What amount of heat is needed to raise the temperature of a 12.7 g piece of aluminum (specific heat = 0.90 J/g°C) from 23.5°C to 72.0°C?

A 80.8 g chunk of granite (specific heat: 0.79 J/g°C) is heated to 225.7 °C and dropped into a beaker containing 150.0 g of methanol (specific heat: 2.549 J/g°C) at 27.1 °C.What will be the final temperature of the system after it reaches thermal equilibrium?

The specific heat capacity of liquid mercury is 0.14J/g-k. How many kilojoules of heat are needed to raise the temperature of 9.00g of mercury from 25.1°C to 65.3°C

When a  brass black was dropped into a 124-gram water, the water temperature increased from 21.0°C to 36.8°C. What is the heat capacity of the brass block? The initial temperature of the brass was 314.2°C and the specific heat of water is 4.184J/gk. If the mass of the brass block is 77.764g, what is the specific heat of the brass?

A 35.0 gram object has a specific heat of 0.832 Joules/gram °C. It gained 2095 Joules of heat from the surroundings. If it had started at 25.0 °C, what was the temperature of the object after it gained the heat from the surroundings? O 25.0 degrees Celsius O 3640 degrees Celsius O 71.9 degrees Celsius O 196.9 degrees Celsius O 1.74 degrees Celsius O 53.1 degrees Celsius O 96.9 degrees Celsius

A 325-g piece of gold at 427°C is dropped into 200.0 mL of water at 22.0°C. the specific heat of gold is 0.131 J/g°C. calculate the final temperature of the mixture. (assume no heat loss to the surroundings)

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0°C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.

A 146.3g piece of iron (specific heat = 0.449 J/g°C) is heated with a flame and dropped into a coffe cup calorimeter containing 450.0 g of water. the water (specific heat = 4.18 J/g°C) in the calorimeter increases from 20.3°C to 32.0°C. what was the initial temperature of iron?

If 31.1 calories of heat are added to a 25.0 g sample of iron (cFe = 0.450 J/g°C) at 32.1°C, what is the final temperature of the iron?