a 150g-iron ball at 95 Celsius is dropped into a cavity in a block of ice.the cavity is then found to contain 21 g of water . CALCULATE THE HEAT OF FUSION OF ICE
(The specific heat capacity of iron is 0.11 cal/g x C degrees.)
To calculate the heat of fusion of ice, we need to follow these steps:
1. Calculate the heat absorbed by the iron ball to reach the temperature of the ice:
- Given mass of the iron ball: 150g
- Specific heat capacity of iron: 0.11 cal/g x C
- Change in temperature of the iron ball: 95°C (initial temperature) - 0°C (final temperature) = 95°C
- Q (heat absorbed) = mass × specific heat capacity × change in temperature
- Q = 150g × 0.11 cal/g x °C × 95°C
2. Calculate the heat released by the iron ball to cool down and reach the melting point of ice:
- Given mass of the iron ball: 150g
- Specific heat capacity of iron: 0.11 cal/g x C
- Q (heat released) = mass × specific heat capacity × change in temperature
- The final temperature at which the iron ball reaches the melting point of ice is 0°C, so the change in temperature is 95°C
- Q = 150g × 0.11 cal/g x °C × 95°C
3. Calculate the heat absorbed by the water during the phase change (melting of ice):
- Given mass of water: 21g
- The heat absorbed by the water during the phase change is equal to the heat released by the iron ball at the melting point of ice, since there is no change in temperature during the phase change.
- Q (heat absorbed) = heat released by iron ball = Q calculated in step 2
4. Calculate the heat of fusion of ice:
- Heat of fusion of ice = heat absorbed by the water / mass of water
- Heat of fusion of ice = Q / 21g
Now, you can plug in the calculated values and solve for the heat of fusion of ice.