# Specific Heat

### Topic Page

Specific Heat### Questions

- How can specific heat be used to identify substances?
- How can the heat capacity of a lead sinker be determined?
- How do the specific heats of metals compare with water?
- How does specific heat change with temperature?
- Dissolving some potassium bromide in 200cm3 of water leads to a decrease in temperature of 3oC. What will the heat released be?
- Is heat capacity larger for polymers?
- Why is heat capacity an extensive property?
- Why does heat capacity change with temperature?
- What is specific heat measured in?
- What is heat capacity measured in?
- What is the heat capacity formula?
- How does specific heat change with pressure?
- How does specific heat affect temperature?
- How does salt change the specific heat capacity of water?
- How does heat capacity change with temperature?
- How do you write specific heat mathematically?
- How can I calculate the specific heat of aluminum?
- How can I calculate specific heat capacity of water?
- How do specific heats of metal compare to that of water?
- How can specific heat capacity be used?
- How can specific heat capacity be measured?
- Does specific heat change with volume?
- Does specific heat change with molarity?
- Does heat capacity change with volume?
- Does heat capacity change with mass?
- What is an example of a heat capacity practice problem?
- What is heat capacity?
- Can you go over #q = m * c * DeltaT# ?
- Question #f6c38
- Question #5ef67
- Question #e51aa
- Question #0efc9
- Question #9a262
- The specific heat capacity of platinum is 0.032 cal/g·K. How to calculate the heat, in joules, necessary to raise the temperature of a sample of platinum weighing 20.0 g from 15.0 Celsius to 65.0 Celsius?
- How much energy will be required to heat a #"1.0 kg"# mass of water from #25^@"C"# to #99^@"C"#?
- The amount of energy needed to heat 2.00 g of carbon from 50.0°C to 80.0°C is 42.6 J. The specific heat capacity of this sample of carbon is ?
- Question #431a4
- How much heat, in joules and in calories, must be removed from 1.75 mol of water to lower its temperature from 25 degree celsius to 15 degree celsius?
- Question #b10d9
- Question #94dc7
- Question #42d33
- Question #f9d73
- The specific heat of wood is 2.03 J/g C. How much heat is needed to raise the temperature of 550 g of wood from -15.0 C to 10.0 C?
- Question #0ee35
- Question #0c7c3
- Question #d5fe2
- Question #c1015
- Question #23a55
- Which heats up faster, wood or glass?
- Question #8a949
- What is the specific heat capacity of lead?
- A gold ring weighing 20 g at 25 °C is dropped into a beaker containing 15 g of boiling water. The final temperature of the water is 97 °C. Recall that the heat capacity of water is 4.184 J/g °C. What is the specific heat capacity of gold?
- What is the specific heat of aluminum ?
- How could specific heat be potentially useful to a biological system or organism?
- The temperature of a piece of copper with a mass of 95.4 g increases from 25°C to 48°C when the metal absorbs 849 J of heat. What is the specific heat of copper?
- If the specific heat of mercury is 0.14 J/g°C, how much heat is required to raise the temperature of 250.0g of mercury from 10°C to 62°C?
- What is the specific heat of a material if a 6.0 g sample absorbs 50 J when it is heated from 30°C to 50°C?
- What is the specific heat of a substance that absorbs #2.5*10^3# joules of heat when a sample of #1 * 10^4# g of the substance increases in temperature from 10°C to 80°C?
- Question #39f99
- Why does the sand on a beach cool down at night more quickly than the ocean water?
- Question #06850
- The same amount of heat which will change the temperature of 50.0 g of water by 4.5° C will raise the temperature of 110.0 g of tin from 25° C to 62.7° C. What is the specific heat of tin?
- A sample of an unknown metal has a mass of 120.7 g. As the sample cools from 90.5 °C to 25.7 °C, it releases 7020 J of energy. What is the specific heat of the sample?
- Question #a0c8b
- Question #44228
- Why is water often used as a coolant?
