A student collects $450$ $mL$ of $HCl (g)$ at a pressure of $100$ $kPa$ and a temperature of $17°C$. What is the new volume of the $HCl$ at standard temperature and pressure?

Md Ariful Islam

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First convert the temperature to kelvin: $17+273=290$ $K$. Standard temperature is $273$ $K$.

Now $100$ $kPa$ is already standard pressure, so the pressure is constant.

We should work in SI units, so $450$ $mL$ = $0.450$ $L$.

From the , but with pressure omitted because it is constant, take $V_1/T_1=V_2/T_2$ and rearrange to $V_2=(V_1T_2)/T_1=(0.450xx273)/290=0.424$ $L$ = $424$ $mL$.

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