A Level H1 Physics Thermal Physics Quiz

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A-Level Physics H1 Quiz - Thermal Physics

Name: ___________________________
Class: ___________________________
Date: ___________________________
Score: _______ / 40

Duration: 50 minutes
Total Marks: 40
Topic: Thermal Physics

Instructions:

• Answer all 20 questions.
• Show your working clearly for calculation questions.
• Use the provided space to write your answers.
• Marks for each question are shown in brackets [ ].

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Section A: Definitions and Concepts (Questions 1–5)

1. State what is meant by thermal equilibrium. [1]

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2. Define specific heat capacity. [2]

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3. A metal block and a wooden block are both at 20 °C. Explain why the metal block feels colder to touch than the wooden block although both are at the same temperature. [2]

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4. State the principle of conservation of energy as applied to heating. [1]

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5. Define latent heat of vaporisation. [2]

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Section B: Calculations (Questions 6–12)

6. Calculate the heat energy required to raise the temperature of 0.50 kg of water from 20 °C to 100 °C. Specific heat capacity of water = 4200 J kg⁻¹ °C⁻¹. [2]

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7. A 2.0 kg aluminium block (specific heat capacity = 900 J kg⁻¹ °C⁻¹) cools from 80 °C to 30 °C. Calculate the heat lost. [2]

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8. An electric heater supplies 500 W of power to 1.0 kg of oil. The temperature rises from 25 °C to 45 °C in 4.0 minutes. Calculate the specific heat capacity of the oil. [3]

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9. 0.20 kg of ice at 0 °C is converted completely to water at 0 °C. The latent heat of fusion of ice is 3.34 × 10⁵ J kg⁻¹. Calculate the energy absorbed. [2]

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10. A substance of mass 0.40 kg undergoes boiling at constant temperature. It absorbs 1.20 × 10⁵ J. Determine the latent heat of vaporisation. [2]

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11. A 1.5 kg copper block (c = 390 J kg⁻¹ °C⁻¹) at 100 °C is placed into 2.0 kg of water at 20 °C in a container of negligible heat capacity. Calculate the final equilibrium temperature. [3]

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12. A heating coil rated 240 V, 0.50 A is used to heat 0.30 kg of water. Assuming all electrical energy becomes heat, calculate the temperature rise in 2.0 minutes. (c_water = 4200 J kg⁻¹ °C⁻¹) [3]

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Section C: Data Interpretation and Structured Response (Questions 13–20)

13. The graph below shows the temperature of a substance as it is heated at a constant rate.

Image pending generation: graph for Q13.

(a) State the temperature at which the substance is undergoing a change of state. [1]
(b) Explain why the graph is horizontal during the plateau. [2]

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14. Describe an experiment to determine the specific heat capacity of a liquid using an electrical method. Include the measurements needed. [4]

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15. A student claims: "When water boils, its temperature increases rapidly because a lot of heat is supplied." Explain why this statement is incorrect. [2]

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16. The table shows masses and temperature changes for four metals each given the same heat energy.

Metal	Mass (kg)	ΔT (°C)	c (J kg⁻¹ °C⁻¹)
A	0.10	10	400
B	0.20	5	400
C	0.10	20	200
D	0.40	5	200

(a) Calculate the heat energy supplied to Metal A. [1]
(b) State which metal received the same heat energy as A. Show your reasoning. [2]

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17. A room contains air at 25 °C. A steel spoon and a plastic spoon are both at 25 °C. Explain, using the concept of thermal conductivity, why the steel spoon feels cooler. [2]

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18.

Image pending generation: experimental_setup for Q18.

Using the setup above, calculate the specific heat capacity of the metal cylinder. [3]

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19. State two assumptions made when using the method of mixtures to find specific heat capacity. [2]

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20. A sample of 0.10 kg of a liquid is cooled from 50 °C to 30 °C, releasing 4200 J. A second sample of the same liquid of mass 0.20 kg is cooled from 60 °C to 20 °C. Calculate the heat released by the second sample. [3]

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A-Level Physics H1 Quiz - Thermal Physics (Answer Key)

Total Marks: 40
Topic: Thermal Physics

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Section A: Definitions and Concepts

Q1 [1 mark]
Thermal equilibrium is the state when two or more bodies in thermal contact have the same temperature and there is no net flow of heat between them.
Teaching note: Heat flows from higher to lower temperature. At equilibrium, temperatures equalise and heat transfer stops.

Q2 [2 marks]
Specific heat capacity is the amount of heat energy required to raise the temperature of 1 kg of a substance by 1 °C (or 1 K).
Marking: [B1] definition of per unit mass; [B1] per unit temperature rise.
Teaching note: Formula: $c = \frac{Q}{m\Delta T}$.

Q3 [2 marks]
Metal has higher thermal conductivity than wood [B1]. It conducts heat away from the hand faster, making it feel colder [B1].
Teaching note: Both are at same temperature; sensation is due to rate of heat transfer, not temperature difference.

