Consider the following reaction: A + B ? products The rate law for this reaction was found to be: rate = k[A][B]2 (1/1pts) a. What is the reaction order with respect to A? Choose...zero orderfirst ordersecond orderthird order check_circle (1/1pts) b. What is the reaction order with respect to B? Choose...zero orderfirst ordersecond orderthird order check_circle (1/1pts) c. What is the overall order of the reaction? Choose...zero orderfirst ordersecond orderthird order check_circle (1/1pts) d. If the concentration of A is doubled while the concentration of B is kept constant, how will this affect the rate of reaction? Choose...decrease the rate by a factor of twono change to the rateincrease the rate by a factor of twoincrease the rate by a factor of fourincrease the rate by a factor of eight check_circle (1/1pts) e. If the concentration of B is doubled while the concentration of A is kept constant, how will this affect the rate of reaction? Choose...decrease the rate by a factor of twono change to the rateincrease the rate by a factor of twoincrease the rate by a factor of fourincrease the rate by a factor of eight check_circle (1/1pts) f. What do we call k in the rate law expression? What are the units of k for this reaction?