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

`186.01\ \text{mL}`

Step-by-step 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

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

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