Question

The adiabatic compression of a mixture of 2 volumes of Hydrogen and 1 volume of oxygen from 320 ml to 10 ml caused explosion. The initial pressure and temperature of the gaseous mixture were 1 atm and ${27}^{\circ }C$.
What is the pressure of the gaseous mixture at the moment of explosion?

• A. 32 atm
• B. 128 atm
• C. 1 / 32 atm
• D. 1 / 128 atm

Answer 1

Answer: (A)

32 atm

For compression,

$V_1$, Initial volume= $320ml$

$V_2$, Final volume= $10ml$

$P_1$, Initial pressure= $1atm$

$P_2$, Final pressure=

By using Boyle's Law;

$P\propto \frac{1}{V}$

or, $\frac{P_1}{P_2}=\frac{V_2}{V_1}\Rightarrow \frac{1atm}{P_2}=\frac{10ml}{320ml}$

$\Rightarrow P_2=32atm$

This will be the pressure at which the gas explodes.