Question

A sample of hydrogen gas has a volume of 145 mL when measured at 44
degrees C and 1.47 atm. What volume would the hydrogen sample occupy
at STP?

Answer 1

Answer:

$186.01\ \text{mL}$

Explanation:

$P_1$ = Initial pressure = 1.47 atm

$P_2$ = Final pressure = $10^5\ \text{Pa}$

$T_1$ = Initial temperature = $44^{\circ}\text{C}$

$T_2$ = Final temperature = $273.15\ \text{K}$

$V_1$ = Initial volume = 145 mL

$V_2$ = Final volume

We have the relation

$\dfrac{P_1V_1}{T_1}=\dfrac{P_2V_2}{T_2}\\\Rightarrow V_2=\dfrac{P_1V_1T_2}{T_1P_2}\\\Rightarrow V_2=\dfrac{1.47\times 101325\times 145\times 273.15}{(44+273.15)\times 10^5}\\\Rightarrow V_2=186.01\ \text{mL}$

Final volume of the sample is $186.01\ \text{mL}$.