If you have 0.301 m³ of water at 25.0 °C in an insulated container and add 0.142 m³ of water at 95.0 °C, what is the final temperature T, of the mixture? Use 1000 kg/m³ as the density of water at any temperature. T₁ = °C

One beaker contains 156 g of water at 20. °C, and a second beaker contains 76.8 g of water at 95 °C. The water in the two beakers is mixed. What is the final water temperature? Final water temperature = °C

A metal sample weighing 128.00 grams and at a temperature of 98.2 degrees Celsius was placed in 45.50 grams of water in a calorimeter at 22.8 degrees Celsius. At equilibrium the temperature of the water and metal was 35.6 degrees Celsius.  What is the change in temperature of the metal (in degrees C)? (Report this as a positive value)

A metal sample weighing 123.50 grams and at a temperature of 98.8 degrees Celsius was placed in 42.50 grams of water in a calorimeter at 20.1 degrees Celsius. At equilibrium the temperature of the water and metal was 38.4 degrees Celsius. What is the change in temperature of the water (in degrees C)? (Report this as a positive value) Your Answer:

A 8.0-kg rock is dropped from a height of 3.0 m. At what height is the rock's kinetic energy twice its potential energy?

14.0 g of cream at 20.3 °C are added to an insulated cup containing 100.0 g of coffee at 78.8 °C. Calculate the equilibrium temperature of the coffee. You may assume no heat is lost to the cup or surroundings, and that any physical properties of cream and coffee you need are the same as those of water. Be sure your answer has 3 significant digits. [°C x10 X S

A piece of cobalt (cp = 0.46 J/g⋅⋅°C) originally at 98.6 °C is placed into a coffee cup calorimeter containing 200.0 grams of water at 25.5 °C. The final temperature of the metal and water was 39.5 degrees Celsius.  What was the mass (g) of the piece of cobalt?  Do not type units into your answer.