Temperature: Practice Questions

Which statement about the thermodynamic scale of temperature is correct?

A piece of ice of mass \(0.60\,\text{kg}\) at \(0^\circ\text{C}\) is added to \(2.0\,\text{kg}\) of water at \(25^\circ\text{C}\). The specific heat capacity of water is \(4200\,\text{J}\,\text{kg}^{-1}\,\text{K}^{-1}\) and the specific latent heat of fusion of ice is \(3.3 \times 10^5\,\text{J}\,\text{kg}^{-1}\).
Assuming no heat is lost to the surroundings, what is the final state of the system?

Two objects, X and Y, are in thermal equilibrium with each other. A third object, Z, is also in thermal equilibrium with Y. Which statement must be correct according to the laws of thermodynamics?

A mass of \(0.050\text{ kg}\) of ice at \(0^\circ\text{C}\) is added to \(0.20\text{ kg}\) of water at \(20^\circ\text{C}\) in a vacuum flask.
Specific latent heat of fusion of ice = \(3.3 \times 10^5\text{ J kg}^{-1}\)
Specific heat capacity of water = \(4200\text{ J kg}^{-1}\text{ K}^{-1}\)
What is the final temperature of the mixture?

The thermodynamic scale of temperature is an absolute scale. Which of the following is a defining characteristic of this scale?

Identify two physical properties, other than electrical resistance, that can be used as a thermometric property for the measurement of temperature.

State the temperature of absolute zero in degrees Celsius and describe the behavior of the molecules of an ideal gas at this temperature according to the kinetic model.

A resistance thermometer has a resistance of 50.00 \(\Omega\) at 0 \(^{\circ}\text{C}\) and 65.00 \(\Omega\) at 100 \(^{\circ}\text{C}\). Calculate the temperature in \(^{\circ}\text{C}\) when the measured resistance is 56.00 \(\Omega\), assuming resistance varies linearly with temperature.

A \( 800 \, \text{W} \) electric heater is used to heat a \( 0.45 \, \text{kg} \) block of ice initially at \( -15 \, ^\circ\text{C} \) until it becomes water at \( 30 \, ^\circ\text{C} \).
Given:
Specific heat capacity of ice = \( 2100 \, \text{J kg}^{-1} \, \text{K}^{-1} \)
Specific heat capacity of water = \( 4200 \, \text{J kg}^{-1} \, \text{K}^{-1} \)
Specific latent heat of fusion of ice = \( 3.34 \times 10^5 \, \text{J kg}^{-1} \)
(a) Define the term specific latent heat of fusion.
(b) Calculate the total energy required for this process.
(c) Calculate the time taken, assuming no heat is lost to the surroundings.

A piece of ice of mass 0.080 kg at \( -12^\circ\text{C} \) is placed in a well-insulated copper calorimeter of mass 0.15 kg containing 0.30 kg of water at \( 25^\circ\text{C} \).
Relevant data:
Specific heat capacity of ice = \( 2100 \text{ J kg}^{-1} \text{ K}^{-1} \)
Specific heat capacity of water = \( 4200 \text{ J kg}^{-1} \text{ K}^{-1} \)
Specific heat capacity of copper = \( 390 \text{ J kg}^{-1} \text{ K}^{-1} \)
Specific latent heat of fusion of ice = \( 3.3 \times 10^5 \text{ J kg}^{-1} \)
(a) Calculate the energy required to raise the temperature of the ice to \( 0^\circ\text{C} \) and then melt it completely.
(b) Determine the final temperature of the contents of the calorimeter once thermal equilibrium is reached.
(c) If the final temperature had been \( 0^\circ\text{C} \) with some ice remaining, describe how you would determine the mass of ice that had melted.