Question

An industrial chemist is studying the rate of the haber synthesis: n2 + 3h2 → 2nh3. starting with a closed reactor containing 1.50 mol/l of n2 and 0.45 mol/l of h2, she finds that the h2 concentration has fallen to 0.16 mol/l after 30. seconds. what is the average rate of reaction of h2 over this time? (enter in mol/liter/sec).

Answer 1

Haber process is the large scale manufacture of a ammonia by reacting nitrogen and hydrogen at a ratio of 1:3
Change in hydrogen concentration is 0.45 - 0.16 = 0.29 moles/l
Therefore, the average rate of reaction of hydrogen = 0.29 / 30 = 0.0096 
   = 0.0096 moles/liter/sec

Answer 2

Haber synthesis is preparation of ammonia  
Reacting of nitrogen and hydrogen are at ratio of 1:3 from the equation.
 Change in hydrogen concentration has fallen, so the difference = 0.45 - 0.16  
Change = 0.29 moles/l
 Now average rate of reaction for hydrogen = Change / t = 0.29 / 30 = 0.0096 moles/liter/sec