Question

A chemical reaction $2A\to 4B+C$; in gaseous phase shows an increase in concentration of $B$ by $5\times {10}^{-3}M$ in $10$ second. Calculate:
(a) rate of appearance of $B$,
(b) rate of the reaction,
(c) rate of disappearance of $A$.

Answer 1

$2A\to 4B+C$

(i) $Rate=\frac{1}{4}\frac{AppearanceofB}{Time}$

$\Rightarrow 5\times {10}^{-4}=\frac{1}{4}\frac{AppearanceofB}{10}$

$\Rightarrow AppearanceofB=2\times {10}^{-2}mol/L$

(ii) $Rate=\frac{Increaseinconcentration}{Time}$

$=\frac{5\times {10}^{-3}}{10}$

$=5\times {10}^{-4}mol{L}^{-1}se{c}^{-1}$

(iii) $Rate=\frac{1}{2}\frac{DisappearanceofA}{Time}$

$\Rightarrow 5\times {10}^{-4}=\frac{1}{2}\frac{DisappearanceofB}{10}$

$\Rightarrow DisappearanceofB={10}^{-2}mol/L$