Reference no: EM132252052

1. A sample of a metal (10.0 g) is equilibrated at 70.0^oC and placed in water (10.0 g) at 18^oC in a calorimeter. The mixture equilibrated at 25^oC. Calculate the specific heat (s) of the metal.

Hint: assume that the heat energy lost by the metal is equal to that gained by the water.

Thus msDT (metal) = msDT (water)

2. Calculate the quantity of heat required to change the temperature of 150.0 g water from 25.0 to 75.0^oC.

C_swater 4.184 J/g^oC

3. Calculate the heat energy required to convert 100.0 g water at 100^oC to 100.0 g steam at 100^oC.

Heat of Vaporization water 40.7 kJ/mole. Note that this is energy per mole.

4. A 10 g ice cube at 0^oC is melted in 100 g water initially at 20^oC. The equilibrium temperature of the mixture is 10.93^oC.

Calculate:

a) The heat lost by the water. (the specific heat for water is 4.186 J/g·°C)

b) The heat absorbed by the ice to achieve melting.( It takes 334 J of heat energy to melt 1 g of ice).

c) The heat gained by the melted water of the ice cube. (the specific heat for ice is 2.093 J/g·°C).

5. When water is boiling, both the water and the steam released are at 100^oC. Why is a burn caused by the steam much worse than scalding by the boiling water?

6. Water and steam are both 100ºC when water is boiling, but a burn from steam is worse than a burn from the water. Why could this is the case.