The average molar heat capacities of ice and water are 37.8 J/mol and ...
Calculation of Heat Required
To calculate the heat required to change 10g of ice at -10 degrees Celsius to water at 10 degrees Celsius, we need to use the following equation:
q = m * Cp * ΔT
- q = heat required (in Joules)
- m = mass of substance (in grams)
- Cp = specific heat capacity (in J/mol°C)
- ΔT = change in temperature (in °C)
Calculation of Heat Required to Melt Ice
First, we need to calculate the amount of heat required to melt the ice at -10 degrees Celsius:
q1 = n * ΔHf
- q1 = heat required to melt ice (in Joules)
- n = number of moles of ice
- ΔHf = enthalpy of fusion of ice (in J/mol)
As we have 10g of ice, we need to convert this to moles:
10g / 18.015 g/mol = 0.555 mol
Now, we can calculate q1:
q1 = 0.555 mol * 6012 J/mol = 3336.66 J
Calculation of Heat Required to Raise Temperature of Water
Next, we need to calculate the amount of heat required to raise the temperature of the water from 0 degrees Celsius to 10 degrees Celsius:
q2 = m * Cp * ΔT
- q2 = heat required to raise temperature of water (in Joules)
- m = mass of water (in grams)
- Cp = specific heat capacity of water (in J/mol°C)
- ΔT = change in temperature (in °C)
As we have melted 10g of ice, we now have 10g of water. Therefore, we can calculate q2:
q2 = 10g * (75.6 J/mol°C) * 10°C = 7560 J
Total Heat Required
Finally, we can calculate the total heat required:
q = q1 + q2 = 3336.66 J + 7560 J = 10896.66 J
Therefore, the answer is d) 1128 J is incorrect. The correct answer is a) 2376 J.