- Question #f723a
- The temperature of a sample of water changes from 10° C to 20°C when the sample absorbs 418 joules of heat. What is the mass of the sample?
- Two substances have the same mass and are both initially at 200°C. They both absorb 150 J of energy. Which substance will have the higher temperature, the one with the higher or the lower specific heat?
- The specific heat of concrete is greater than that of soil. Given this fact, would you expect a major-league baseball field or the parking lot that surrounds it to cool off more in the evening following a sunny day?
- What instrument can be used to calculate specific heat capacity?
- The temperature of a sample of water changes from 10°C to 20°C when the water absorbs 420 joules of heat. What is the mass of the sample?
- What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample by 15° C?
- When you use a microwave oven to increase the temperature of a cup of hot chocolate, which type of heat transfer is taking place?
- 25.0 g of mercury is heated from 25°C to 155°C, and absorbs 455 joules of heat in the process. What is the specific heat capacity of mercury?
- How do you calculate the specific heat capacity of a piece of wood if 1500.0 g of the wood absorbs #6.75 * 10^4# joules of heat, and its temperature changes from 32°C to 57°C?
- A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. What is the specific heat capacity of iron?
- How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C?
- Question #72765
- What is the specific heat of lead if 30.0 g of lead undergoes a 250.0°C change while absorbing 229.5 calories?
- If you add large amounts of heat to a liquid, what could happen?
- What quantity of heat energy must have been applied to a block of aluminum weighing 42.7 g if the temperature of the block of aluminum increased by 15.2°C?
- If 69.5 kJ of heat is applied to a 1012-g block of metal, the temperature of the metal increases by 11.4°C. What is the specific heat capacity of the metal in J/g°C?
- Why is water in a glass cup quickly warmed in a microwave oven, but the glass cup itself warms much more slowly, if at all?
- What is the heat capacity of a piece of wood if 1500 g of the wood absorbs 67,500 joules of heat, and its temperature changes from 32°C to 57°C?
- It takes 23.5 kJ of heat energy to raise the temperature of 100 g of a substance by 50°C. What is the substance?
- When 2211 J of heat energy is added to 47.7 g of ethanol, #C_2H_6O#, the temperature increases by 18.9°C. What is the molar heat capacity of #C_2H_6O#?
- Question #16930
- Question #5dc43
- Question #1dcd8
- On a night at the beach, which would you expect to cool faster: the ocean water or the beach sand?
- What is the specific heat capacity of a 50-gram piece of 100°C metal that will change 400 grams of 20°C water to 22°C?
- Question #02440
- Question #89fac
- It takes 770 joules energy to raise the temperature of 50.0 g of mercury by 110°C. What is the specific heat of mercury?
- When 1942 J of heat energy is added to 47.4 g of ethanol, #C_2H_6O#, the temperature increases by 16.7 °C. What is the molar heat capacity of #C_2H_6O#?
- When 435 J of heat is added to 3.40 g of olive oil at 21.0°C, the temperature increases by 85°C. What is the specific heat of the olive oil?
- Question #3a69a
- What is the specific heat of an unknown substance if 2000 J of energy are required to raise the temperature of 400 grams of the substance 45 degrees Celsius?
- The amount of heat needed to raise the temperature of 25 g or a substance by 15°C is 915 J. What is the specific heat of the substance?
- Do all non-conductors of heat have a specific heat of zero?
- Which will normally warm faster: a black pot of cold water or a silvered pot of cold water? Which will cool faster?
- Question #cb41a
- How do we find the change in heat in a chemical reaction?
- The temperature of a sample of iron with a mass of 10.0 g changed from 50.4°C to 25.0°C with the release of 114 J of energy. What is the specific heat of iron?
- Solid aluminum has a specific heat of 0.89 J/g oC, and a heat of fusion of 398 J/g. Aluminum melts at 660.4oC. How much heat is required to convert a 10.0 g sample of aluminum metal at 580.0oC to a fully-molten sample of liquid at 660.4oC?
