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Questions and Answers
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?
- ΔE = w - q
- ΔE = q - w (correct)
- ΔE = -q - w
- ΔE = q + w
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?
- H = E - 2PV
- H = PV - E
- H = E + PV (correct)
- H = E - PV
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:
- volume (ΔV)
- internal energy (ΔE)
- pressure (ΔP)
- enthalpy (ΔH) (correct)
The calorific value of a fuel is defined as:
The calorific value of a fuel is defined as:
The heat of reaction (ΔH) for a chemical reaction is equal to:
The heat of reaction (ΔH) for a chemical reaction is equal to:
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:
What is the relationship between ΔH and ΔE in a chemical reaction?
What is the relationship between ΔH and ΔE in a chemical reaction?
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?
What is the unit of heat of reaction (ΔH)?
What is the unit of heat of reaction (ΔH)?
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?
What is the value of q in a constant volume calorimeter?
What is the value of q in a constant volume calorimeter?
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?
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?
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?
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?
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?
What is the enthalpy (H) of a system at constant pressure?
What is the enthalpy (H) of a system at constant pressure?
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?
