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163 ml of hydrogen gas, measured at 23°C and 1.5 atm pressure, and 249 ml of nitrogen gas, measured at 23°C and 2.6 atm pressure, were forced into a 163 ml container at 23°C. What would be the pressure (in atm) of the mixture of gases now in the 163 ml container? Enter to 2 decimal places.

Answer :

The total pressure is 3.9 atm

What is the ideal gas equation?

We would have to use the idea gas equation in each case;

Number of moles of the hydrogen = 1.5 * 0.163/0.082 * 296

= 0.24/24.3

= 0.0099 moles

Number of moles of nitrogen = 2.6 * 0.163/0.082 * 296

n = 0.017 moles

Now we know from the Dalton's law that when we mix the gases that the total pressure is the pressure in each of the vessels summed up.

Hence the total pressure is; 1.6 + 2.3 = 3.9 atm

It would have a total pressure of about 3.9 atm.

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