A 1.00kg piece of metal at 52.0C is placed into 100. g of water at 10.0C. The final temperature of the water is 31.4C. Assuming a coffee cup calorimeter heat capacity of 42.0 J/C, calculate the specific heat of the metal. The specific heat of water is 4.18 J.gC.

A 28.602 g sample of a metal is heated to 99.9°C in a hot water bath until thermal equilibrium is reached. The sample is quickly transferred to 55.604 g of water at 22.6°C contained in a calorimeter. When thermal equilibrium is reached the temperature of the water is measured to be 27.3°C. What is the specific heat of the metal? Specific heat of water is 4.184 J/ grams•°C   In part A, (metal-water ) how was the initial temperature of WATER determined?   In part A, (metal-water ) how was the initial temperature of METAL determined?

A hot lump of 25.4 g of aluminum at an initial temperature of 83.0 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.

A 0.602-g sample of isophthalic acid (C8H604) is burned in a bomb calorimeter and the temperature increases from 24.80 °C to 27.05 °C. The calorimeter contains 1.01x10³ g of water and the bomb has a heat capacity of 936 1/°C. The heat capacity of water is 4.1843 g ¹¹. Based on this experiment, calculate AE for the combustion reaction per mole of isophthalic acid burned. 9 kJ/mol

7. In a calorimeter, 50.00 mL of 2.50 M NaOH was combined with 50.00 mL of 2.25 M HCI to form a solution. The temperature of the solution went from 20.0 °C to 36.0 °C. The heat capacity of the solution is 4.184 J/g°C. Assume a density of 1.00 g/mL Determine the AHneutzn of HCI.

A 77.5g piece of brass is heated so that its temperature is 98.7◦C. Next,it is quickly placed in a calorimeter containing 102.76 g of water at 18.5◦C.Knowing that the final temperature is 23.5◦C, what is the specific heat of this alloy?Note: Brass is an alloy of copper and zinc. From 98.7 to 23.5◦C, this alloy does not changeno phase, it remains in solid form.

A piece of lead (mass = 2.85 g) at 10.3 C is placed in a Styrofoam coffee cup containing 7.55 mL of water at 52.3 C. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature should be? The specific heat capacity of lead = 0.128 J/g°C and water = 4.18 J/g°C. density of water = 1.00 g/mL

A piece of titanium metal with a mass of 21.6 g is heated in boiling water to 99.5 °C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.8 °C. When thermal equilibrium is reached, the final temperature is 24.5 °C. Calculate the specific heat capacity of titanium. (The specific heat capacity of liquid water is 4.184 J/g. K.) Specific heat capacity= J/g. K

A 22.1g piece of aluminum (which has a molar capacity of 24.03 J/oC.mol) is heated to 82.4oC and dropped into a calorimeter containing water (specific heat capacity of water is 4.18J/goC) initially at 22.3oC. The final temperature of the water is 25.8oC. Ignoring significant figures, calculate the mass of the water in the calorimeter.

10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C