How many kJ of heat are needed to completely melt 1.70 moles of H₂O,given that the water is at its melting point? The heat of fusion for water is 6.02 kJ/mole.

Question

Quizplus · Accepted Answer

To determine the amount of heat required to completely melt 1.70 moles of H₂O at the melting point of water, we use the equation: q = nΔHf where q is the heat required, n is the number of moles of H₂O, and ΔHf is the heat of fusion for water. Substituting the values given, we have: q = (1.70 mol) x (6.02 kJ/mol) q = 10.234 kJ Rounding to the appropriate number of significant figures gives 10.2 kJ, which is answer choice B.

How Many KJ of Heat Are Needed to Completely Melt