Question

a sample of hydrogen gas (h2) is mixed with water vapor (h2o (g)). the make sure has a total pressure of 811 torr, and the water vapor has a partial pressure of 12 torr. how many moles of hydrogen gas are present in a 10.0 l mixture at 298k?

Answer 1

`n=0.430molH_2`

Step-by-step explanation:

Hello!

In this case, considering the partial Dalton's law of partial pressures, we can notice that the total pressure equals the pressure of steam and the pressure of hydrogen, which can be determined as shown below:

`p_T=p_H+p_w\\\\p_H=811torr-12torr=799torr*(1atm)/(760torr)\\\\p_H=1.05atm`

Thus, by using the ideal gas law, we can compute the moles of hydrogen as shown below:

`PV=nRT\\\\n= (PV)/(RT)=(1.05atm*10.0L)/(0.082(atm*L)/(mol*K)*298K)\\\\n=0.430molH_2`

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