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According to the first law of thermodynamics, what is the relationship between internal energy change (ΔE), heat (q), and work (w) for a system?
According to the first law of thermodynamics, what is the relationship between internal energy change (ΔE), heat (q), and work (w) for a system?
Which of the following is the correct definition of enthalpy (H) in thermodynamics?
Which of the following is the correct definition of enthalpy (H) in thermodynamics?
In a constant pressure process, the heat absorbed by a system is equal to the change in:
In a constant pressure process, the heat absorbed by a system is equal to the change in:
The calorific value of a fuel is defined as:
The calorific value of a fuel is defined as:
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The heat of reaction (ΔH) for a chemical reaction is equal to:
The heat of reaction (ΔH) for a chemical reaction is equal to:
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In an isothermal process, the change in internal energy (ΔE) of a system is:
In an isothermal process, the change in internal energy (ΔE) of a system is:
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What is the relationship between ΔH and ΔE in a chemical reaction?
What is the relationship between ΔH and ΔE in a chemical reaction?
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What is the significance of the heat of reaction in a chemical equation?
What is the significance of the heat of reaction in a chemical equation?
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What is the unit of heat of reaction (ΔH)?
What is the unit of heat of reaction (ΔH)?
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Why are the calorific values of gaseous fuels usually determined in constant volume calorimeters?
Why are the calorific values of gaseous fuels usually determined in constant volume calorimeters?
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What is the value of q in a constant volume calorimeter?
What is the value of q in a constant volume calorimeter?
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What is the value of ΔH for the reaction H2(g) + F2(g) → H2F2 (g) if ΔE = – 14.2 kcal/mole at 25º C?
What is the value of ΔH for the reaction H2(g) + F2(g) → H2F2 (g) if ΔE = – 14.2 kcal/mole at 25º C?
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According to the first law of thermodynamics, what is the change in internal energy (ΔE) for a process where a system absorbs 400 J of thermal energy from its surroundings?
According to the first law of thermodynamics, what is the change in internal energy (ΔE) for a process where a system absorbs 400 J of thermal energy from its surroundings?
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What is the maximum work done when pressure on 10 g of hydrogen is reduced from 20 to one atmosphere at a constant temperature of 273 K, given that the gas behaves ideally?
What is the maximum work done when pressure on 10 g of hydrogen is reduced from 20 to one atmosphere at a constant temperature of 273 K, given that the gas behaves ideally?
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Will there be any change in internal energy (ΔE) when the pressure on 10 g of hydrogen is reduced from 20 to one atmosphere at a constant temperature of 273 K?
Will there be any change in internal energy (ΔE) when the pressure on 10 g of hydrogen is reduced from 20 to one atmosphere at a constant temperature of 273 K?
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What is the heat content (q) of the system in a process where the pressure on 10 g of hydrogen is reduced from 20 to one atmosphere at a constant temperature of 273 K?
What is the heat content (q) of the system in a process where the pressure on 10 g of hydrogen is reduced from 20 to one atmosphere at a constant temperature of 273 K?
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What is the enthalpy (H) of a system at constant pressure?
What is the enthalpy (H) of a system at constant pressure?
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What is the difference between the heat content and enthalpy of a system?
What is the difference between the heat content and enthalpy of a system?
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