The reaction 2 NO(g)+2 H2( g) ⟶N2( g)+2 H2 O(g) is found to be first-order in H2( g) . Which rat

step 1 We know that the reaction is going to be first order in hydrogen. So it's going to be H2 to the

The reaction 2 NO(g)+2 H2( g) ⟶N2( g)+2 H2 O(g) is found to...

The reaction $$ 2 \mathrm{NO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) $$ is found to be first-order in $\mathrm{H}_{2}(\mathrm{~g}) .$ Which rate equation cannot be correct? (a) Rate $=k[\mathrm{NO}]^{2}\left[\mathrm{H}_{2}\right]$ (b) Rate $=k\left[\mathrm{H}_{2}\right]$ $$ \text { (c) Rate }=k\left[\mathrm{NOl}^{2}\left[\mathrm{H}_{3}\right]^{2}\right. $$

The reaction
$$
2 \mathrm{NO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})
$$
is found to be first-order in $\mathrm{H}_{2}(\mathrm{~g}) .$ Which rate equation cannot be correct?
(a) Rate $=k[\mathrm{NO}]^{2}\left[\mathrm{H}_{2}\right]$
(b) Rate $=k\left[\mathrm{H}_{2}\right]$
$$
\text { (c) Rate }=k\left[\mathrm{NOl}^{2}\left[\mathrm{H}_{3}\right]^{2}\right.
$$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Rate Law

A rate law is an equation that relates the rate of a chemical reaction to the concentrations of its reactants, typically expressed with a constant multiplied by each reactant concentration raised to a power. This law is determined experimentally and does not necessarily mirror the stoichiometry of the overall reaction.

Reaction Order

The reaction order with respect to a given reactant is the exponent on its concentration term in the rate law. The overall reaction order is the sum of these exponents, and it indicates how the rate of the reaction changes as the concentration of the reactants changes.

Experimental Determination of Reaction Order

Determining the order of a reaction with respect to each reactant involves varying the reactant concentrations and measuring the effect on the reaction rate. This process allows scientists to assign an order that might differ from the reaction's stoichiometric coefficients, ensuring consistency with observed kinetic behavior.

Consistency of Rate Equation with Experimental Order

Any proposed rate equation must reflect the experimentally determined orders for each reactant. In this problem, since the reaction is found to be first order in H2, the correct rate law must include H2 raised to the power of one, making any rate equation that does not conform to this requirement incorrect.

Transcript

Please give Ace some feedback