6.66. Use the 334 J/g (0.334 kJ/g) heat of fusion to calculate the heat of melting. Then use the heat of
melting to calculate Δt, the temperature change.
Heat of melting = x 31.5 g x 334 J
1 g
= 10521 J
Heat melting + heat warming = heat lost by 210 g H2O
Let t = the final temperature, and substitute into the above equation:
10521 J + 4.18 J1/ g • C x 31.5 g x (t − 0°C) = 4.18 J/1 g • Cx 210 g x (21.0°C − t)
Solve the above equation for t.
10521 J + 131.67t = 18433.8 J − 877.8t
t = 18433.8 J - 10521 J
(131.67 + 877.
J/°C
= 7.838 = 7.84°
for the +heat warming---> why is tfinal 0?