N2O5 decomposes to NO2 and O2 and follows first order kinetics. After 50 minutes, the pressure inside the vessel increases from 50mm Hg to 87.5mm Hg. The pressure of the gaseous mixture after 100 minutes at constant temperature will be __________. 175.0mmHg 116.25mmHg 106.25mmHg 136.25mmHg

N2O5→2NO2+12O2
R=k[N2O5]
1.Po-p2p12p→50min
3.Po-p12p112p1→100min
Po=50
∴P50min=Po+32P=87.5
P=23(87.5-50)
P=37.5
3×2=25
First order
Eqn:t=2.303klog[(N2O5)(N2O5)t]
At 50 min :t=2.303klog2
k=2.30350×0.3010
At 100min :100=2.303×502.303×0.3010log[(N2O5)o(N2O5)100]
2×0.3010=log10[50x]
4=50x
x=504
∴Po-p1=12.5
p1=50-12.5
p1=37.5
∴Total Pressure=Po+32×37.5=106.25mm of Hg
Hence, the correct option is B