Suppose you mix 100.0 g of water at 22.8 oC with 75.0 g of water at 76.3  oC. What will be the final temperature of the mixed water, in oC?

The specific heat of ice is 2.10 kJ/kg °C, the heat of fusion for ice at 0 °C is 333.7 kJ/kg, the specific heat of water 4.186 kJ/kg °C, and the heat of vaporization of water at 100 °C is 2,256 kJ/kg. What is the final equilibrium temperature when 5.00 grams of ice at −15.0 °C is mixed with 40.0 grams of water at 75.0 °C?

0.595 g sample of steam at 107.4∘C is condensed into a container with 5.77g of water at 16.5∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 J g⋅∘C, the specific heat of steam is 2.01 Jg⋅∘C, and Δ𝐻vap=40.7 kJ/mol.

An insulated calorimeter contains 100 g of water at 22 °C. A chemical reaction causes the temperature to increase by 6 °C. What would be the final temperature of the water if the reactant concentration is cut in half (assume the same starting temperature of 22 °C). Group of answer choices28252231

A 100 g glass container is at 10.0 °C. 200 g of water at 90.0 °C is added to the glass container. What is the final temperature of the water and the glass, in °C? (specific heat of water = 1.00 cal/g °C, specific heat of glass = 0.200 cal/g °C)

A chemist mixes 500 g of lead at 500°C with 1,200 g of water at 20°C. She then mixes 500 g of copper at 500°C with 1,200 g of water at 20°C. The specific heat capacity of lead is 0.1276 J/g°C and the specific heat capacity of copper is 0.3845 J/g°C. What will be true about the final temperatures of the two systems?  A. The final temperature of the lead-water system will be equal to the final temperature of the copper-water system.  B. The final temperature of the lead-water system will be higher than the final temperature of the copper-water system.  C. The final temperature of the lead-water system will be lower than the final temperature of the copper-water system.  D. Cannot be determined from the given information.