Question

A sample of hydrogen gas collected by displacement of water occupied 30mL at 24 C on a day when the barometric pressure was 736t orr. What volume would the hydrogen occupy if it were dry and at STP? The vapor pressure of water at 24 C is 22.4 torr

Answer 1

`v_2=6,48*10^(-4)L`

Step-by-step explanation:

From the question we are told that:

Volume of hydrogen
`V_1=30mL=>30*10^(-3)`

Temperature
`T_1=24C=>24+273=>297k`

Pressure of water
`P_1=22.4torr=>(22.4)/(760)=0.0295atm`

Let

STP(Standard Temperature and pressure)

`T_2=273K`

`P_2=1atm`

Generally the equation for ideal gas is mathematically given by

`(p_1V_1)/(T_1)=(P_2V_2)/(T_2)`

Therefore

`v_2=(P_1v_1T_2)/(T_1P_2)`

`v_2=(0.0295*30*10^(-3)*273)/(297*1)`

`v_2=6.48*10^(-4)L` (at STP(Standard Temperature and pressure))