166. 40.0 g of ice cubes at 0.0°C are combined with 150. g of liquid water at 20.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (Data: specific heat capacity of H20(1), c = 4.18 J/g.°C; H2O(s) → H2O(1) A) 0.0 %3D НаО() B) 10.6 AH= 6.02 kJ/mol) C) 30.7 D) 43.2 E) 56.4 %3D

166. 40.0 g of ice cubes at 0.0°C are combined with 150. g of liquid water at 20.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (Data: specific heat capacity of H20(1), c = 4.18 J/g.°C; H2O(s) → H2O(1) A) 0.0 %3D НаО() B) 10.6 AH= 6.02 kJ/mol) C) 30.7 D) 43.2 E) 56.4 %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 1.37 g sample of butane, C4H10(g), was burned in a bomb calorimeter in the presence of excess oxygen. The calorimeter contained 1.09 kg of water. Calculate the heat exchanged with respect to the system during the reaction if the calorimeter has a heat capacity of 648. J/°C and the temperature of the calorimeter and water changed from 23.6°C to 35.6°C? Enter your answer to 3 significant figures in decimal form. Do not enter units since they are already given. 58.12 kJ Calculate the heat exchanged with respect to the system per mole of butane. Enter your answer to 3 signficant figures in decimal form. Do not enter units since they are already given.’ 2547.5 kJ
The combustion of 1.00 mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.23 g of glucose is burned in a calorimeter containing 877 g of water, and the temperature of the assembly increases from 20.10oC to 23.94oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol
An electrical heater is used to add 19.75 kJ of heat to a constant-volume calorimeter. The temperature of the calorimeter increases by 4.76°C. When 2.00 g of methanol (CH3OH) is burned in the same calorimeter, the temperature increases by 10.92°C. Calculate the molar heat of combustion for methanol (in kJ).
5) The combustion of sucrose (C12H22O11, molar mass = 342.3 g/mol) has a AErxn of -1.40 x 104 kJ/mol. When 1.25 grams of sucrose undergoes combustion in a bomb calorimeter, the temperature rises from 22.2 °C to 34.3 °C. What is the heat capacity of the bomb calorimeter? 0 5.39 kJ/C 05.90 ki 04.23 KJPC 04.90 ki/C
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C. The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data. Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol). C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy
When a 4.31 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.2 kJ/•C. The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane. Enter your answer numerically and in terms of kJ/mol.
The combustion of 1.00mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.64g of glucose is burned in a calorimeter containing 788 g of water, and the temperature of the assembly increases from 20.10oC to 24.16oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol.
20.0 g of ice cubes at 0.0°C are combined with 150. g of liquid water at 70.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (Data: specific heat capacity of H20(), c = 4.18 J/g.°C; H 20( s) – H20() A H= 6.02 kJ/mol)Hint: When you equate heat lost to heat gained the heat capacity is cancelled since it si found on both sides of the equation and this simplifies your calculation. O 0.0 O 10.6 O 30.7 O 56.4 O61.8
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.3215 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.162×10 g of water. During the combustion the temperature increases from 25.15 to 27.48 °C. The heat capacity of water is 4.184 J glc-!. The heat capacity of the calorimeter was determined in a previous experiment to be 769.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O,(g) – → 5 H,O(1) + 14 CO2(g) + Energy Molar Heat of Combustion = kJ/mol
2) The combustion of 0.25 g sucrose, C1HO11, in a bomb calorimeter causes the temperature to rise from 24.9 to 28.3 °C. If the heat capacity of the calorimeter is 4.90 kJ/°C, calculate the heat of combustion of sucrose in kJ/g.
1.) The molar heat of combustion of octane to form carbon dioxide and water vapour is ─5470.1kJ/mol. Using this value, determine the mass of octane required to increase the temperature of 1.50 L of water from 22.0°C to 85.6°C. 2.) A simple calorimeter is filled with 250g of water initially at 25.0°C. A mass of 0.500g of benzene is completely burned to heat the water in the calorimeter. The highest temperature of the calorimeter water is measured at 44.0°C. What is the experimental value of the molar enthalpy of combustion of benzene?
THERMODYNAMICS: A 1.96 g sample of acetic acid (HC;H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/°C, contained 776 g of water. The temperature of the calorimeter and its contents increased from 24.51°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place) Round your answer to 1 decimal place.