In a lab, a known metal with a known specific heat and mass was heated for 5 minutes in bunsen burner flame and then hung by nichrome wire in a cup of water with a known initial temp and mass.  The final temp of the water was then recorded and Joules of heat energy absorbed by water was calculated. amount of heat energy lost by metal = amount of heat energy gained by water.  Given a list of metals with specific heats
(Specific heats: water 4.18 copper .385, iron .444 and tungsten .134 J/gdegC)
31 grams of copper was heated for 5 minutes to 769degC and caused the water temp to raise from 18 to 29 degrees celsius mass of water was 196 g

Questions
1.which metal would raise the temperature of the water the greatest? the least and why?
2.Error is present in every experiment. In this experiment you neglected the small mass of water that was changed to steam when the hot sample was initially immersed in the water.  Would this tend to make the calculated temperature lower or higher than the actual temperature of the flame? Explain?
3.It takes about 2.26 kilojoules of energy to evaporate each gram of water. Suggest a way to include the evaporated water in your calculation.
4.Another error that was neglected comes from the small amount of hot nichrome wire that was also immersed in the water. Would this tend to make the calculated temperature lower or higher than the actual temperature of the flame? Explain. Assume metal was weighed before attaching the wire.