In the reaction shown below, the rate of the reaction ______ if the concentration of A increases.A + B → ABMultiple choice question.increasesdecreasesdoes not change

The rate of the reaction 2A + B2 Rate = k [A] [B2]. →2AB is given by The value of rate constant (k) can be increased by: (A) increasing the concentration of A (B) increasing the concentration of B (C) increasing the temperature (D) all the above three

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.

Which of the following tends to increase the rate of a chemical reaction?A.Decreasing the concentration of the reactantsB.Increasing the temperature of the reaction mixtureC.Increasing the amount of solvent usedD.Using larger particles of solid reactants

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?

The rate constant of the reaction A→B is 0.6×10−3 mole per litre per second. If the concentration of A is 5 M, then concentration of B after 20 minutes is: