We're being asked to determine the rate law for the following reaction:
2 H2(g) + 2 NO(g) → 2 H2O(g) + N2(g)
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
2H2(g) + 2NO(g) → 2H2O(g) + N2(g)
is known to be first-order in H2 and second-order in NO at a particular temperature.
What is the rate law?
A) Rate = k[H2]2[NO]2
B) Rate = k[H2][NO]2
C) Rate = k[H2][NO]
D) Rate = k[H2O]2[N2]
E) Rate = k[H2]2[NO]