The question is how many kilojoules are required to melt 24g of ice at 100 degrees celsius?
Can you please correct me if im wrong. ( Which I'll probably will be )
I did:
24 x 333= 800kj
Melting does not occur at 100 C. It occurs at 0 C (with a small dependence upon pressure). Are you sure you do not want the heat required for vaporization? Or the heat required to melt ice at 0 C and heat the liquid to 100 C?
To correctly answer the question, we need to take into account the heating and melting processes involved. Let's break it down step by step:
1. Heating the ice from -100°C to 0°C:
To determine the energy required to heat the ice from -100°C to 0°C, we can use the specific heat capacity of ice. The specific heat capacity of ice is approximately 2.09 J/g°C.
So, the energy required to heat 24g of ice from -100°C to 0°C can be calculated as:
Energy = mass x specific heat capacity x change in temperature
Energy = 24g x 2.09 J/g°C x (0°C - (-100°C))
Since the ice is initially at -100°C, we have to account for the absolute value of the temperature difference:
Energy = 24g x 2.09 J/g°C x 100°C
Energy = 5028 J or 5.028 kJ
2. Melting the ice at 0°C:
Once the ice reaches 0°C, we need to calculate the energy required to melt it. The heat of fusion, also known as the latent heat of fusion for ice, is approximately 334 J/g.
Therefore, the energy required to melt 24g of ice can be calculated as:
Energy = mass x latent heat of fusion
Energy = 24g x 334 J/g
Energy = 8016 J or 8.016 kJ
Now, we add the energy required for heating and melting together:
Total energy required = Energy for heating + Energy for melting
Total energy required = 5.028 kJ + 8.016 kJ
Total energy required = 13.044 kJ
So, the correct answer is that approximately 13.044 kilojoules (kJ) are required to melt 24g of ice at 100 degrees Celsius.
It's great that you attempted the calculation, but the value you calculated, 800 kJ, is not correct. Remember to consider both the heating and melting processes.