how much energy in joules is required to melt 10.00 moles of ice
To find the amount of energy required to melt a certain number of moles of ice, you need to use the formula:
ΔH = moles × ΔHfus
ΔH represents the amount of energy (enthalpy) needed, moles is the number of moles of ice being melted, and ΔHfus is the molar enthalpy of fusion for ice.
The molar enthalpy of fusion for ice is commonly known as ΔHfus and its value is 6.02 kJ/mol. However, this value needs to be converted to joules since the answer should be in joules.
1 kJ = 1000 J
Therefore, 6.02 kJ/mol × 1000 J/kJ = 6020 J/mol.
Finally, you can calculate the amount of energy needed to melt 10.00 moles of ice:
ΔH = 10.00 moles × 6020 J/mol = 60,200 J.
So, 60,200 joules (J) of energy are required to melt 10.00 moles of ice.