[ahawk1]

27.23 g of ice at -9.7°C is placed in 67.98 g of water at 98.3°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 J/K/mol and 75.3 J/K/mol, respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Calculate the final temperature. (You must answer in Kelvin, not °C.)


can someone start me off with a formula, thanks!

[Borek]

heat lost = heat gained

[ahawk1]

so is this correct?

qsolid+n(deltahfusion)+nch20(l)[Tf-(-9.7]=-(nch20(l)[Tf-98.3]
9.7*6.01*1.513+1.513*37.5+6.32[Tf+9.7]=-15.788[Tf-98.3]
87.41+6.32Tf+61.304=-15.788Tf+1551.96
22.108Tf=1403.246
Tf=63.472 degrees celsius or 336.47 degrees kelvin???

where did i go wrong?

[Borek]

qsolid+n(deltahfusion)+nch20(l)[Tf-(-9.7]=-(nch20(l)[Tf-98.3]

Explain symbols, I have no idea what is what of what.

[Tf-(-9.7]

Whatever the symbols are, this is wrong.