1. What does temperature measure?

2. Which of the following temperature scales is the SI unit?

3. A mercury thermometer shows a reading of -10°C. Which of the following thermometers could also accurately measure this temperature?

4. What is the primary factor determining the amount of heat required to change a substance's state (e.g., from solid to liquid)?

5. What is meant by 'thermal equilibrium'?

6. A blacksmith heats a piece of iron to shape it. Which statement explains why the iron becomes easier to work with when heated?

7. You want to design a container to keep food warm for a long time. What colour and surface finish would be the best choice for the container's exterior?

8. Why do you feel warmer when standing near a bonfire compared to standing the same distance away from a hot stove?

9. Explain why you feel a burning sensation when you touch a hot metal object.

10. Imagine you have two identical metal rods, one painted white and the other painted black. Both rods are exposed to direct sunlight for an hour. Which rod will be hotter? Explain why.

11. A recipe calls for 500 ml of water at 80°C. You only have water at 20°C. How much boiling water (100°C) should you mix with the 20°C water to achieve the desired temperature?

12. A 100g block of ice at 0°C is placed in 200g of water at 25°C. What will be the final temperature of the mixture, assuming no heat is lost to the surroundings? (Specific heat capacity of water = 4.2 J/g°C, latent heat of fusion of ice = 334 J/g).

13. 50g of ice at -10°C is heated until it completely changes to steam at 100°C. Calculate the total amount of heat energy required for this process. (Specific heat capacity of ice = 2.1 J/g°C, specific heat capacity of water = 4.2 J/g°C, latent heat of fusion of ice = 334 J/g, latent heat of vaporization of water = 2260 J/g).

14. A metal rod with a mass of 2 kg is heated from 20°C to 80°C. The rod absorbs 24,000 Joules of heat energy. Calculate the specific heat capacity of the metal.

15. A 100 g piece of metal at a temperature of 100°C is dropped into 200 g of water at 20°C. The final temperature of the mixture is 25°C. Assuming no heat is lost to the surroundings, calculate the specific heat capacity of the metal. (Specific heat capacity of water = 4.2 J/g°C).