What would happen to the rate of a reaction with rate law rate = k [NO]2[H2] if the concentration of NO were doubled?A.The rate would be four times larger.B.The rate would be halved.C.The rate would not change.D.The rate would also be doubled.

For a reaction with rate equation Rate = k[A][B][C]², how would the rate change if the concentration of reactant C is doubled while the concentrations of reactants A and B remain unchanged?Select one:a.The rate would be halved.b.The rate would quadruple.c.The rate would double.d.The rate would remain unchanged.

A reaction has the rate law:Rate = k[NO] 2 [H 2 ].If [NO] and [H 2 ] are both increased by a factor of 3, what will be the observed changein the rate?

For the following reaction…BrO3–  +  5Br–  +  6H+  →  3 Br2  +  3H2OThe rate law is…Rate = k[BrO3–][Br–][H+]2What will happen to the rate of the reaction if the H+   concentration is doubled?Group of answer choicesrate will decreaserate will remain unchangedrate will quadruplerate will double

If the reaction studied in this experiment was first order with respect to the concentration of H2O2, what would happen to the rate of the reaction if the concentration of H2O2 was doubled?Question 3Select one:The rate would not change. The rate would be doubled. The rate would be tripled.The rate would increase by a factor of 4.The rate would increase by a factor of 8.

For a reaction of type A + B → products, it is observed that doubling concentration of Acauses the reaction rate to be four times, but doubling amount of B does not affect the rate.What will be the rate equation?