Recall that the rate law only focuses on the reactant concentrations and has a general form of:
$\overline{){\mathbf{rate}}{\mathbf{}}{\mathbf{law}}{\mathbf{=}}{\mathbf{k}}{\left[\mathbf{A}\right]}^{{\mathbf{x}}}{\left[\mathbf{B}\right]}^{{\mathbf{y}}}}$
Calculate the order of the reaction with respect to NO.
[NO] (M) | 0.30 | 0.60 | 0.60 |
[H_{2}] (M) | 0.35 | 0.35 | 0.70 |
Rate (mol/L·s) | 2.835x10^{-3} | 1.134x10^{-2} | 2.268x10^{-2} |
Calculate order with respect to NO:
Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation:
H_{2 (g)} + 2NO_{(g)} ⟶ N_{2}O_{(g)} + H_{2}O_{(g)}
Determine the rate equation, the rate constant, and the orders with respect to each reactant from the following data:
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