Which statement is true of the internal energy of the system andits surroundings following a process in which ∆Esys = +65 kJ?Explain.a. The system and the surroundings both lose 65 kJ of energy.b. The system and the surroundings both gain 65 kJ of energy.c. The system loses 65 kJ of energy, and the surroundings gain65 kJ of energy.d. The system gains 65 kJ of energy, and the surroundings lose65 kJ of energy.

Q: The specific heat capacity of water (l) is 1.18 J/g∙℃. What is the molar specific heat capacity of…

A: Given:specific heat capacity of water (l) = 1.18 J/g∙℃.molar mass of water = 18.01 g/mol.

Q: Find the work energy, w, gained or lost by the system when a sample of gas expands from 10 L to 30 L…

A:

Q: The specific heat capacity of silver is 0.24 J/°C·g. Calculate the energy required to raise the…

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Q: 10. Explain enthalpy, entropy, and internal energy.

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Q: A 5.00 grams of LiOH is dissolved in 100.0 grams of water in a perfect calorimeter. Calculate the…

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Q: 22.8 g teaspoon made of stainless steel 304 (s = 0.5024 J g-1 K-1) originally at 10.°C is immersed…

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Q: The same quantity of energy is added to 25.0 g pieces of gold ( molar heat capacity y = 25.41 J/ mol…

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Q: A 1.72 g sample of the saccharide, C6H1206, shown below is combusted in a constant volume…

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Q: How many microstates are available to a substance in its liquid state

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Q: At constant pressure, which of these systems do work on the surroundings? O2 A(g) + 2 B(g) → 5C(g) O…

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Q: An imaginary machine takes 9,000 J of heat from a hot reservoir and 3,000 J of heat from a cold…

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Q: Which of the following statements correctly describe the second law of thermodynamics? I. Heat will…

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Q: 22. What is the change in internal energy (AE) when a system is heated with 35 J of energy while it…

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Q: The specific heat capacity of silver is 0.24 J/°C g. a. Calculate the energy required to raise the…

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Q: 20.) Calculate for the heat evolved in one mole of glucose (180.56 g/mol) if 3.00 g was ignited in a…

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Q: Which of the following represents a system that is exothermic and is doing work on the surroundings?…

A: Given information,     System is exothermic and doing work on the surroundings

Q: .

A: According to the first law of thermodynamics, the summation of heat gained or lost by the system and…

Q: A system expands from a volume of 1.00 L to 2.00 L against a constant external pressure of 1.00 atm.…

A:

Q: (a) Consider the following chemical reaction: 3Fe2O3(s) + CO(g) → 2Fe3O4(s) + CO2(g) ΔH = ? Use…

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Q: If the process is exothermic and not spontaneous, then what must be TRUE? O a. AS> 0 O b. AS0 O d.…

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Q: Calculate the work gained or lost by a system when a gas expands from 15 L to 40 L against a…

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Q: Which of the following statements correctly describe the second law of thermodynamics? I. Heat will…

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Q: Given the thermochemical formation reactions:   1/2 Br2(l) + F2(g) → BrF(g) ∆H˚ = -58. kJ   and…

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Q: A system goes from state 1 to state 2 and back to state 1. Suppose the changes in state are…

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Q: Consider heating 1.0 kg of water at a constant pressure of 1 atm. How much heat is needed to raise…

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Q: 2. A rubberized, cubic chamber was filled with butane gas and was expanded from 3.0L to 4.5L at a…

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Q: Without doing any calculations, match the following thermodynamic properties with their appropriate…

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Q: N2(g)2NO(g)++O2(g)O2(g)2N2O(g)→→→2NO(g),2NO2(g),2N2(g)+O2(g),ΔH=+180.7kJΔH=−113.1kJΔH=−163.2kJ use…

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Q: Consider the following thermochemical data: Cl2(g) → 2Cl(g) ΔH° = 242.3 kJ I2(g) → 2l(g) ΔH° =…

A:

Q: The molar heat capacity at constant pressure for CO2 is 36.61 J mol-1 K-1. How much heat in J is to…

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Q: At constant pressure, which of these systems do work on the surroundings?…

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A:

Q: If the process is exothermic and not spontaneous, then what must be TRUE? O a. AS0 O c. AH=0 O d.…

A:

Q: (1) What are the thermodynamic quantities of a system that affect the amount and sign of the…

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Q: Which of the following 1.00 mole of fossil fuel when burned (combustion in open atmospheres) will…

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A: Mg(s) + 2 H2O(l) ⟶ Mg(OH)2(s) + 2H2(g) | ∆Hrxn = —353.0 kJ/mol  99 mL of water temperature change =…