The progress of reaction, A leftharpoons n B with time, is represented in fig. use given below. Determine (i) the value of n (ii) the equilibrium constant, K and (iii) the initial rate of conversion of A.

Question

The progress of reaction, A leftharpoons n B with time, is represented in fig. use given below. Determine (i) the value of n (ii) the equilibrium constant, K and (iii) the initial rate of conversion of A. (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Observing the graph indicates that when 0.20 mole of A is reacted. 0.40 mole o f product is formed. <img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/38d95c50ee0c9f676157f15a0e81c97e-.png" /> At equilibrium. [ A ]=0.30 M .[ B ]=0.60 M Kp=([B]2/[A])=(0.36/0.30)=1.2

Q. The progress of reaction, $A ⇌ n B$
with time, is represented in fig. use given below.
Determine (i) the value of $n$
(ii) the equilibrium constant, $K$ and
(iii) the initial rate of conversion of $A$ .

Observing the graph indicates that when $0.20$ mole of $A$ is reacted. $0.40$ mole o f product is formed.

At equilibrium. $[A] = 0.30 M . [B] = 0.60 M$
$K_{p} = \frac{[ B ] ^{2}}{[ A ]} = \frac{0.36}{0.30} = 1.2$

Q. The progress of reaction, A⇌nB with time, is represented in fig. use given below. Determine (i) the value of n (ii) the equilibrium constant, K and (iii) the initial rate of conversion of A.

Observing the graph indicates that when 0.20 mole of A is reacted. 0.40 mole o f product is formed. At equilibrium. [A]=0.30M.[B]=0.60M Kp​=[A][B]2​=0.300.36​=1.2

Q. The progress of reaction, $A ⇌ n B$
with time, is represented in fig. use given below.
Determine (i) the value of $n$
(ii) the equilibrium constant, $K$ and
(iii) the initial rate of conversion of $A$ .

Observing the graph indicates that when $0.20$ mole of $A$ is reacted. $0.40$ mole o f product is formed.

At equilibrium. $[A] = 0.30 M . [B] = 0.60 M$
$K_{p} = \frac{[ B ] ^{2}}{[ A ]} = \frac{0.36}{0.30} = 1.2$