Four ice cubes at exactly 0°C with a total mass of 51.0 g are combined with 120 g of water at 85 °C in an insulated container (AH-6.02 kJ/mol Cwater-4.18J/g. C) If no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using two significant figures. 197| ΑΣΦ T= Submit Previous Answers Request Answer * Incorrect; Try Again ? ROVERW "C

Four ice cubes at exactly 0°C with a total mass of 51.0 g are combined with 120 g of water at 85 °C in an insulated container (AH-6.02 kJ/mol Cwater-4.18J/g. C) If no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using two significant figures. 197| ΑΣΦ T= Submit Previous Answers Request Answer * Incorrect; Try Again ? ROVERW "C

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 102E: A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice,...

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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).
In regions with dry climates, evaporative coolers are used to cool air. A typical electric air conditioner is rated at 1.00 104 Btu/h (1 Btu, or British thermal unit = amount of energy to raise the temperature of 1 lb water by 1F). What quantity of water must be evaporated each hour to dissipate as much heat as a typical electric air conditioner?
The amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.
A quantity of ice at 0C is added to 64.3 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C).
Sublimation is the phase change from solid to gas without going through a liquid phase. Solid CO2, called dry ice, is an example of one substance that sublimed. Use Hesss law to show that the enthalpy of sublimation, subH, is equal to fusH vapH.
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.
Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water that you drink may eventually be converted into sweat and evaporate. If you drink a 20-ounce bottle of water that had been in the refrigerator at 3.8 C, how much heat is needed to convert all of that water into sweat and then to vapor? (Note: Your body temperature is 36.6 oc. For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water.)
On a hot day, you take a six-pack ot a on a pcmc, cooling it with ice. Each empty (aluminum) can weighs 12.5 g. A can contains 12.0 oz of soda. The specific heat of aluminum is 0.902 J/g C; take that of soda to be 4.10 J/g C. (a) How much heat must be absorbed from the six-pack to lower the temperature from 25.00 to 5.00C? (b) How much ice must be melted to absorb this amount of heat? (Hfus of ice is given in Table 8.2.)
Sodium chloride is added in cooking to enhance the flavor of food. When 10.00 g of NaCl are dissolved in 200.0 mL of water at 25.0C in a coffee-cup calorimeter, 669 J of heat are absorbed. (You can make the following assumptions about the solution: volume =200.0 mL, density =1.00 g/mL, specific heat =4.18J/gC) (a) Is the solution process exothermic? (b) What is qH2O? (c) What is the final temperature of the solution?
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?
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.)
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?

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