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Why heat capacity is so important in our everyday life? please give an examples.

Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter9: Energy For Today

Section: Chapter Questions

Problem 15E

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Explain the difference between heat capacity and specific heat of a substance.
High-quality audio amplifiers generate large amounts of heat. To dissipate the heat and prevent damage to the electronic components, heat-radiating metal fins are used. Would it be better to make these fins out of iron or aluminum? Why? (See Table 7- l for specific heat capacities.)
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.)
Calculate Suppose that two pieces of iron, one with amass exactly twice the mass of the other, are placed in aninsulated calorimeter. If the original temperatures of thelarger piece and the smaller piece are 90.0°C and 50.0°C,respectively, what is the temperature of the two pieceswhen thermal equilibrium has been established? Referto Table R-9 on page 975 for the specific heat of iron.
A 500.0-g sample of an element at 195C is dropped into an ice--water mixture; 109.5 g ice melts and an ice--water mixture remains. Calculate the specific heat of the element. See Exercise 131 for pertinent information.
Consider the following specific heats of metals. Metal Specific Heat copper 0.385 J/(gC) magnesium 1.02 J/(gC) Mercury 0.138 J/(gC) Silver 0.237 J/(gC) Four 25-g samples, one of each metal, and four insulated containers with identical water volumes, all start out at room temperature. Now suppose you add exactly the same quantity of heat to each metal sample. Then you place the hot metal samples in different containers of water (that all have the same volume of water). Which of the answers below is true? a The water with the copper will be the hottest. b The water with the magnesium will be the hottest. c The water with the mercury will be the hottest. d The water with the silver will be the hottest. e The temperature of the water will be the same in all the cups.
The temperature of the cooling water as it leaves the hot engine of an automobile is 240 F. After it passes through the radiator it has a temperature of 175 F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g oC.
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
A piece of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5 C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.7 C. When thermal equilibrium is reached, the final temperature is 24.3 C. Calculate the specific heat capacity of titanium.
What mass of carbon monoxide must be burned to produce 175 kJ of heat under standard state conditions?

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