Question

Consider a reaction $A\left(g\right)\to 3B\left(g\right)+2C\left(g\right)$with rate constant $1.386\times {10}^{-2}mi{n}^{-1}$. Starting with $2moles$ of $A$ in $12.5litre$ vessel initially, if reaction is allowed to takes place at constant pressure & at $298K$ then find the concentration of $B$ after $100min$.

• A. $0.04M$
• B. $0.36M$
• C. $0.09M$
• D. none of the above

Answer 1

The correct option is D none of the above

Rate constant $\left(K\right)=1.386\times {10}^{-2}{min}^{-1}$

$\therefore$ It is a $1^{st}$ order reaction.

$\therefore$ Rate$=k\left[A\right]=1.386\times {10}^{-2}\times \frac{2}{12.5}=2.2176\times {10}^{-3}mol{L}^{-1}mi{n}^{-1}$

Now, Rate$=\frac{1}{3}\frac{d\left[B\right]}{dt}\therefore 2.2176\times {10}^{-3}=\frac{1}{3}\times \frac{[B{]}_t}{100}{\left[B\right]}_t=0.665M$