Which of the following best describes the Zeroth law of thermodynamics?

A. Energy cannot be created or destroyed, only transferred or converted.

B. The entropy of an isolated system always increases.

C. If two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other.

D. The energy of the universe is constant.

On which temperature scale is absolute zero equivalent to 0?

A. Celsius

B. Kelvin

C. Fahrenheit

D. Rankine

What is the primary difference between heat and temperature?

A. Heat is a form of energy, while temperature is a measure of energy.

B. Heat and temperature are the same thing.

C. Heat is a measure of energy, while temperature is the form of energy.

D. Heat is a measure of the average kinetic energy of particles, while temperature is the total energy of a system.

If a substance has a high heat capacity, it means that:

A. It can store a large amount of heat without a significant change in temperature.

B. Its temperature changes rapidly when heat is added.

C. It cannot store heat.

D. It has a low boiling point.

In a calorimetry experiment, if the water in the calorimeter gains heat, the sample:

A. Gains an equal amount of heat.

B. Loses an equal amount of heat.

C. Neither gains nor loses heat.

D. Loses more heat than the water gains.

a) Define temperature in terms of molecular activity. [2]

b) A metal rod is heated at one end and left to reach thermal equilibrium. Describe the molecular interpretation of what happens to the rod during this process. [3]

a) State the Zeroth law of thermodynamics. [2]

b) If two systems, A and B, are each in thermal equilibrium with a third system, C, but not necessarily with each other, what can be inferred about the thermal relationship between A and B? [2]

a) Differentiate between the Celsius, Kelvin, and Fahrenheit temperature scales in terms of their reference points. [3]

b) Convert a temperature of 100°C to Kelvin. [2]

a) Define heat capacity. [2]

b) A metal block of mass 500 g has a specific heat capacity of 0.9 J/g°C. If 450 J of heat is supplied to the block, calculate the temperature change of the block. [3]

c) How would the temperature change differ if the same amount of heat was supplied to a block of the same mass but with a specific heat capacity of 1.2 J/g°C? [2]

a) Explain the zeroth law of thermodynamics. [2]

b) If two systems A and B are in thermal equilibrium with a third system C, are A and B necessarily in thermal equilibrium with each other? Justify your answer. [2]

c) How does this law form the basis for temperature measurement? [3]

Which temperature scale has the smallest interval or degree size?

A. Celsius

B. Kelvin

C. Fahrenheit

D. All have the same interval size.

The molecular interpretation of temperature relates to:

A. The average potential energy of molecules.

B. The total kinetic energy of molecules.

C. The average kinetic energy of molecules.

D. The total potential energy of molecules.

If two objects are in thermal equilibrium with each other:

A. They are at the same temperature.

B. They have the same heat content.

C. They are of the same material.

D. They are of the same size.

Which of the following is NOT a unit of temperature?

A. Joule

B. Kelvin

C. Celsius

D. Fahrenheit

The impulse-momentum theorem relates:

A. Force to velocity.

B. Force to acceleration.

C. Force to time.

D. Force to displacement.

a) Differentiate between heat and temperature. [3]

b) A substance absorbs heat but does not show any change in temperature. Explain this phenomenon. [2]

c) How is this phenomenon utilised in the process of calorimetry? [3]

a) What is meant by the Fahrenheit scale of temperature? [2]

b) Convert a temperature of 212°F to the Celsius scale. [2]

c) Why is the Kelvin scale preferred in scientific studies over the Fahrenheit and Celsius scales? [3]

a) Explain how the kinetic theory of gases relates to temperature. [3]

b) A gas sample has an initial temperature of 300 K. If it is heated to 400 K while keeping the volume constant, calculate the final pressure of the gas using the ideal gas law equation, assuming the gas behaves ideally. (R = 8.314 J/(mol·K)) [3]

c) Why does the pressure of a gas increase when it is heated at constant volume, according to the kinetic theory of gases? [3]

d) Using a graph, illustrate how the pressure of a gas varies with temperature at constant volume according to the kinetic theory of gases. [1]

a) Define heat capacity and molar heat capacity. [3]

b) Calculate the heat capacity of a 25 g sample of water if it undergoes a temperature change of 10°C. The specific heat capacity of water is 4.18 J/(g·°C). [3]

c) Explain why substances with higher molar heat capacities require more energy to raise their temperatures compared to substances with lower molar heat capacities. [3]

d) Using a graph, compare the heat capacities of two substances, one with a high molar heat capacity and the other with a low molar heat capacity. [1]

a) Explain why the Kelvin scale is considered an absolute temperature scale. [3]

b) Calculate the temperature in Kelvin when a gas at -50°C is heated. [3]

c) Describe the relationship between Celsius and Kelvin temperatures. [3]

d) Using a graph, illustrate the relationship between Celsius and Kelvin temperatures. [1]