Question

$11$ g of $C_3{H}_8$ is filled in a bulb having $1$ litre capacity which can withstand a maximum pressure of $10$ atm. At what temperature will the pressure of gas reach the bursting limit?

• A. ${365.89}^{\circ }\text{C}$
• B. ${124.21}^{\circ }\text{C}$
• C. ${214.21}^{\circ }\text{C}$
• D. ${487.21}^{\circ }\text{C}$

Answer 1

The correct option is C ${214.21}^{\circ }\text{C}$

Using the ideal gas equation, PV = nRT
where, P = Pressure of the gas
V = volume of the bulb
n = number of moles of gas
T = Temperature of the gas equation

Substituting the values,
$T=\frac{PV}{nR}=\frac{10\times 1}{\left(11/44\right)\times 0.0821}=487.21\text{K}=214.21{}^{\circ }\text{C}$