# Problem: A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0 ˚C. The reaction is2 Na (s) + 2 H2O (l) → 2 NaOH (aq) + H2 (g)          ΔH = -368 kJAssuming no heat loss to the surroundings, will the ice melt? Assuming the final mixture has a specific heat capacity of 4.18 J/g • ˚C, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.

###### FREE Expert Solution

Lets first answer the first question:

a. Assuming no heat loss to the surroundings, will the ice melt?

We can determine if the ice will melt by calculating the kJ produced once we dropped the Na metal

93% (236 ratings) ###### Problem Details

A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0 ˚C. The reaction is

2 Na (s) + 2 H2O (l) → 2 NaOH (aq) + H2 (g)          ΔH = -368 kJ

Assuming no heat loss to the surroundings, will the ice melt? Assuming the final mixture has a specific heat capacity of 4.18 J/g • ˚C, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.