaction of NO and H2?

Context: Chemistry
Thread starter i_love_science
Start date Mar 3, 2021
Tags

Law Rate Reaction

Click For Summary

SUMMARY

The discussion centers on determining the rate law for the reaction between nitric oxide (NO) and hydrogen (H2). Participants express concerns about potential misprints in the homework statement and solution provided. The consensus is that clarity in the question is essential for accurate interpretation and calculation of the rate law. Participants emphasize the importance of verifying the stoichiometry and reaction order based on experimental data.

PREREQUISITES

Understanding of chemical kinetics
Familiarity with rate laws and reaction orders
Knowledge of stoichiometry in chemical reactions
Experience with interpreting experimental data

NEXT STEPS

Research the derivation of rate laws for elementary reactions
Study the impact of reaction order on rate constants
Explore methods for determining rate laws experimentally
Learn about common pitfalls in interpreting chemical reaction data

USEFUL FOR

Chemistry students, educators, and researchers interested in chemical kinetics and reaction mechanisms.

Mar 3, 2021

i_love_science

Homework Statement: Determine the rate law for this reaction given the data below.

2 NO + 2 H2 -> N2 + 2H2O

Reaction 1:
Initial [NO] = 0.20
Initial [H2] = 0.15
Initial rate = 2.0 * 10^(-4)

Reaction 2:
Initial [NO] = 0.40
Initial [H2] = 0.15
Initial rate = 8.0 * 10^(-4)

Reaction 3:
Initial [NO] = 0.40
Initial [H2] = 0.30
Initial rate = 1.6 * 10^(-3)

I think the rate law is rate = k[NO][SUP]2[/SUP][H2], since when you double the NO concentration, you quadruple the rate.

The solution is rate = k[NO][H2]. Is this wrong? Thanks.