Q4 [1 mark]
Energy supplied as heat = energy gained by substance (assuming no losses). Total energy is conserved.

Q5 [2 marks]
Latent heat of vaporisation is the heat energy required to change 1 kg of a substance from liquid to vapour at constant temperature.
Marking: [B1] change of state liquid→vapour; [B1] per unit mass at constant T.

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Section B: Calculations

Q6 [2 marks]
$Q = mc\Delta T = 0.50 \times 4200 \times (100-20) = 0.50 \times 4200 \times 80 = 168000$ J = $1.68 \times 10^5$ J.
Marking: [M1] correct formula; [A1] correct value.
Teaching note: ΔT = 80 °C.

Q7 [2 marks]
$Q = mc\Delta T = 2.0 \times 900 \times (80-30) = 2.0 \times 900 \times 50 = 90000$ J = $9.0 \times 10^4$ J lost.
Marking: [M1] formula; [A1] answer.

Q8 [3 marks]
Energy supplied: $E = Pt = 500 \times (4.0 \times 60) = 500 \times 240 = 120000$ J.
$\Delta T = 45 - 25 = 20$ °C.
$c = \frac{E}{m\Delta T} = \frac{120000}{1.0 \times 20} = 6000$ J kg⁻¹ °C⁻¹.
Marking: [M1] E = Pt; [M1] substitution; [A1] c = 6000.

Q9 [2 marks]
$Q = mL = 0.20 \times 3.34 \times 10^5 = 6.68 \times 10^4$ J.
Marking: [M1] formula; [A1] answer.

Q10 [2 marks]
$L = \frac{Q}{m} = \frac{1.20 \times 10^5}{0.40} = 3.00 \times 10^5$ J kg⁻¹.
Marking: [M1] formula; [A1] answer.

Q11 [3 marks]
Heat lost by Cu = heat gained by water:
$1.5 \times 390 \times (100 - T) = 2.0 \times 4200 \times (T - 20)$
$585(100 - T) = 8400(T - 20)$
$58500 - 585T = 8400T - 168000$
$226500 = 8985T$
$T = 25.2$ °C.
Marking: [M1] equating heats; [M1] algebra; [A1] T = 25.2 °C.

Q12 [3 marks]
Electrical energy: $E = VI t = 240 \times 0.50 \times 120 = 14400$ J.
$\Delta T = \frac{E}{mc} = \frac{14400}{0.30 \times 4200} = \frac{14400}{1260} = 11.4$ °C.
Marking: [M1] E = VIt; [M1] ΔT formula; [A1] 11.4 °C.

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Section C: Data Interpretation and Structured Response

Q13 [3 marks]
(a) 60 °C [1]
(b) During plateau, heat energy is used for latent heat of fusion/vaporisation (state change) not to raise temperature [B1]; temperature stays constant until phase change complete [B1].

Q14 [4 marks]

• Use insulated beaker with liquid of known mass m. [B1]
• Immersed heater of known power P, stir, record initial T_i. [B1]
• Heat for time t, record final T_f. [B1]
• Calculate $c = \frac{Pt}{m(T_f - T_i)}$, assuming no losses. [B1]
  Teaching note: Measurements: m, P, t, T_i, T_f.

Q15 [2 marks]
Incorrect because during boiling temperature remains constant [B1]; supplied heat is latent heat for state change, not temperature rise [B1].

Q16 [3 marks]
(a) $Q_A = mc\Delta T = 0.10 \times 400 \times 10 = 400$ J [1]
(b) Metal B: $0.20 \times 400 \times 5 = 400$ J [B1]; same as A [B1].

Q17 [2 marks]
Steel has higher thermal conductivity [B1]; draws heat from skin faster so feels cooler [B1].

Q18 [3 marks]
Heat to water: $Q_w = m_w c_w \Delta T = 0.50 \times 4200 \times (28-20) = 0.50 \times 4200 \times 8 = 16800$ J.
Electrical energy: $E = Pt = 60 \times 300 = 18000$ J.
Heat to metal: $Q_m = 18000 - 16800 = 1200$ J.
$c = \frac{Q_m}{m\Delta T} = \frac{1200}{0.80 \times 8} = 187.5$ J kg⁻¹ °C⁻¹.
Marking: [M1] water heat; [M1] metal heat; [A1] c = 187.5.

Q19 [2 marks]

• No heat loss to surroundings / container. [B1]
• Substances uniformly mixed / same final temperature. [B1]

Q20 [3 marks]
For first: $c = \frac{4200}{0.10 \times 20} = 2100$ J kg⁻¹ °C⁻¹.
Second: $Q = 0.20 \times 2100 \times (60-20) = 0.20 \times 2100 \times 40 = 16800$ J.
Marking: [M1] find c; [M1] use for second; [A1] 16800 J.