Question

Be sure to answer all parts. Consider the reaction N2(g) + 3H2(g) → 2NH3(g)

Suppose that at a particular moment during the reaction, molecular hydrogen is reacting at the rate of −0.091 M/s.

(a) At what rate is ammonia being formed?

(b) At what rate is molecular nitrogen reacting?

PLEASE HELP! THANKS!

Answer 1

rate of reaction in terms of all reactant and products are:

rate = -(1/3)*rate of reaction of H2 = - rate of reaction of N2 = (1/2)*rate of reaction of NH3

a)

USE:

-(1/3)*rate of reaction of H2 = (1/2)*rate of reaction of NH3

rate of reaction of NH3 = -(2/3)*rate of reaction of H2

= -(2/3)*(-0.091 M/s)

= 0.0607 M/s

Answer: 0.0607 M/s

b)

-(1/3)*rate of reaction of H2 = - rate of reaction of N2

rate of reaction of N2 = (1/3)*rate of reaction of H2

= (1/3)*(-0.091 M/s)

= -0.0303 M/s

Answer: -0.0303 M/s