How much heat does it take to raise 50.0 g of liquid water to 120 °C if its initial temperature is 50°C? (Possibly useful values: Cwater = 4.184 J/g.°C, Csteam = 1.99 J/g.°C, Cice = 2.108 J/g.°C, AHfus6.01 kJ/mol, AHvap = 40.79 kJ/mol)%3D%3D142.3 kJ14.6 kJ312.6 kJ125.6 kJ284.3 kJ

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Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter11: Liquids And Solids

Section: Chapter Questions

Problem 11.98QE

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The cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of vaporization of ethanol (ethyl alcohol), C2H5OH. C2H5OH(l)C2H5OH(g);H=? The standard enthalpy of formation of C2H5OH(l) is 277.7 kJ/mol and that of C2H5OH(g) is 235.1 kJ/mol.
Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?
9.46 The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy would be needed to melt a 5.24-g sample of silicon at its melting point of 1693 K?
If you want to convert 56.0 g ice (at 0 °C) to water at 75.0 °C, calculate how many grams of propane, C3H8, you would have to bum to supply the energy to melt the ice and then warm it to the final temperature (at 1 bar).
The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.
he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy fusion(41kJ/molvs.6kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?
Why are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.
Benzene, C6H6, is an organic liquid that freezes at 5.5 C (Figure 11.1) to form beautiful, feather-like crystals. How much energy is evolved as heat when 15.5 g of benzene freezes at 5.5 C? (The enthalpy of fusion of benzene is 9.95 kJ/mol.) If the 15.5-g sample is remelted, again at 5.5 C, what quantity of energy is required to convert it to a liquid?
A 1.40-g sample of polyethylene, a common plastic, is dissolved in enough organic solvent to give 100.0 mL of solution. What is the average molar mass of the polymer if the measured osmotic pressure of the solution is 1.86 mm Hg at 25 C?
A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0C. The reaction is 2Na(s)+2H2O(l)2NaOH(aq)+H2(g)H=368kJ Assuming no heat loss to the surroundings, will the ice melt? Assuming the final mixture has a specific heat capacity of 4.18 J/gc, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.
Liquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.
Which requires the absorption of a greater amount of heatâ€”vaporizing 100.0 g of benzene or boiling 20.0 g of water? (Use Table 8.2.)

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How much heat does it take to raise 50.0 g of liquid water to 120 °C if its initial temperature is 50 °C? (Possibly useful values: Cwater = 4.184 J/g.°C, Csteam = 1.99 J/g.°C, Cice = 2.108 J/g.°C, AHfus 6.01 kJ/mol, AHvap = 40.79 kJ/mol) %3D %3D 142.3 kJ 14.6 kJ 312.6 kJ 125.6 kJ 284.3 kJ