A 40 g block of ice is cooled to -75°C. and is then added to 570 g of water in an 80 g copper calorimeter at a temperature of 25°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. Remember that the ice must first warm to 0°C, melt, and then continue warming as water. The specific heat of ice is 0.500 cal/g °C = 2090 J/kg°C.

Liquid nitrogen is often used as an effective coolant, as its boiling temperature is 77.0 K. A 0.750 kg block of iron with an initial temperature of 313.27 K is immersed in an insulated bath of liquid nitrogen with an initial temperature of 77.0 K. After the iron and the liquid nitrogen reach a state of thermal equilibrium, the iron block has cooled to a final a temperature of 77.0 K, and 198 g of liquid nitrogen has boiled off (vaporized). Assuming that the specific heat of iron over this temperature range is is 285 J/kg·K, What is the latent heat of vaporization of liquid nitrogen?

An unknown substance has a mass of 0.250 kg and an initial temperature of 90.0°C. The substance is then dropped into a calorimeter made of aluminum containing 0.300 kg of water initially at 25.0°C (assume the water and calorimeter start in thermal equilibrium). The mass of the aluminum container is 0.200 kg, and the temperature of the calorimeter increases to a final equilibrium temperature of 32.0°C. Assuming no thermal energy is transferred to the environment, calculate the specific heat of the unknown substance.  The specific heat of water is 4186 J/(K*mol)  and aluminum is 900 J/(K*mol).

A 50.0 g copper calorimeter contains 290 g of water at 20.0°C. How much steam must be condensed into the water if the final temperature of the system is to reach 40.0°C?

A 155 g copper bowl contains 230 g of water, both at 20.0°C. A very hot 300 g copper cylinder is dropped into the water, causing the water to boil, with 4.05 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy (in calories) is transferred to the water as heat? 8.6 X kcal (b) How much energy (in calories) is transferred to the bowl? 55 X kcal (c) What is the original temperature of the cylinder? 553.6 X °C Did you use the idea of conservation of energy? That is, did you equate the sum of the energy transfers to zero? For the bowl and cylinder, did you substitute the expression relating an energy transfer, the specific heat, the mass, and the temperature change? For the water, did you use the same expression to get the water to the boiling point? Did you also include an expression for the heat of vaporization? Did you use the given final temperature for each of the three materials?

A 40-g block of ice is cooled to −69°C and is then added to 650 g of water in an 80-g copper calorimeter at a temperature of 23°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter. (If not all the ice melts, determine how much ice is left.) Remember that the ice must first warm to 0°C, melt, and then continue warming as water. (The specific heat of ice is 0.500 cal/g · °C = 2,090 J/kg · °C.) Tf = __ °C My answer of 33°C was incorrect.

Lead pellets, each of mass 1.90 g, are heated to 200°C. How many pellets must be added to 498 g of water that is initially at 20.0°C to make the equilibrium temperature 25.0°C? Neglect any energy transfer to or from the container. pellets Need Help? Read t

A 1.50-kg iron horseshoe initially at 650°C is dropped into a bucket containing 13.0 kg of water at 22.0°C. What is the final temperature of the water-horseshoe system? Ignore the heat capacity of the container and assume a negligible amount of water boils away. °C