(Solved): Consider the following reaction: 2NO(g)+2H2(g)N2(g)+2H2O(g) (a) The rate law for th ...

Consider the following reaction: $2\mathrm{NO}(\mathrm{g})+2{\mathrm{H}}_2(\mathrm{g})?{\mathrm{N}}_2(\mathrm{g})+2{\mathrm{H}}_2\mathrm{O}(\mathrm{g})$ (a) The rate law for this reaction is second order in $\mathrm{NO}(\mathrm{g})$ and first order in ${\mathrm{H}}_2(\mathrm{g})$. What is the rate law for this reaction? $\begin{array}{l}\text{ Rate }=\mathrm{k}[\mathrm{NO}(\mathrm{g})]\left[{\mathrm{H}}_2(\mathrm{g})\right]\\ \text{ Rate }=\mathrm{k}[\mathrm{NO}(\mathrm{g}){]}^2\left[{\mathrm{H}}_2(\mathrm{g})\right]\\ \text{ Rate }=\mathrm{k}[\mathrm{NO}(\mathrm{g})]{\left[{\mathrm{H}}_2(\mathrm{g})\right]}^2\\ \text{ Rate }=\mathrm{k}[\mathrm{NO}(\mathrm{g}){]}^2{\left[{\mathrm{H}}_2(\mathrm{g})\right]}^2\\ \text{ Rate }=\mathrm{k}[\mathrm{NO}(\mathrm{g})]{\left[{\mathrm{H}}_2(\mathrm{g})\right]}^3\\ \text{ Rate }=\mathrm{k}[\mathrm{NO}(\mathrm{g}){]}^4\left[{\mathrm{H}}_2(\mathrm{g})\right]\end{array}$ (b) If the rate constant for this reaction at a certain temperature is 95200 , what is the reaction rate when $[\mathrm{NO}(\mathrm{g})]=0.0970\mathrm{M}$ and $\left[{\mathrm{H}}_2(\mathrm{g})\right]=$ $0.150M$ ? $\text{ Rate }=M/\mathrm{s}$ (c) What is the reaction rate when the concentration of $\mathrm{NO}(\mathrm{g}$ ) is doubled, to $0.194M$ while the concentration of ${\mathrm{H}}_2$ (g) is $0.150\mathrm{M}$ ? $\text{ Rate }=\mathrm{M}/\mathrm{s}$