Question

The rate of dissappearance of $S{O}_2$ in the reaction $2S{O}_2+O_2\to 2S{O}_3$ is $1.28\times {10}^{-3}g/sec$. Then the rate of formation of $S{O}_3$ is :

• A. $0.64\times {10}^{-3}g/sec$
• B. $0.80\times {10}^{-3}g/sec$
• C. $1.28\times {10}^{-3}g/sec$
• D. $1.60\times {10}^{-3}g/sec$

Answer 1

Answer: (C)

$1.28\times {10}^{-3}g/sec$

The Rate of disappearance of $S{O}_2$ is $1.28\times {10}^{-3}g/sec$

In this Reaction,

Rate of disappearance of $S{O}_2$ = Rate of Formation of $S{O}_3$

So, The Rate of formation of $S{O}_3$ = $1.28\times {10}^{-3}g/sec$