1. To 50.0 g of water at 25.00°C in a calorimeter was added 5.00 g of solid sodium nitrate, also at 25.00°C. The specific heat of the resultant solution was 4.20 J/g-°C. The heat capacity of the calorimeter was 15.0 JC. The energy change for dissolving sodium nitrate in water is 20.5 kJ per mole of sodium nitrate. a. Write a chemical equation showing the dissolution of solid sodium nitrate in water. b. Is the dissolution of solid sodium nitrate in water endothermic, exothermic, neither, or cannot be determined? Justify your choice. c. After the solid sodium nitrate dissolved in water, what was the final solution temperature?

In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl are mixed. Both solutions were originally at 24.6 C. After the reaction, the final temperature is 31.3 C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.

1. The metabolism of one mole of glycerol trioleate, C5 H9306, a common fat, produces 3.022 x 10¹kJ of heat. How many grams of the fat must be burned to raise the temperature of 50 g of water from 25.0°C to 30.0°C? 2. A metal sample having a temperature of 100°C and a mass of 45.2 g was placed in 50 g of water with a temperature of 26°C. At equilibrium, the final temperature was 32.7°C a) How much heat flowed into the water? b) What is the specific heat of the metal?

4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6

One day while camping, a student used a propane stove to boil some water. The student heated 5.00 L of water from 15.6°C to 98.5°C. The molar enthalpy of combustion of propane is -2043.9 kJ/mol and heating the water required 1.38 mol of propane. Determine the efficiency of the propane camp stove if the heat released from the stove was used to heat the water. 62.4 % 38.4% D162 % 61.6%

Iron has a specific heat capacity of 0.444J/g-C. 50.0 g of iron at 35C is added to 50.0 g of water with a specific heat capacity of 4.184 J/g-C. When the temperature of the resulting mixture stops changing, the temperature is closer to that of the original water than to the iron. True or false?

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