Consider the first-order reaction: PCl5(g) → PCl3(g) + Cl2(g) In this reaction, the concentration of PCl5 reduces from an initial concentration of 50 mol L-1 to 10 mol L-1 in 120 minutes at 300 K. If the rate constant for the reaction at 300 K is x × 10-2 min-1, find the value of x. [Given: log 5 = 0.6989, ln 10 = 2.303]

Match List I (Order of reaction) with List II (Unit of rate constant): List I: A. Zero order B. First order C. Second order D. Third order List II: I. mol-1 L s-1 II. mol-2 L2 s-1 III. s-1 IV. mol L-1 s-1 Choose the correct matching:

Given below is an expression for the rate constant of a first order reaction occurring at a certain temperature, T (K): ln k = 14.34 - 1.25 × 104T The energy of activation in kcal mol-1 for the reaction is: (Given: k in s-1, R = 1.987 cal mol-1 K-1)