For the gaseous reaction 2A + B → C + D,rate = k[A][B]. The volume of the containercontaining the reaction mixture is suddenlyreduced to one fourth of its original volume.New rate with respect to original rate is :

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.

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

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.

3. At constant Pressure what will be the change in temperature when the volume ofa gas will become twice of what it is at 0oC?A. 546oC B. 200oCC. 546 K D. 273 K4. Rate equation for a reaction 2A product is Rate = K [A]2. Unit of specificrate constant for this reaction is:A. mol2dm-6 S-1 B. mol-1dm3 S-1C. moldm-3 D. S-15. A substance which itself is not a catalyst but increases the activity of a catalyst iscalled:A. Enzyme B. inhibitorC. Promoter D. Poisoner

The rate constant of a first order reaction is 4×10−3sec−1 .At a reactant concentration of 0.02 M, the rate of reaction would be: