A 3.00kg block of lead (Clead=128 kg°C) initially at 30.00°C is placed in thermal contact with a 10.00kg block of germanium (Cgerm=322 kg°C) initially at 45.00°C. What is the final temperature of the blocks once they reach thermal equilibrium? O 67.73°C O 43.40°C O 35.96°C O-347.34°C O 38.55°C What assumption do we make when solving calorimetry problems like this? O The substances are in a closed, isolated container that does not allow any energy to enter or leave the system. O Some of the energy transferred from one substance is lost to its surroundings and does not go to the other substance. O The two substances must have different specific heats. O We can only have two substances in thermal contact.

6. 3.00 moles of Argon, a monatomic ideal gas, occupies a volume of 12.0 L at a temperature equal to 25.0° C. The gas then undergoes an isobaric expansion to 16.0 L. What is the heat absorbed by the gas? a. 3.25 kJ b. 5.17 kJ с. 6.19 kJ d. 7.38 kJ е. 8.60 kJ

Equal masses of substance A at 98.1°C and substance B at 26.2°C are placed in a well-insulated container of negligible mass and allowed to come to equilibrium. If the equilibrium temperature is 77.4°C, which substance has the larger specific heat? a) substance A     b) The answer depends on the exact initial temperatures. c) More information is required. d) The specific heats are identical.

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

A jet of steam at 100°C is applied to a 2.00 kg block of ice at 0°C. How many grams of steam would be required to completely melt the ice assuming a complete transfer of thermal energy? nA d bloow olle boutaig erd 15000 lo yolla an ai e W lobin bna 1900 lo yolla ns e losbinom 4

A copper sample (ccu = 387 J/kg•K) of mass mẹ = 75 g and temperature Te = 312ºC is dropped into a glass beaker that contains a mass of water me = 220 g (cw = 4190 J/kg•K). %3D The initial temperature of the water and the beaker is Tw,b = 12.0°C. What is the final temperature of the copper, beaker, and water? * The heat capacity (the specific heat times the mass) of the beaker is Cb' = 190 J/K.

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

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