1. Calculate the value of ΔE in joules for a system that loses 50 J of heat and has 150 J of work performed on it by the surroundings. 2. What is the change in the internal energy of a system that absorbs 2,500 J of heat and that does 7,655 J of work on the surroundings in J? 3. The value of ΔH0 for the reaction is -126 kJ. Determine the amount of heat that is released by the reaction of 25.0 g of Na2O2 with water in kJ: 2Na2O2 (s) + 2H2O (l) → 2NaOH(s) + O2 (g)
1. Calculate the value of ΔE in joules for a system that loses 50 J of heat and has 150 J of work performed on it by the surroundings.
2. What is the change in the internal energy of a system that absorbs 2,500 J of heat and that does 7,655 J of work on the surroundings in J?
3. The value of ΔH0 for the reaction is -126 kJ. Determine the amount of heat that is released by the reaction of 25.0 g of Na2O2 with water in kJ: 2Na2O2 (s) + 2H2O (l) → 2NaOH(s) + O2 (g)
4. The value of ΔH0 for the reaction is -482 kJ. What is the heat released to the surroundings when 12.0 g of CO (g) reacts completely: 2CO(g) + O2(g) →2CO2(g) in kJ?
5. The value of ΔH0 for the reaction below is -186 kJ. Determine the heat released from the reaction of 25 g of Cl2: H2(g) + Cl2 → 2HCl(g) in kJ.
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