Partial Pressure Question

Question

A mixture of hydrogen and krypton gases, in a 6.18 L flask at 76 °C, contains 0.320 grams of hydrogen and 6.06 grams of krypton. The partial pressure of krypton in the flask is____atm and the total pressure in the flask is____atm.

Answer 1

This a question using Daltons law of Partial Pressures - Pt = Pa + Pb .......

You are given the total volume of the mixture of H2(g) and Kr(g) at 6.18 L. as well as the temperature of the gas in ^0C at 76. You are as well given the grams of the H2 gas 0.320 g and the grams of Kr at 6.06.

Assuming the gasses act as ideal gasses, you can use the ideal gas law equation PV=nRT.

step 1: convert grams of H2 and grams of Kr to moles

step 2) convert celsius temperature to Kelvin Temperature

step 3: using PV = nRT knowing the values that you previously calculated of each gas (moles, Kelvin temperature and. the given volume in Liters), plug in the values for each using the ideal gas law equation for each to solve the unknown Pa which will know be in atm of each gas.

Step 4: To find the Pt (total pressure) in the flask add the 2 calculated Pa that you just calculated for H2(g) and Kr(g)

I hope this was helpful. If you need any further help you can always contact me.