A certain Zero order reaction has rate constant K is 0.025 MS^-1 for disappearance of A . What will be the concentration of A after 15 sec if initial concentration is A is 0.5M.

(A) 2.5 M  (B) 0.5 M (C) 1.5 M  (D) 0.125 M

The rate constant for zero order reaction is 2× 10^-2 Mole L^-1 sec-1. If the concentration of reactant after 25 sec is 0.5M ,the initial concentration must have been ?

(A) 1M (B) 2M (C) 1.5M  (D) 2.5M

Consider a general reaction A--->B follow zero order kinetics.if concentration of A is reduces from 0.1 M to 0.05 M in 10 second then calculate time taken when concentration reduce to 0.025 M.

(A) 2.5 sec  (B) 2 sec (C) 5 sec   (D) 10 sec

For the equilibrium, PCl 5​ (g)⇌PCl 3​ (g)+Cl 2​ (g) at 298K, K=1.8×10 −7 .Calculate ΔG 0 for the reaction (R=8.314JK −1 mol −1 ).

Equilibrium constant for the reaction given below is 2.0 × 10^-7 at 300 K. calculate standard Gibb's free energy change for the reaction PCl5 (g) --=--PCl3 (g) + Cl2 (g) also calculate standard entropy change if ∆H° = 28.40 Kj mole-1.