A 37 g sample of copper is at 22°C. If 821 J of energy are added to the copper, what is its final temperature? Assume the specific heat of copper is 387 J/kg x °C. Answer in units of °C

A sealed container holding 0.492 kg of liquid nitrogen at its boiling point of 77.3 K is placed in a large room at 23.2°C. Energy is transferred from the room to the nitrogen as the liquid nitrogen boils into a gas and then warms to the room's temperature. Liquid nitrogen has a latent heat of vaporization of 2.01 ✕ 105 J/kg. The specific heat of N2 gas at constant pressure is  cN2 = 1.04 ✕ 103 J/kg. K (a) Assuming the room's temperature remains essentially unchanged at 23.2°C, calculate the energy (in J) transferred from the room to the nitrogen. (b) Estimate the change in entropy of the room (in J/K).

A chunk of hot iron is pulled out of a fire and placed between aluminum vice grips.  The mass of the iron is 219 g and the mass of the aluminum is 66.4 g.  The iron is initially 351.8 °C.  The aluminum is initially 24.7 °C.  Assuming no loss of heat to the environment, what is the final temperature of the iron-aluminum system? I couldn't even get started on this one.

A 0.200-kg mass of metal with a specific heat of 1255.8 J/kg-°C, initially at 90°C, is placed in a 0.500-kg calorimeter, with a specific heat of 418.6 J/kg-°C, initially at 20°C. The calorimeter is filled with 0.100 kg of water, initially at 20°C. The specific heat of water is 4186 J/kg-°C. What is the final temperature once the combination of metal, calorimeter, and water reach equilibrium? O 70°C 40°C 60°C O 50°C

How much thermal energy (in J) is required to boil 2.45 kg of water at 100.0°C into steam at 135.0°C? The latent heat of vaporization of water is 2.26 ✕ 106 J/kg and the specific heat of steam is  2010  J kg · °C . HINT  J

While swimming, conduction can play a big role in heat loss from the body. The body of one swimmer has a total surface area of 1.80 m2 and an average thickness of 1.60 mm. The skin's thermal conductivity is 0.370 W/m-K. If the water's temperature is 20.0°C, and the blood reaching the inner surface of the skin is at 37.0°C, what is the rate of energy loss for that person through conduction?

Suppose you place 0.265 kg of 24.5°C water in a 0.45 kg aluminum pan with a temperature of 147.5°C, and 0.0125 kg of the water evaporates immediately, leaving the remainder to come to a common temperature with the pan. What would be the final temperature, in degrees Celsius, of the pan and water? The heat of vaporization of water is Lv = 2256 kJ/kg. You may neglect the effects of the surroundings and the heat required to raise the temperature of the vaporized water.  Te =

A 2.80-kg steel ball at 24.7°C is dropped from a height of 15.4 m into an insulated container with 4.50 L of water at 10.1°C. If no water splashes, what is the final temperature of the water and steel? The specific heat of steel and water is 450 J/(kg·K) and 4186 J/(kg·K) respectively.

How much thermal energy (in J) is required to boil 1.90 kg of water at 100.0°C into steam at 157.0°C? The latent heat of vaporization of water is 2.26 x 10° J/kg and the specific heat of steam is 2010 kg · °C HINT

An aluminum bar has a cross-section that is 5.07 cm by 6.38 cm and is 1.53 m long. Aluminum has a thermal conductivity of 205 W/m K. If the aluminum bar is used to bridge between ice at 0 °C and boiling water at 100 °C, what is the rate of heat transfer (in W) along the bar?