- A sample of mercury absorbed 257 J of heat and its mass was .45 kg. If it's temperature increased by 4.09 K, what is its specific heat in J° / kg K?
- It takes 3,190 J to increase the temperature of a 0.400 kg sample of glass from 273 K to 308 K. What is the specific heat for this type of glass?
- What is the specific heat of copper metal?
- A 50.0 g sample of an unknown substance absorbed 1.64 kJ of energy as it changed from a temperature of 36°C to 98°C. What is the specific heat of the unknown substance in J/g°C?
- Why does it take so much energy to heat liquid water?
- If it takes 41.72 joules to heat a piece of gold weighing 18.69 g from 10.0°C to 27.0°C, what is the specific heat of the gold?
- A sample of an unknown substance has mass of 89.5 g. If 345.2 J of heat are required to heat the substance from 285 K to 305 K, what is the specific heat of the substance?
- The specific heat of ice is 0.5 calories/gram°C? 20 grams of ice will require how many calories to raise the temperature 1°C?
- What amount of energy is required to melt a 10.7 g piece of ice at 0 C? The heat of fusion of ice = 333 Jg-1
- What is the final equilibrium temperature when 20.00 grams of ice at -15.0°C is mixed with 5.000 grams of steam at 120.0°C?
- How many grams of formaldehyde are needed to produce enough heat in a combustion reaction to change 10.00g of ice to steam at 100 degrees C?
- A 40 g block of ice is cooled to -76°C. and is then added to 640 g of water in an 80 g copper calorimeter at a temperature of 28°C. What is the final temperature of the system consisting of the ice, water, and calorimeter?
- What quantity of heat is necessary to convert 50 g of ice at 0 degrees C into steam at 100 degrees C?
- A 31 g ice cube at its melting point is dropped into an insulated container of liquid nitrogen. How much nitrogen evaporates if it is at its boiling point of 77 K and has a latent heat of vaporization of 200 kJ/kg?
- Given the following what is the specific heat capacity of ice if the specific heat capactiy of liquid water is 4.2 J/g/degrees C?
- A 0.003 0-kg lead bullet is traveling at a speed of 240 m/s when it embeds in a block of ice at 0°C. If all the heat generated goes into melting ice, what quantity of ice is melted?
- What is specific heat of steam?
- Specific heat of ice in #"J/kg K"#?
- What is the specific heat of ice in j/gc?
- What is the specific heat of ice in joules?
- What is the specific heat of ice at #0^oC#?
- How do you determine the specific heat of ice?
- How do specific heats of ice liquid, water, and steam compare?
- How do you calculate the specific heat capacity of ice?
- What is specific latent heat?
- What is the specific heat of ice at 0 degrees Celsius?
- What is the specific heat of ice in calories?
- A 36.07 g sample of a substance is initially at 27.8°C. After absorbing 2639 J of heat, the temperature of the substance is 109.0°C. What is the specific heat of the substance?
- Ten grams of iron cooled from 60.4 °C to 35.0°C, and released 114 J of heat in the process. What is the specific heat of iron?
- What is the specific heat capacity of a metal if it requires 178.1 J to change the temperature to 15.0 g of the metal from 25.00 C to 32.00 C?
- How much heat is liberated by the combustion of 206 g of hydrogen? #DeltaH_(comb)# = -286 kJ/mol
- You are given the following two equations. How do you calculate #DeltaH# for this reaction: #Sn(s) + 2Cl_2(g) -> SnCl_4 (l)#?
- When 435 J of heat is added to 3.4 g of olive oil at 21 C, the temperature increases to 85 C. What is the specific heat of the olive oil?
- What does the specific heat for a substance indicate?
- What expression represents the #DeltaH# for a chemical reaction in terms of the potential energy, #E#, of its products and reactants?
- How would you calculate #DeltaE# of a gas for a process in which the gas absorbs 35 J of heat and does 8 J of work by expanding?
- What is the specific heat of a substance?
- What is the heat required to raise #"1 g"# of a sample by #1^@"C"#?
