How much heat in calories would have to be added to 82 g of ice, initially at a temperature of -26°C to melt it completely(i.e. to turn it into water at 0°C)
Specific heat for ice is 0.5cal/g°C, latent heat of fusion is 80 cal/g , don't write the unit.
To find the amount of heat required to melt the ice, we need to consider two factors: the heat required to raise the temperature of the ice from -26°C to 0°C and the heat required for the phase change from solid to liquid.
First, let's calculate the heat required to raise the temperature of the ice from -26°C to 0°C:
Heat required = Mass * Specific heat * Change in temperature
Given:
Mass of ice = 82 g
Specific heat of ice = 0.5 cal/g°C
Change in temperature = 0°C - (-26°C) = 26°C
Heat required = 82 g * 0.5 cal/g°C * 26°C = 1073 cal
Next, let's calculate the heat required for the phase change from solid to liquid:
Heat required = Mass * Latent heat of fusion
Given:
Mass of ice = 82 g
Latent heat of fusion = 80 cal/g
Heat required = 82 g * 80 cal/g = 6560 cal
Finally, to find the total amount of heat required to melt the ice completely, we add the heat required for raising the temperature and the heat required for the phase change:
Total heat required = Heat required to raise temperature + Heat required for phase change
Total heat required = 1073 cal + 6560 cal = 7633 cal
Therefore, the amount of heat in calories that would have to be added to 82 g of ice to melt it completely is 7633 cal.