Recall that the rate law only focuses on the reactant concentrations and has a general form of:
k = rate constant
A & B = reactants
x & y = reactant orders
The experimentally determined rate law for the reaction 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) is Rate = k[NO]2[H2].
If the concentration of H2 is doubled, will the reaction rate quadruple, double, or remain the same?
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