Question

(a) Consider the combustion of ethylene, given below.

C_{2}H_{4}(*g*) + 3
O_{2}(*g*) ? 2 CO_{2} (*g*) + 2
H_{2}O (*g*)

If the concentration of C_{2}H_{4} is decreasing
at the rate of 0.26 *M*/s, what are the rates of change in
the concentrations of CO_{2} and H_{2}O?

CO_{2}

(b) The rate of decrease in N_{2}H_{4} partial
pressure in a closed reaction vessel from the following reaction is
41 torr/hr.

N_{2}H_{4} (*g*) + H_{2}
(*g*) ? 2 NH_{3} (*g*)

What are the rates of change of NH_{3} partial pressure
and total pressure in the vessel?

NH_{3}

Answer #1

(a)

The given reaction is

C_{2}H_{4}(*g*) + 3
O_{2}(*g*) ? 2 CO_{2} (*g*) + 2
H_{2}O (*g*)

rate = -d[C2H4]/dt = -1/3d[O2]/dt = +1/2d[CO2]/dt = +1/2d[H2O]/dt

Given, -d[C2H4]/dt = 0.26 M/s

Rate of change in concentration of CO2 is

-d[C2H4]/dt = +1/2d[CO2]/dt

0.26 M/s = +1/2d[CO2]/dt

d[CO2]/dt = 2 x 0.26 = **0.52 M/s**

Rate of change in concentration of H2O is

-d[C2H4]/dt = +1/2d[H2O]/dt

0.26 M/s = +1/2d[H2O]/dt

+1/2d[H2O]/dt = 2 x 0.26 = **0.52
M/s**

--------------------------------------------

(b)

The given reaction is

N_{2}H_{4} (*g*) + H_{2}
(*g*) ? 2 NH_{3} (*g*)

rate = -d[N2H4]/dt ] = -d[H2]/dt = +1/2d[NH3]/dt

-d[N2H4]/dt ] = 41 torr/hr

The rate of change of NH3 partial pressure is

-d[N2H4]/dt ] = +1/2d[NH3]/dt

d[NH3]/dt = 2 x -d[N2H4]/dt ] = 2 x 41 torr/hr = 82 torr/hr

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