Fig. 4.1 shows the particles (atoms) at one instant in a sample of iron at a temperature below its melting point. [Figure 4.1]

1. (a)(i)State the lowest possible temperature on the Celsius scale and on the Kelvin scale. Celsius scale ...................................... °C Kelvin scale ...................................... K[1]
2. (a)(ii)The temperature of the solid increases. The sample remains a solid. Describe how the motion of the particles changes.[2]
3. (a)(iii)The solid melts. State what happens to the internal energy and the temperature of the solid as it melts. internal energy ........................................................................................................................ temperature ........................................................................................................................[2]
4. (b)(i)A student: • places a 300g piece of iron in boiling water until the iron is at a temperature of 100°C • removes the iron from the water and places it immediately into 100g of water at 25°C. The iron cools and the water warms until both reach the same temperature, 44 °C. The specific heat capacity of water is 4.2 J/(g°C). No energy is lost to the surroundings. Calculate the change in energy (internal energy) of the water as it warms up. change in energy = ................................................. J[2]
5. (b)(ii)Calculate the specific heat capacity of iron. specific heat capacity = ................................................. J/(g°C)[2]

This question uses a diagram from the original paper, which isn't shown here. Open the full paper from the past papers archive to see it.