How much heat is necessary to change 345 g of ice at -11°C to water at 20°C
To calculate the amount of heat necessary to change ice at -11°C to water at 20°C, you need to consider three different heating stages:
1. Heating the ice from -11°C to 0°C.
2. Melting the ice at 0°C.
3. Heating the resulting water from 0°C to 20°C.
Let's calculate the heat required for each stage and then sum them up:
1. Heating the ice from -11°C to 0°C:
The specific heat capacity of ice is 2.09 J/g°C. To calculate the heat required to raise the temperature of 345 g of ice from -11°C to 0°C, use the formula:
Heat = mass * specific heat capacity * temperature change
Heat = 345 g * 2.09 J/g°C * (0°C - (-11°C))
2. Melting the ice at 0°C:
To calculate the heat required to melt the ice, we use the heat of fusion of ice, which is 333.55 J/g. The total heat required is given by:
Heat = mass * heat of fusion
Heat = 345 g * 333.55 J/g
3. Heating the resulting water from 0°C to 20°C:
The specific heat capacity of water is 4.18 J/g°C. To calculate the heat required to raise the temperature of 345 g of water from 0°C to 20°C, use the formula:
Heat = mass * specific heat capacity * temperature change
Heat = 345 g * 4.18 J/g°C * (20°C - 0°C)
Finally, add up the three stages to find the total heat required:
Total Heat = Heat Stage 1 + Heat Stage 2 + Heat Stage 3
By substituting the values and performing the calculations, you can find the total heat necessary to change the given amount of ice to water at the specified temperatures.