(a)
Interpretation:
The result of heating a sample of water from -20 to 200 0C at a constant pressure of 600 Torr should be described.
Concept introduction:
When a phase change occurs, temperature remains constant. Temperature at which a solid starts to melt is called melting point and temperature at which the vapor pressure of a liquid equals to atmospheric pressure is called boiling point. All three phases are in equilibrium at triple point and beyond the critical point liquid and vapor phases become indistinguishable.
(b)
Interpretation:
The result of increase in the pressure on a sample of iodine from
Concept introduction:
Temperature at which a solid starts to melt is called the melting point and temperature at which the vapor pressure of a liquid equals to atmospheric pressure is called boiling point. All three phases are in equilibrium at triple point and beyond the critical point, the liquid and vapor phases become indistinguishable. A gas can be liquefied under the temperatures below critical temperature.
(c)
Interpretation:
The result of cooling the sample of carbon dioxide at
Concept introduction:
Temperature at which a solid starts to melt is called melting point and temperature at which the vapor pressure of a liquid equals to atmospheric pressure is called boiling point. All three phases are in equilibrium at triple point and beyond the critical point liquid and vapor phases become indistinguishable. A gas can be liquefied under the temperatures below critical temperature.
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General Chemistry: Principles and Modern Applications (11th Edition)
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- Answer the following questions: (a) If XX behaved as an ideal gas, what would its graph of Z vs. P look like? (b) For most of this chapter, we performed calculations treating gases as ideal. Was this justified? (c) What is the effect of the volume of gas molecules on Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (d) What is the effect of intermolecular attractions on the value of Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (e) In general, under what temperature conditions would you expect Z to have the largest deviations from the Z for an ideal gas?arrow_forward5-111 Diving, particularly SCUBA (Self-Contained Underwater Breathing Apparatus) diving, subjects the body to increased pressure. Each 10. m (approximately 33 ft) of water exerts an additional pressure of 1 atm on the body. (a) What is the pressure on the body at a depth of 100. ft? (b) The partial pressure of nitrogen gas in air at 1 atm is 593 mm Hg. Assuming a SCUBA diver breathes compressed air, what is the partial pressure of nitrogen entering the lungs from a breathing tank at a depth of 100. ft? (c) The partial pressure of oxygen gas in the air at 2 atm is 158 mm Hg. What is the partial pressure of oxygen in the air in the lungs at a depth of 100. ft? (d) Why is it absolutely essential to exhale vigorously in a rapid ascent from a depth of 100. ft?arrow_forwardWhich is denser at the same temperature and pressure, dry air or air saturated with water vapor? Explain.arrow_forward
- ook at Fig. 14.2. Why doesn't temperature increase continuously ever time? That is, why does the temperature stay constanl for periods of time?arrow_forwardIdentify two common observations indicating some solids, such as dry ice and mothballs, have vapor pressures sufficient to sublime?arrow_forwardWhen dry ammonia gas (NH3)is bubbled into a msp;125mLsample of water, the volume of the sample (initially, at least) decreases slightly. Suggest a reason for this.arrow_forward
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