Question

A 21.5 L sample of gas at 107 kPa has a temperature of 27.2 °C. What is the pressure of the gas
if it is transferred to a 32.6L container at 44.1 °C?

Answer 1

Answer:

The right answer is "74.516 kPa".

Explanation:

The given values are:

V₁ = 21.5 L

V₂ = 32.6L

P₁ = 107 kPa

T₁ =27.2°C+273

T₂ = 44.1 °C+273

As we know,

⇒  $\frac{P_1V_1}{T_1}= \frac{P_2V_2}{T_2}$

then,

⇒  $P_2=\frac{P_1V_1T_2}{T_1V_2}$

On substituting the given values, we get

⇒       $=\frac{107\times 21.5\times (44.1+273)}{(27.2+273)\times 32.6}$

⇒       $=\frac{107\times 21.5\times 317}{300.2\times 32.6}$

⇒       $=\frac{729258.5}{9786.52}$

⇒       $=74.516 \ kPa$