Question

For the decomposition of dinitrogen pentoxide at 200°C,
N2O5(g) to N2O4(g) + 1/2O2(g)
if the initial pressure is 114 mm and after 25 minutes of the reaction, total pressure of the gaseous mixture is 133 mm, calculate the average rate of the reaction in (a) atm/min (b) mol/L/s

Answer 1

Answer:

For the decomposition of dinitrogen pentoxide at 200°C,

N2O5(g) to N2O4(g) + 1/2O2(g)

if the initial pressure is 114 mm and after 25 minutes of the reaction, total pressure of the gaseous mixture is 133 mm

Explanation:

Reaction involved:

N2O5(g) to N2O4(g) + 1/2O2(g)

initial pressure is 114 mm

total pressure of the gaseous mixture is 133 mm

initially               114mm     0     0

after 25 mins     114-a     a       a/2

total pressure:

114-a+a+a/2=133

a= 38 mm

   = 38/760

   = 0.05 atm

average rate of reaction in atm min^-1

= change in pressure/ change in rate

=0.05/(25-0)

= 0.002 atm/min

average rate of reaction in L^-1 s^-1

n/V= P/RT

average rate=  0.002/(0.0821*473*60)

                = 8.58 *10^-7 mol L^-1 s^-1