Chemical and Ionic Equilibrium - Result Question 102
####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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Solution:
- Observing the graph indicates that when 0.20 mole of $A$ is reacted, 0.40 mole of product is formed.
$$ \begin{gathered} A \ -0.20 \end{gathered} \rightleftharpoons \begin{gathered} n B \ +0.40 \Rightarrow n=2 \end{gathered} $$
At equilibrium, $[A]=0.30 M,[B]=0.60 M$
$$ K _c=\frac{[B]^{2}}{[A]}=\frac{0.36}{0.30}=1.2 $$
