5. At 320 K and 16 bar, the molar volume of ammonia, NH3, is about 10% less than that of an ideal gas. The best explanation for this observation is: (a) The volume of an NH3 molecule is significant at this concentration. (b) The volume of an NH3 molecule is smaller than that of an ideal gas. (c) At this temperature, a significant amount of NH3 decomposes to N₂ and H₂. (d) Intermolecular forces of attraction for NH3 become significant at this temperature and pressure.

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5. At 320 K and 16 bar, the molar volume of ammonia, NH3, is about 10% less than that of an
ideal gas. The best explanation for this observation is:
(a) The volume of an NH3 molecule is significant at this concentration.
(b) The volume of an NH3 molecule is smaller than that of an ideal gas.
(c) At this temperature, a significant amount of NH3 decomposes to N2 and H₂.
(d) Intermolecular forces of attraction for NH3 become significant at this temperature and
pressure.
Transcribed Image Text:5. At 320 K and 16 bar, the molar volume of ammonia, NH3, is about 10% less than that of an ideal gas. The best explanation for this observation is: (a) The volume of an NH3 molecule is significant at this concentration. (b) The volume of an NH3 molecule is smaller than that of an ideal gas. (c) At this temperature, a significant amount of NH3 decomposes to N2 and H₂. (d) Intermolecular forces of attraction for NH3 become significant at this temperature and pressure.
6. The van der Waals a constant for CH4 is a = 0.2283 Pa mº mol-2. What is the constant in bar
L² mol-²?
(a) 2.283x10-²
(b) 2.283x10-5
(c) 2.283
(d) 2.283x104
Transcribed Image Text:6. The van der Waals a constant for CH4 is a = 0.2283 Pa mº mol-2. What is the constant in bar L² mol-²? (a) 2.283x10-² (b) 2.283x10-5 (c) 2.283 (d) 2.283x104
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