Calculate the number of moles of ice in 10.0 g: The amount of heat required to melt 0.555 mol of ice at 0 C is equal to: Since this amount is greater than the amount added (of 0.850 kJ), some of the ice will melt as 0.850 kJ of energy are added, but the temperature will remain at 0 C. 91.
(the amount; added; ) (The amount of heat; required; ) (some of the ice; will melt; as 0.850 kJ of energy are added, but the temperature will remain at 0 C. 91) (The amount of heat required to melt 0.555 mol of ice at 0 C; are added; ) (The amount of heat required to melt 0.555 mol of ice at 0 C; is; equal to: Since this amount is greater than the amount added (of 0.850 kJ), some of the ice will melt as 0.850 kJ of energy are added, but the temperature will remain at 0 C. 91) (the temperature; will remain; at 0) (this amount; is; greater than the amount)
the amount The amount of heat some of the ice The amount of heat required to melt 0.555 mol of ice at 0 C The amount of heat required to melt 0.555 mol of ice at 0 C the temperature this amount
added required will melt are added is will remain is
as 0.850 kJ of energy are added, but the temperature will remain at 0 C. 91
equal to: Since this amount is greater than the amount added (of 0.850 kJ), some of the ice will melt as 0.850 kJ of energy are added, but the temperature will remain at 0 C. 91
at 0
greater than the amount