A 40-g block of ice is cooled to -71°C and is then added to 570 g of water in an 80-g copper calorimeter at a temperature of 22°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 mice, final = g

In Dexter’s lab, he pours 1.65kg of molten gold at 1063°C into a 1.30kg iron cauldron filled with 2.70kg of water both at 15.0°C. At the same moment he drops a 0.400kg piece of ice initially at -20.0°C into the cauldron and begins to stir. If we treat the cauldron and its contents as a calorimeter, what will be the final temperature for the system in degrees Celsius?

A 2.35-kg sample of water at 18.8°C is in a calorimeter. You drop a piece of steel with a mass of 0.58 kg at 196°C into it. After the sizzling subsides, what is the final equilibrium temperature? (Make the reasonable assumptions that any steam produced condenses into liquid water during the process of equilibration and that the evaporation and condensation don't affect the outcome). Express your answer in °C, to at least one digit after the decimal point.

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?

A 40 g block of ice is cooled to -76°C and is then added to 610 g of water in an 80 g copper calorimeter at a temperature of 27°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.

Suppose that 0.95 g of steam (aka gaseous water), initially at 100 °C, condenses on a 75.0 g block of iron that is initially at 22 °C. What is the final temperature of the combined system when thermal equilibrium is reached?

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.

A 1.19-kg sample of water at 13°C is in a calorimeter. You drop a piece of steel with a mass of 0.31 kg at 224°C into it. After the sizzling subsides, what is the final equilibrium temperature? Make the reasonable assumptions that any steam produced condenses into liquid water during the process of equilibration and that the evaporation and condensation taken together don't affect the outcome, as we'll see later. Hint   The final equilibrium temperature of water and steel is °C. If the water is in a glass beaker with a mass of 0.2 kg, which in turn is in a calorimeter, with the beaker at the same temperature as the water, how will this affect the answer? Try answering before doing a detailed calculation.   Final temperature will be higher but not significantly so. Final temperature will be significantly lower. Final temperature will be lower but not significantly so. Final temperature will be significantly higher.   Using the setup in (b), the final equilibrium temperature of…

A 40-g block of ice is cooled to -76°C and is then added to 570 g of water in an 80-g copper calorimeter at a temperature of 28°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.) T₁ °℃ mice, final g

Your 500 cm3 soda is at 20° C so you add 100 g of ice which is at –20° C. Does all the ice melt? If so, what is the final temperature? If not, what fraction of the ice melts? Assume the cup is well–insulated and that the soda has the same thermal properties as liquid water.