- 31.5 grams of an unknown substance is heated to 102.4 C and then placed into a calorimeter containing 103.5 grams of water at 24.5 C. If the final temperature reached in the calorimeter is 32.5 C, what is the specific heat of the unknown substance?
- If 832J of energy is required to raise the temperature of a sample of aluminum from 20.0°C to 97.0°C, what mass is the sample of aluminum? The specific heat of aluminum is 0.90 J/(g x degrees C)
- A chef was in a hurry to prepare a meal. He had two pans of the same size: one with a copper bottom, and one with an aluminum bottom. After looking up the specific heat capacity of each metal in his chemistry book, which pan did he use? Why?
- Solid iron a specific heat of 0.444 J/g°C. If 75 calories of energy were removed from a piece of iron, and the temperature of the iron went from 21.4°C to -25.2°C, what was the mass of the iron?
- How much heat is required to raise the temperature of 250.0 g of mercury to 52°C?
- What units express specific heat capacity?
- A 17.5 g sample of metal at 125.0°C is placed in a calorimeter with 15.0 g of water at 25.0°C. if the temperature of the water rises to 30.0°C, what is the specific heat of the metal?
- The mass of water is 70.0 g. What is the energy required to heat a beaker of water at 18 degrees C to boiling?
- As 390-g of hot milk cools in a mug, it transfers 30,000 J of heat to the environment. How does the temperature of the milk change?
- A 0.050g ball of aluminum foil absorbs 1.42 J heat when it is heated 31.6°C. What is the specific heat of aluminum foil?
- What is the specific heat of an unknown substance if 2000 J energy are required to raise the temperature of 4 grams of the substance 5°C?
- If you wish to warm 100 kg of water by 20 degrees C for your bath how much heat is required?
- Question #7e78b
- What is the amount of heat energy associated with the reverse process?
- How much heat does a 23.0 gram ice cube absorb as its temperature increases from-17.4 °C to 0.0 °C ? The specific heat of ice is 2.108 J/(g C).
- Question #23db5
- Does vegetable oil have low specefic heat capacity?
- If the temperature of 34.4 g of ethanol increases from 25 °C to 78.8 °C, how much heat has been absorbed by the ethanol? The specific heat of ethanol is 2.44 J/(gC)?
- What is the molar specific heat capacity of ammonium chloride?
- Is heat being added or taken away when water boils?
- Why, compared to most other substances, a great deal of heat is needed to raise the temperature of water by a given amount?
- Question #66cc0
- What is the specific heat capacity of silver metal if 55.00 g of the metal absorbs 47.3 calories of heat and the temperature rises 15.0°C?
- How many grams of water would require 2200 joules of heat to raise its temperature from 34°C to 100°C?
- How much heat does it take to raise the temperature of 9.0 kg of wood from 12°C to 97*C?
- How much heat is needed to melt 1.25 kg of water at its melting point?
- How much heat does it take to raise the temperature of 2.5 kg of plastic from 15°C to 75°C?
- Question #79ed9
- A sample of glass that has a mass of 6.0 g gives off 12 J of heat. If the temperature of the sample changes by 4.0°C during this change, what is the specific heat of the glass?
- How much heat is added if .617g of water is increased in temperature by .241 degrees C?
- How much energy is needed to change the temperature of 95.4g of nickel from 22°C to 32°C? Is the energy absorbed or released?
- Question #3a1a1
- Question #ed7d1
- What is the final temperature of the copper and water given that the specific heat of copper is 0.385 #J/(g * "^oC)#?
- How much heat is required to convert 20.0 g of ice at -50.0°C to liquid water at 0.0°C? The specific heat of ice is 2.06 J/(g *#"^o#C) and the heat of fusion of water is 334 J/g?
- #"2659 J"# of heat energy are required to heat a substance with a mass of #"24.25 g"# from #"23.7"^@"C"# to #"163.5"^@"C"#. What is its specific heat capacity?
