Phereseadula has to determine the specific heat capacity of milk. He uses a constant volume calorimeter with a heat capacity of 758 J/K and the combustion of acetylene (C2H2) to do the experiment: 2C2H2(g) + 502(g) 4CO2(g) +2H20(g) -AH = -2610kJ The calorimeter is filled with 1.190L of milk (instead of water). The density of milk is 1.034 g/ cm. When 4.413 g of acetylene is burned in excess oxygen in the reaction vessel (bomb) of the calorimeter, the temperature of the milk and the bomb increased from 22.5°C to 61.9°C. The heat absorbed by the bomb is: O 1.23 x 103 J 3.96 x 100 J 2.99 x 103 J 2.22 x 105 J 1.92 x 105 J None of the above

Phereseadula has to determine the specific heat capacity of milk. He uses a constant volume calorimeter with a heat capacity of 758 J/K and the combustion of acetylene (C2H2) to do the experiment: 2C2H2(g) + 502(g) 4CO2(g) +2H20(g) -AH = -2610kJ The calorimeter is filled with 1.190L of milk (instead of water). The density of milk is 1.034 g/ cm. When 4.413 g of acetylene is burned in excess oxygen in the reaction vessel (bomb) of the calorimeter, the temperature of the milk and the bomb increased from 22.5°C to 61.9°C. The heat absorbed by the bomb is: O 1.23 x 103 J 3.96 x 100 J 2.99 x 103 J 2.22 x 105 J 1.92 x 105 J None of the above

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 88QAP: A sample of sucrose, C12H22O11, is contaminated by sodium chloride. When the contaminated sample is...

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A sample of sucrose, C12H22O11, is contaminated by sodium chloride. When the contaminated sample is burned in a bomb calorimeter, sodium chloride does not burn. What is the percentage of sucrose in the sample if a temperature increase of 1.67C is observed when 3.000 g of the sample are burned in the calorimeter? Sucrose gives off 5.64103kJ/mol when burned. The heat capacity of the calorimeter and water is 22.51 kJ/C.
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
Natural gas companies in the United States use the therm as a unit of energy. One therm is 1105 BTU. (a) How many joules are in one therm? (1J=9.48104BTU) (b) When propane gas, C3H8, is burned in oxygen, CO2 and steam are produced. How many therms of energy are given off by 1.00 mol of propane gas?
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Ethyl alcohol, C2H5OH, is the intoxicating agent in liquor. Burning 1.00 g of ethyl alcohol in an excess of oxygen at 23.28C and constant volume releases 29.52 kJ of heat. When 7.40 g of ethyl alcohol is burned in oxygen under the same conditions in a bomb calorimeter, the temperature of the bomb and water rises from 23.28C to 48.04C. The bomb holds 0.750 kg of water. (a) What is q for the combustion of the ethyl alcohol in the bomb calorimeter? (b) What is qH2O? (c) What is qcal? (d) What is the heat capacity of the calorimeter?
A 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 21.8C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, and volumes are additive.