Chemical Kinetics and Nuclear ChemistryHard

Question

For the second-order reaction A + B → Products, the rate constant k, is given as$k = \frac{2.303}{(a - b)t}\log\frac{b(a - x)}{a(b - x)}$, where, a and b are the initial concentrations of ‘A’ and ‘B’ and x is the change in concentration after time t. If b >> a, the reaction reduces to

Options

A.first-order with respect to ‘A’.
B.zero-order with respect to ‘A’.
C.first-order with respect to ‘B’.
D.overall zero-order.

Solution

$(b - a) \simeq b\text{ and }(b - x) \simeq b$

$\therefore Kt = \frac{2.303}{a - b}.\ln\frac{b(a - x)}{a(b - x)} \simeq \frac{2.303}{( - b)}.\ln\frac{b(a - x)}{ab} \text{Or, }(b.K).t = 2.303.\ln\frac{a}{a - x}$

∴ Reaction becomes first-order with respect to A.

Create a free account to view solution

View Solution Free
Topic: Chemical Kinetics and Nuclear Chemistry·Practice all Chemical Kinetics and Nuclear Chemistry questions

More Chemical Kinetics and Nuclear Chemistry Questions

For hypothetical reaction A → B takes place according to$$A\overset{\quad K_{1}\quad}{\leftleftarrows}C\left( \text{fast...In first order reaction, the concentration of the reactant decreases from 0.8 M to 0.4 M in 15 minutes. The time taken f...For the elementary reaction M → N, the rate of disappearance of M increases by a factor of 8 upon doubling the con...Decomposition of A is a first order reaction at $T(K)$ and is given by $A(g) \rightarrow B(g) + C(g)$. In a closed 1 L v...Identify compound which give fastest dehydration ?...