- In a experiment it is observed that 252 J of heat must be absorbed to raise the temperature of 50.0 g of Ni(s) from 20.0 C to 31.4 C. How do you calculate the specific heat of Ni in both J/g °C and cal/g.C?
- To sterilize a 50.0 g glass baby battle, we must raise its temperature from 22°C to 95.0°C. How much heat is required?
- Suppose 3260 joules are absorbed by 135 grams of water. If the initial temperature of the water is 21.4°C, what is its final temperature?
- How much thermal energy is absorbed by 750 grams of water when its temperature increases from 15.4 C to 86.3°C?
- Question #d32d8
- How would you calculate the specific beat of silver, given that 280 g of the metal absorbed 136 calories when changed from 22.13°C to 30.79°C?
- The specific heat of aluminum is 0.214 cal/g°c. What is the energy, in calories, necessary to raise the temperature of a 55.5 g piece of aluminum from 23.0 to 48.6°C?
- What is the specific heat capacity of a 17.5g sample of an unknown metal that releases 6700J of heat when it cools from 90 to 25 degrees C?
- What is the temperature change in 224 g of water upon the absorption of 55 kJ of heat, the specific heat of water is 4.18 J/g °C?
- The specific heat of steel is 420 J/(kg°C). How much energy is required to heat 1 kg of steel by 20 °C?
- Specific heat is the amount of heat required to raise the temperature of 1 g of a substance by what?
- If the specific heat of water is about 4 and the specific heat of air is about 1, which of the two substances will cool down the slowest?
- If an object has a low specific heat, does it heat up and cool down quickly or slowly?
- Question #ce46f
- How much heat is needed to increase the temperature of #"1 kg"# of foam by #"2 K"# knowing that the specific heat of foam is #"1200 J kg"^(-1)"K"^(-1)# ?
- Question #a6da5
- The specific heat of iron is 0.11 cal (g°C) . A cafeteria fork made of iron has a mass of 20 grams. How much heat energy is needed to raise the temperature of this fork from 25°C to 75°C?
- What is likely to be cooler on a sunny day: ocean water or sand on the beach?
- What is the specific heat capacity of substance if #2.41times10^4# #J# are needed to change the temperature of #105.0# #g# of it from #25.00°C# to #250.0°C#?
- Question #cb561
- The specific heat of copper is 0.385 J/g #*# °C. How would you calculate the amount of heat needed to raise the temperature of 0.75 g of copper from 7°C to 29°C?
- A 0.2 kg piece of unknown metal is heated to 87 °C and then dropped into a 0.28 kg sample of water at 22°C. If the final temperature of the mixture is 24°C, what is the specific heat of the unknown metal?
- Given the specific heat of lead is 0.129 J/g#*#K and that it takes 93.4 J of energy to heat a sample of lead from 22.3°C to 40.°C, how do you find the mass of the lead.?
- A 0.52g sample of metal that looks like gold requires 1.65 J of energy to change its temperature from 25.0°C to 40°C. Is this metal pure gold?
- Why does water feel cooler than hot pavement at the same temperature?
- An unknown substance has a mass 26.3 g. The temperature of the substance increases by 11.9 degrees C when 73.5 J of heat is added to the substance. What is the most likely identity of substance?
- How much heat, in calories, is given off when 1.25 grams of silver is cooled from 100.0 C to 80.0 C? (The specific heat of silver is 0.057 cal/g C)?
- What does a high specific heat tell about a substance?
- How do I find the specific heat in this question?
- A 60 g piece of metal at an initial temperature of 92°C is transferred into 70 g of water initially at 24.5°C. The final temperature of the water and the metal is 40°C. How do you determine the specific heat of the metal?
- Question #c1168
- The specific heat of gold is 0.129 J/g#*#c. What is the molar heat capacity of gold?
- What is the specific heat of water with three units that include calories?
- How much heat is required to change 25.0 g of liquid water at 75°C into steam at 100°C?
- Question #a5e2b
- How does the specific heat capacity of water compare with that of other common substances?
