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Iculate föllowing. aicate if the system do work on the surroundings or the surroundings do work on the system. a. q=-47 kJ, w = +88 kJ b. q=+82 kJ, w = -47 kJ c. q=+47 kJ, w = 0 kJ

Iculate föllowing. aicate if the system do work on the surroundings or the surroundings do work on the system. a. q=-47 kJ, w = +88 kJ b. q=+82 kJ, w = -47 kJ c. q=+47 kJ, w = 0 kJ

Chemistry
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1. Calculate AE for each of the following. Indicate if the system do work on the surroundings or the surroundings do work on the system. a. q= -47 kJ, w =+88 kJ b. q=+82 kJ, w = -47 kJ c. q= +47 kJ, w = 0 kJ 2. A piston is compressed from a volume of 8.30 L to 2.80 L against a constant pressure of 1.90 atm. In the process, there is a heat gain by the system of 350. J. Calculate the internal energy change. 3. The equation for the fermentation of glucose to alcohol and carbon dioxide is C,H1206 (aq) → 2 C,H;OH(aq) + 2 CO2(9) The enthalpy change for the reaction is -67 kJ. Is the reaction exothermic or endothermic? Is energy, in the form of heat absorbed or evolved as the reaction occurs?
Transcribed Image Text:1. Calculate AE for each of the following. Indicate if the system do work on the surroundings or the surroundings do work on the system. a. q= -47 kJ, w =+88 kJ b. q=+82 kJ, w = -47 kJ c. q= +47 kJ, w = 0 kJ 2. A piston is compressed from a volume of 8.30 L to 2.80 L against a constant pressure of 1.90 atm. In the process, there is a heat gain by the system of 350. J. Calculate the internal energy change. 3. The equation for the fermentation of glucose to alcohol and carbon dioxide is C,H1206 (aq) → 2 C,H;OH(aq) + 2 CO2(9) The enthalpy change for the reaction is -67 kJ. Is the reaction exothermic or endothermic? Is energy, in the form of heat absorbed or evolved as the reaction occurs?
4. The enthalpy of combustion of CH:(g) when H20(1) is formed is -891 kJ/mol and the enthalpy of combustion of CH-(g) when H20(g) is formed is -803 kJ/mol. Use these data and Hess's law to determine the enthalpy of vaporization of water. 5. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for CAH4 (-2341 kJ/mol), CAH3 (-2755 kJ/mol), and H2 (-286 kJ/mol), calculate AH for the reaction C4H4(g) + 2 H2 (g) → C4H3(g) Hint: write the balanced equations for the combustion reactions of C4H4, C4HS, and H2 6. Given the following data 2 CIF (g) + 02(g)→ Cl20(g) + F20(g) 2 CIF;(g) + 2 02(g) Cl20(g) + 3 F,0(g) 2 F,(g) + 02(g) → 2 F,0(g) AH = 167.4 kJ 341.4 kJ AH = -43.4 k] AH = Calculate AH for the reaction CIF(g) + F2(g) → CIF;(g) 7. A 30.0 g sample of water at 280. K is mixed with 50.0 g of water at 330. K. Calculate the final temperature of the mixture assuming no heat loss to the environment.
Transcribed Image Text:4. The enthalpy of combustion of CH:(g) when H20(1) is formed is -891 kJ/mol and the enthalpy of combustion of CH-(g) when H20(g) is formed is -803 kJ/mol. Use these data and Hess's law to determine the enthalpy of vaporization of water. 5. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for CAH4 (-2341 kJ/mol), CAH3 (-2755 kJ/mol), and H2 (-286 kJ/mol), calculate AH for the reaction C4H4(g) + 2 H2 (g) → C4H3(g) Hint: write the balanced equations for the combustion reactions of C4H4, C4HS, and H2 6. Given the following data 2 CIF (g) + 02(g)→ Cl20(g) + F20(g) 2 CIF;(g) + 2 02(g) Cl20(g) + 3 F,0(g) 2 F,(g) + 02(g) → 2 F,0(g) AH = 167.4 kJ 341.4 kJ AH = -43.4 k] AH = Calculate AH for the reaction CIF(g) + F2(g) → CIF;(g) 7. A 30.0 g sample of water at 280. K is mixed with 50.0 g of water at 330. K. Calculate the final temperature of the mixture assuming no heat loss to the environment.
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