1. Calculate the change in total internal energy for a system that releases 2.38 × 104...
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Chemistry
1. Calculate the change in total internal energy for a systemthat releases 2.38 × 104 kJ of heat and does 6.80 ×104 kJ of work on the surroundings. Enter your answer inscientific notation.
2. In a gas expansion, 69 J of heat is absorbed by the system,and the energy of the system decreases by 114 J.
Calculate the work done.
3. Be sure to answer all parts. Given the thermochemicalequation for photosynthesis, 6H2O(l) +6CO2(g)→C6H12O6(s) +6O2(g) . ΔH = +2803 kJ/mol. Calculatethe solar energy required to produce 8503 g ofC6H12O6.
4. In a constant-pressure calorimetry experiment, a reactiongives off 23.8 kJ of heat. The calorimeter contains 150 g of water,initially at 25.4 c. What is the final temperature of the water?The heat capacity of the calorimeter is negligibly small.
5. A piece of silver with a mass 4.10 ×102 g has aheat capacity of 97.2 J/° C. What is the specific heat ofsilver?
1. Calculate the change in total internal energy for a systemthat releases 2.38 × 104 kJ of heat and does 6.80 ×104 kJ of work on the surroundings. Enter your answer inscientific notation.
2. In a gas expansion, 69 J of heat is absorbed by the system,and the energy of the system decreases by 114 J.
Calculate the work done.
3. Be sure to answer all parts. Given the thermochemicalequation for photosynthesis, 6H2O(l) +6CO2(g)→C6H12O6(s) +6O2(g) . ΔH = +2803 kJ/mol. Calculatethe solar energy required to produce 8503 g ofC6H12O6.
4. In a constant-pressure calorimetry experiment, a reactiongives off 23.8 kJ of heat. The calorimeter contains 150 g of water,initially at 25.4 c. What is the final temperature of the water?The heat capacity of the calorimeter is negligibly small.
5. A piece of silver with a mass 4.10 ×102 g has aheat capacity of 97.2 J/° C. What is the specific heat ofsilver?
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