Substances Solids Aluminum Concrete Copper Glass Human Body (37°C) Iron, steel Liquids Water Mercury Specific heat (c) J/kg C 900 840 387 840 3500 452 4186 139 kcal/kg C 0.215 0.20 0.0924 0.20 0.83 0.108 1.000 0.0333

2900000 48 cal/g eat meat sheet of paper, solve the following problems. Note that quantity of heat energy required to change the phase of a substance is given by the following equation: Q = mL, where is the heat required, m is the mass, and L is the heat of fusion or vaporization. 1. How much energy is absorbed when 25.0 g of ice at 0.0°C melts to form water at 0.0°C? The heat of fusion of ice is 80 cal/g. 2. How much energy is absorbed when the water at 0.0°C in Question 1 is heated to 100.0°C? The specific heat of water is 1.0 cal/g °C. 3. How much energy is absorbed when the water at 100.0°C in Question 2 vaporizes to 100.0°C? The heat of vaporization of water is 540 cal/g. 4. The steam in Question 3 is used to melt ice. How much ice will be melted by the energy released by the condensation of the steam at 100.0°C?

G67

A glass coffee pot has a 9.00 cm diameter circular bottom in contact with a heating element that keeps the coffee warm with a continuous 50.0-W heat input. (a) What is the temperature of the bottom of the pot, if it is 2.90 mm thick and the inside temperature is 67.8°C? The thermal conductivity of the pot is 0.84 J/(s · m · °C). *Answer in °C, please

H78

The temperature of a 63 g sample of an unknown substance is raised from 28° C to 86° C when 390 calories of heat are added . What is the specific heat of the sample , in cal/g . C ? Enter your calculated value to the nearest .001 cal/g . C .

13. Solve

Water vapor at 100 degrees Celsius is put in contact with ice at 0 degrees Celsius and this mixture eventually results in 45 kg of liquid water at 30 degrees Celsius.  A. How many kilograms of ice were part of the mixture? B. How many kilograms of steam were part of the mixture?