Chapter 10 - Gases - Exercises: 10.63a

For He(g): 1.87 atm For Ne(g) = 0.8085 atm For Ar(g) = 0.2695 atm

Work Step by Step

To find the partial pressure of each gas we can perform PV = nRT with each of the different quantities of moles since the partial pressures are independent of one another. First we convert the 25C to Kelvin by adding 273 = 298K. Then we have P = nRT / V but since T and V will stay constant, we will find the value of (RT/V) RT/V = (0.0821 * 298K) / 10L = 2.45 Then for each gas we have: P = n * (RT/V) so for He(g) we have P = 0.765mol * 2.45 = 1.87 atm for Ne(g) we have P = 0.330 mol * 2.45 = 0.8085 atm for Ar(g) we have P = 0.110 * 2.45 = 0.2695 atm

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