Interpretation:
Calculation of volume of dry ice at given pressure and temperature.
Concept introduction:
Sublimation is a process in the solid state directly gets converted into gaseous form without getting converted into liquid.
The
Where, p is pressure of the gas in unit −atm, v is volume of gas in liters, n is amount of the gas in moles, r is the ideal gas constant
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Chapter 5 Solutions
Bundle: Introduction to General, Organic and Biochemistry, 11th + OWLv2, 4 terms (24 months) Printed Access Card
- 5-106 The normal boiling point of hexane, C6H14, is 69°C, and that of pentane, C5H12, is 36°C. Predict which of these compounds has a higher vapor pressure at 20°C.arrow_forward5-86 Using the phase diagram of water (Figure 5-20), describe the process by which you can sublime 1 g of ice at-10°C and at 1 atm pressure to water vapor at the same temperature.arrow_forwardDefine the following and give an example of each: (a) dispersion force (b) dipole-dipole attraction (c) hydrogen bondarrow_forward
- On the basis of intermolecular attractions, explain the differences in the boiling points of n butane (1 C) and chloroethane (12 C), which have similar molar masses.arrow_forwardIn an experiment, 20.00 L of dry nitrogen gas, N2, at 20.0C and 750.0 mmHg is slowly bubbled into water in a flask to determine its vapor pressure (see the figure on next page). The liquid water is weighed before and after the experiment, from which the experimenter determines that it loses 353.6 mg in mass. Answer the following questions. a How many moles of nitrogen were bubbled into the water? b The liquid water diminished by how many moles? What happened to the liquid? c How many moles of gas exit the flask during the experiment? What is the partial pressure of nitrogen gas exiting? The total gas pressure is 750.0 mmHg. d From these data, calculate the vapor pressure of water at 20C. Does this agree with what you expect?arrow_forwardPredict which liquid—glycerol, HOCH2CH(OH)CH2OH, or hexane, C6H14—has the greater surface tension. Explain your prediction.arrow_forward
- 5-81 Compare the number of calories absorbed when 100. g of ice at 0°C is changed to liquid water at 37°C with the number of calories absorbed when 100. g of liquid water is warmed from 0°C to 37°C.arrow_forwardIn terms of the kinetic molecular theory, in what ways are liquids similar to gases? In what ways are liquids different from gases?arrow_forwardAnswer 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_forward
- In each of the following groups of substances, pick the one that has the given property. Justify your answer. a. highest boiling point: HBr, Kr, or Cl2 b. highest freezing point: H2O, NaCl, or HF c. lowest vapor pressure at 25C: Cl2, Br2, or I2 d. lowest freezing point: N2, CO, or CO2 e. lowest boiling point: CH4, CH3CH3, or CH3CH2CH3 f. highest boiling point: HF, HCl, or HBr g.arrow_forwardA tank of gas at 21C has a pressure of 1.0 atm. Using the data in the table, answer the following questions. Explain your answers. a If the tank contains carbon tetrafluoride, CF4, is the liquid state also present? b If the tank contains butane, C4H20, is the liquid state also present?arrow_forwardGases that cannot be liquefied at room temperature merely by compression are called permanent gases. How could you liquefy such a gas?arrow_forward
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