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.

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 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?

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

the reactant concentration is doubled, what would happenthen to equilibrium constant?(a) Remains constant(b) Be doubled(c) Be halved(d) Cannot be predicted

The reaction rate constant may be defined as the rate of the reaction when theconcentration of each reactants is ___________a) Zerob) Unityc) Doubled the initial concentrationd) Infinite