What would happen to the rate of a reaction with rate law kNO2H2 if the concentration of H2 were halved?

In the rate law ( \text{Rate} = k[\text{NO}_2][\text{H}_2] ), the rate of the reaction is directly proportional to the concentration of both reactants. If the concentration of ( \text{H}_2 ) is halved, the rate of the reaction would also decrease by half, assuming the concentration of ( \text{NO}_2 ) remains constant. This is because the rate depends on the product of the concentrations of the reactants, so any reduction in ( [\text{H}_2] ) directly affects the overall reaction rate.