- What is the amount of energy needed to heat 55.0 g of water from 45°C to 67°C?
- A metal spoon becomes hot after being left in a pan of boiling water. What is this an example of?
- How much energy does it take to heat 346 g of steam at 100 degrees to steam at 110 degrees Celsius if the specific heat of steam is 2.01 J/g°C?
- Question #f3dcd
- What is the formula used for determining specific heat?
- Molten iron is extremely hot, averaging about 1,500 C. The specific heat of iron is 0.46 J/gC. How much heat is released to the atmosphere when 1 kg molten iron cools to room temperature (25 C)?
- How much heat is released as a 5.89 kg block of aluminum cools from 462°C to 315 °C?
- How many joules of heat would be required to heat 0.5 kg of aluminum by 2K?
- If it takes 21,966 J of heat energy to warm 750 g of water, what was the temperature change?
- A 45.0 mL sample of water is heated from 15.0°C to 35.0°C. How many joules of energy have been absorbed by the water?
- How much heat is absorbed by a 2000 kg granite boulder as energy from the sun causes its temperature to change from 10°C to 29°C?
- How do you find the specific heat of an unknown metal given the following information?
- How do you determine the specific heat of a material if a 35 g sample absorbed 96 J as it was heated from 293 to 313 K?
- Question #bce5b
- How would you rank these substances from highest to lowest using specific heat values: silver, water, sodium, wood, copper, glass?
- How does the mass of the substance effect the specific heat value?
- It takes 78.2 J to raise the temperature of 45.6 grams of lead by 13.3 C. What is the specific heat of lead?
- How do you calculate the amount of heat needed to melt 35.0 g of ice at 0 °C?
- Question #eee3a
- A 10.0 g sample of pure gold (Au) at 55.0 C gives off 45.0 J of heat to its surroundings. The specific heat capacity (C) of Au is 0.129J/g*C. What is the final temperature, in C, of the Au sample?
- The table below shows the specific heats of several metals. The temperature of a 15-g sample of an unknown metal increases from 20.0 C to 30.0 C when it absorbs 67.5 J of heat. Which of the metals in the table below could be the unknown metal?
- The specific heat of iron is 0.46 J/gC. How many joules will it take to make the temperature of a 150 g bar go up from 25 C to 60 C?
- When 18 grams of copper absorbs 1 kJ (1000 J) of energy, the temperature increases from 35.0°C to 179.3 °C. What is the specific heat of copper?
- When ice metals to give water why is the temperature profile STATIC with the ice still present?
- How much heat is needed to raise the temperature of 50 g of a substance by 15°C when the specific heat is .92 J/g-°C?
- Question #2e5cf
- Question #7c57c
- What is the specific heat capacity of silver atom, if #"386 g"# of #"Ag"# has a heat capacity of #"91.5 J/"^@ "C"#?
- If a sample of chloroform is initially at 25°C, what is its final temperature if 1.5 kg of chloroform absorbs 1.0 kilojoules of heat, and the specific heat of chloroform is 960 J/kg C?
- Question #5d6c3
- A 25 g piece of an unknown metal alloy at 150°C is dropped into an insulated container with 200 g of ice. How do you calculate the specific heat capacity of the metal, given that 9.0 g of ice melted?
- The specific heat of nickel is 0.44 J/g°C. How much energy needed to change the temperature of 95.4g of nickel from 32°C to 22°C. Is the energy absorbed or released?
- If 8.40 kJ of heat is needed to raise the temperature of a sample of metal from 15 °C to 20 °C, how many kilojoules of heat will be required to raise the temperature of the same sample of metal from 25 °C to 40 °C?
- Question #fcc68
- Question #d6cee
- Question #dc2ff
- How much heat is required to convert 200. g of 40 degrees C water to steam at 100' degrees C?
- Which sample is most likely to undergo the smallest change in temperature upon the absorption of 100 kj of heat? A.15g of water B.15g of lead C.50g of water D.50g of lead Why water?
- Question #a5ef6