Question

1.

A 110.4 g110.4 g sample of a substance is initially at 20.1 °C20.1 °C . After absorbing 335 cal335 cal of heat, the temperature of the substance increases to 67.6 °C67.6 °C . What is the specific heat (SH)(SH) of the substance?

2.

When 165.0165.0 J of heat are added to a 15.015.0 g sample of mercury the final temperature of the mercury is recorded as 63.063.0 °C. The metal has a specific heat of 0.13950.1395 J/(g·°C).

3.

A solution is made by mixing 264.0 mL264.0 mL of ethanol initially at 13.4 ∘C13.4 ∘C with 264.0 mL264.0 mL of water initially at 21.5 ∘C21.5 ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL0.789 g/mL and the density of water is 1.00 g/mL1.00 g/mL. The specific heat of ethanol is 2.46 J/g⋅°C2.46 J/g·°C and the specific heat of water is 4.184 J/g⋅°C4.184 J/g·°C.

4.

After an afternoon party, a small cooler full of ice is dumped onto the hot ground and melts. If the cooler contained 8.90 kg8.90 kg of ice and the temperature of the ground was 38.0 °C,38.0 °C, calculate the energy that is required to melt all the ice at 0 °C.0 °C. The heat of fusion for water is 80.0 cal/g.

Thanks!

Answer 1