122ch10c_002

# 122ch10c_002 - 32 10.76 33 10.76(cont 10.78 34 10.79 Under...

This preview shows pages 1–6. Sign up to view the full content.

32 10.76)

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
33 10.76) (cont.) 10.78)
34 10.79) Under these conditions this gas exhibits a negative deviation from ideality The intermolecular attractive forces reduce the effective number of particles and the real pressure. This is reasonable for 1 mole of gas at relatively low temp. and pressure. 10.82) 10.85)

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
35 10.88) It is simplest to calculate the partial pressure of each gas as it expands into the total volume, then sum the partial pressures. Use Boyle’s Law to calculate the new pressures of each gas in the mixture after the expansion. The final vol is: V 2 = 1.0 L + 1.0 L + 0.5 L = 2.5 L 10.89) Use mole fraction to calculate moles of O 2 in air (n O 2 = P O 2 n air ).
36 10.92) Calculate the average molar mass of the mixture of O 2 and Kr. Then relate the average molar mass to the molar masses of O 2 and Kr using mole fractions . Remember mole fractions add to 1.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

### Page1 / 9

122ch10c_002 - 32 10.76 33 10.76(cont 10.78 34 10.79 Under...

This preview shows document pages 1 - 6. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online