A hot iron horseshoe (mass-0.4 kg), just forged, is dropped into 1.3 liter of water in a 0.3 kg iron pot initially at 200c. If the final equilibrium temperature is 25 °C, estimate the initial temperature of the hot horseshoe.

A 1500-W hotplate is used to heat up a 1.04kg aluminum pot filled with 1.22kg of water and a 0.855kg lead mass for 5 minutes. If the initial temperature of the system was 72 degrees F, find the final equilibrium temperature. Assume that all the energy of the hot plate goes into the system. (C water = 4180 J/kg*K , C aluminum - 910 J/kg*K, C lead = 160 J/kg*K).

Three moles of an ideal gas at 135C and 0.5 atm is allowed to expand 1 atm at a constant pressure to a volume twice as large. What is the new temperature?

What mass of water at 20.0°C must be allowed to come to thermal equilibrium with a 1.95-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 60.0°C? Assume any water turned to steam subsequently recondenses. kg

What mass of water at 20.0°C must be allowed to come to thermal equilibrium with a 1.90-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 70.0°C? Assume any water turned to steam subsequently recondenses. kg

a cup of coffee sits on a table in an insulated mug. to coool the coffee down a ice block is added. the inital mass of coffee in the mug is 90g. the intial temperature of the coffee is 90 degree celsius. the ice block has started to melt and is then put into the coffee. the ice melts and the new temperature of the cofee is 78 degree c and the new mass is 110g. the ice block (final-intital mass) is 20g. what are teh tempeartuare changes for the coffee and ice (started at 0 degree celsius) also if specific heat of water is used for both the coffee and ice waht is the heat energy lost by the coffee and the heat energy gained by the ice after it melted?