Chemical and Ionic Equilibrium - Result Question 46
46. The progress of reaction,
$ A \rightleftharpoons 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 $A$.
$(1994,3 M)$
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Answer:
Correct Answer: 46. $(1, 2)$
Solution:
- Observing the graph indicates that when $0.20$ mole of $A$ is reacted, $0.40$ mole of product is formed.
$\underset{-0.20}{A} \rightleftharpoons \underset{+0.40 \Rightarrow n=2}{n B} $
At equilibrium, $[A]=0.30 M,[B]=0.60 M$
$ K _c=\dfrac{[B]^{2}}{[A]}=\dfrac{0.36}{0.30}=1.2 $
BETA
