Answer:
Step-by-step explanation:
The process can be broken down into two steps:
Heat required to raise the temperature of ice from -20°C to 0°C.
Heat required to melt ice at 0°C and raise the temperature of water from 0°C to 10°C.
Step 1:
The heat required to raise the temperature of ice can be calculated using the specific heat capacity of ice, which is 2.09 J/g°C.
Heat required = mass × specific heat capacity × change in temperature
Heat required = 10 g × 2.09 J/g°C × (0°C - (-20°C))
Heat required = 418 J
Step 2:
The heat required to melt ice and raise the temperature of water can be calculated using the heat of fusion of ice and the specific heat capacity of water.
Heat required to melt ice = mass × heat of fusion of ice
Heat required to melt ice = 10 g × 334 J/g
Heat required to melt ice = 3340 J
Heat required to raise the temperature of water can be calculated using the specific heat capacity of water, which is 4.18 J/g°C.
Heat required = mass × specific heat capacity × change in temperature
Heat required = 10 g × 4.18 J/g°C × (10°C - 0°C)
Heat required = 418 J
Total heat required = Heat required in Step 1 + Heat required to melt ice + Heat required in Step 2
Total heat required = 418 J + 3340 J + 418 J
Total heat required = 4176 J
Therefore, 4176 J of heat is required to change 10 g of ice at -20°C into water at 10°C.