As a system decreases in volume, it releases 50.0 J of energy in the form of heat to the surroundings. The piston has an internal pressure of 0.500 atm. The final volume of the system is 42.0 L. What was the initial volume of the system if the internal energy of the system increased by 115.0 J?

A 75.0 mL of 2.0 M HNO3 at 25.0 °C is mixed with 75.0 mL of 2.0 M NaOH also at 25°C in a calorimeter. After the reactants are mixed by stirring, the temperature is observed to increase to 35.8 °C. Calculate the total energy formed from the reaction, and the energy per mole of the water produced?

 Given the following data:  Fe2O3(s)  + 3CO(g) —–> 2Fe(s) + 3CO2(g)         ΔH° = – 23 kJ  3Fe2O3(s) +  CO(g) ——> 2Fe3O4 (s) + CO2(g)    ΔH° = – 39 kJ   Fe3O4(s) +  CO(g) ——->  3FeO(s) + CO2(g)      ΔH° = – 18 kJ  Calculate the ΔH° for the reaction.  FeO(s)  + CO(g) ——–> Fe(s) + CO2(g) 

Consider the reaction:   2SO₂(g) + O₂(g) → 2SO₃(g)carried out at 25°C and 1 atm. Calculate ΔH°, ΔS°, and ΔG° using the following data:SubstanceΔH°f (kJ/mol)S° (J/K·mol)SO₂(g)-297248SO₃(g)-396257O₂(g)0205

 Given the following data:  Fe2O3(s)  + 3CO(g) —–> 2Fe(s) + 3CO2(g)         ΔH° = – 23 kJ  3Fe2O3(s) +  CO(g) ——> 2Fe3O4 (s) + CO2(g)    ΔH° = – 39 kJ   Fe3O4(s) +  CO(g) ——->  3FeO(s) + CO2(g)      ΔH° = – 18 kJ  Calculate the ΔH° for the reaction.  FeO(s)  + CO(g) ——–> Fe(s) + CO2(g) 

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Which time-management tool includes tracking your tasks, setting deadlines, and reviewing daily?

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According to the Yerkes-Dodson Law, optimal performance occurs at:

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