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

Answer:

$v_2=6,48*10^{-4}L$

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 $P_1=22.4torr=>\frac{22.4}{760}=0.0295atm$

Let

STP(Standard Temperature and pressure)

 $T_2=273K$

 $P_2=1atm$

Generally the equation for ideal gas is mathematically given by

 $\frac{p_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

Therefore

 $v_2=\frac{P_1v_1T_2}{T_1P_2}$

 $v_2=\frac{0.0295*30*10^{-3}*273}{297*1}$

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