A person makes ice tea by adding ice to 1.8 kg of hot tea, initially at 80°C. How many kilograms of ice, initially at 0.00°C, are required to bring the mixture to 10°C? The heat of fusion of ice is 334 kJ/kg, and we can assume that tea has essentially the same thermal properties as water, so its specific heat is 4190 J/(kg K).

A bullet made of silver (specific heat 234 J/kg deg C) traveling at 380 m/s hits a wooden post and stops. If 39% of the kinetic energy of the bullet becomes heat trapped in the bullet, what is the temperature change (in deg C) of the bullet? (Hint: you do not need the mass of the bullet, it cancels out)

A 0.0725 kg ice cube at −30.0°C is placed in 0.557 kg of 35.0°C water in a very well insulated container. What is the final temperature? The latent heat of fusion of water is 79.8 kcal/kg, the specific heat of ice is 0.50 kcal/(kg · °C), and the specific heat of water is 1.00 kcal/(kg · °C).

1.2-kg of ice at -6.0°C is dropped into 5.0 L (5.566-kg) of car coolant. The initial temperature of the coolant is 25.0°C. The ice and coolant are insulated, so energy transfers to the outside is negligible. After hours, all ice melts and the final temperature of the mixture of water-coolant is 1.8°C. The specific heat of ice is 2090 J/kg °C; the specific heat of water is 4186 J/kg °C; the latent heat of fusion for water is 334000 J/kg. A. What is the energy needed for heating the ice to 0 °C? B. Determine the energy needed to melt the ice into water. C. Determine the total energy needed to heat the -6.0°C ice to 1.8°C water. (Please note: the total energy also includes the part heating water from 0.0 °C to 1.8 °C.) D. Determine the specific heat capacity of the coolant.

When it rains, water vapor in the air condenses into liquid water, and energy is released. (a) How much energy is released when 0.0318 m (1.25 inch) of rain falls over an area of 2.59×106 m² (one square mile)? (b) If the average energy needed to heat one home for a year is 1.50x1011 J, how many homes could be heated for a year with the energy determined in part (a)? (a) Number (b) Number i i Units Units >

A blacksmith cools a chunk of iron initially at 650 degrees celsius by trickling water from a jug over it. The water in the jug has a temperature of 15 degrees celsius. All of the water boils away and the iron chunk cools down 120 degrees celsius. If, in total, he poured 0.90 kg of water over the iron, what is the mass of this chunk of iron?

Ice at 0 °C is placed in a Styrofoam cup containing 0.62 kg of lemonade at 32 °C. The specific heat capacity of lemonade is virtually the same as that of water; that is, c = 4180 J/(kg C°). After the ice and lemonade reach an equilibrium temperature, some ice still remains. The latent heat of fusion for water is Lf = 3.35 x 105 J/ kg. Assume that the mass of the cup is so small that it absorbs a negligible amount of heat, and ignore any heat lost to the surroundings. Determine the mass of ice that has melted, in grams.

A chunk of metal with a mass of 85.0 grams and a specific heat of 759 joules per kilogram·kelvin is heated to 78.9 degrees Celsius and placed in 122 milliliters of water (c = 4186 J/kg·K) at 18.6 degrees Celsius. What is the final temperature of the metal and water? Hint: The heat lost by the metal is gained by the water, so the sum of the heats is zero.

Problem 2: 0.4 kg of ice at – 10°C are mixed with 0.2 kg of water at 50°C. The water and ice are mixed in a calorimeter so that no heat escapes the system. The specific heat of ice is c; = 2090 J/(kg.°C), the la- tent heat of fusion of water is Lf = 3.33× 10° J/kg, and the specific heat of water is cu = 4186 J/(kg-°C). (a) What is the final temperature of the system? (b) How many kg of ice remain in the end? (c) How many kg of water remain in the end?

A 20-g ice cube floats in 150 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 86°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 x 105 J/kg and 4,186 J/kg °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg °C, respectively.) kg Need Help? Read It Master It