A .250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g of water and 50 g of ice, both at 0 deg celcius. The reaction is:
2Na(s) + 2H2O(l) ---> 2NaOH(aq) + H2(g) .... delta H = -368 kJ
Assuming no heat loss to the surroundings, will the ice melt? Assuming the final temperature has a specific heat capacity of 4.18 J/g*deg C, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.