Question

3 Consider the reaction :

Answer 1

Answer:

(a) The rate at which ammonia being formed = 0.0493 M/s

(b) The rate at which molecular nitrogen reacting = 0.0247 M/s

Explanation:

$N_{2}+3H_{2}\longrightarrow2NH_{3}$

The rate at which molecular hydrogen is reacting = $\frac{d}{dt}[H_{2}]=0.074\:M/s$

The rate of the above reaction can be expressed as:

$rate=-\frac{d}{dt}[N_{2}]=-\frac{1}{3} \frac{d}{dt}[H_{2}]=\frac{1}{2}\frac{d}{dt}[NH_{3}]$

(a) $\frac{d}{dt}[NH_{3}]=\frac{2}{3}(0.074)=0.0493$

The rate at which ammonia being formed = 0.0493 M/s

(b) $-\frac{d}{dt}[N_{2}]=\frac{1}{3}(0.074)=0.0247$

The rate at which molecular nitrogen reacting = 0.0247 M/s