An ice bag containing 325g of ice at 0 degrees Celsius was used to treat sore muscles. When the bag was removed, the ice had melted and the liquid water had a temperature of 18.5 degrees Celsius. How many kilojoules of heat were absorbed?

An ice bag containing 325g of ice at 0 degrees Celsius was used to treat sore muscles. When the bag was removed, the ice had melted and the liquid water had a temperature of 18.5 degrees Celsius. How many kilojoules of heat were absorbed?

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Energy

Section: Chapter Questions

Problem 58A

See similar textbooks

Related questions

Q: The ethylene glycol (d = 1.11 g/mL; c = 2.42) in a car radiator cools from 37.0°C to 25.0°C by…

A: The volume of ethylene glycol is 5468.43 mL

Q: How much energy is required to raise the temperature of 10.8 grams of solid chromium from 21.5…

A: According to thermodynamics: q=mc∆T . . . (1) Here, m is the mass = 10.8 g c is the…

Q: Calculate the amount of heat in joules needed to increase the temperature of 350 g of water from 20…

A: Specific heat capacity is amount of heat needed to increase the temperature of one gram of substance…

Q: 500.0 g of water in its liquid phase loses 5,892 J of heat. If it started at a temperature of 25.0…

A: We have given that The mass of water = 500g Heat release in liquid phase = 5892J Initial…

Q: How much heat ( in joules) does it take to heat 45.0 g of 23.0 C water until it is steam at 112.0 C?

A: Answer: Heat (in joule) = 117319.5 J

Q: The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to…

Q: Calculate the heat capacity, in joules per degree, of 28.4 g of water. Specific heat of water is…

Q: 5. How much heat must be,removed from 15.5 g of water at 90.0°C to cool it to 43.2°C? 30353

Q: Calculate the amount of heat required to raise the temperatureof a 65-g sample of water from 32oC to…

A: The heat Q required to raise the temperature is,

Q: The specific heat of water is 4.184 J gc. What is the amount of heat associated with heating 50.0 ml…

Q: I have 270 mL of hot coffee in an insulated vessel. I cool it down to 83 degrees C by adding a 25…

A: If the ice is placed in container with water, the heat start flowing from water to the ice, and…

Q: Determine the specific heat of 122 grams of an unknown substance if it absorbed 270 kJ of heat as it…

A: Specific heat of a substance can be defined as the amount of heat required to raise temperature by…

Q: How much heat is required to convert 24.0 g of ethanol at 25 ∘C to the vapor phase at 78 ∘C?…

A: Given : Mass of ethanol = 24g Initial temperature = 25oC Final temperature = =78oC Heat of…

Q: water has a specific heat of 4.184j/degree celcius. aluminum has a specific heat of j/g degrees…

A: Specific heat capacity of water = 4.184 J/goC Specific heat capacity of aluminium = 0.89 J /goC Heat…

Q: How much heat is required to warm 1.60 kg of sand from 24.0 degree Celsius to 100.0 degree Celsius?

A: Given data is as follows: The mass of the sand = 1.60 kg = 1600 g The initial temperature of the…

Q: How much heat is required to warm 1.50 kg of sand from 24.0 ∘C to 100.0 ∘C

A: Given: Mass of water = 1.5 kg = 1500 g Initial temperature (T1) = 24°C Final temperature (T2) =…

Q: A vessel containing 1 000 kg of water at 25 degrees celsius is heated until it boils. How much heat…

A: In this question, you will need to Calculate the heat, means how much heat is required in kJ by the…

Q: How much total heat, in kJ, does it take to heat 82.58 grams of ice at 0°C to 91.36°C? cwater =…

A: Here there are two heat to be consider as q1 = Heat require to melt the ice at 0 oC and q2 = heat…

Q: A 149-g sample of steam at 100 ∘C is emitted from a volcano. It condenses, cools, and falls as snow…

A: The emitted volcano at 1000C is 149 g. The heat of condensation = 2260 J/g =149 g x 2260 J/g= 336740…

Q: How much heat is absorbed by 750 grams of water as it is heated from 25.0°C to 96.0°C? (in kJ,…

A: Heat absorbed by water, q = ms∆T q = 750 x 4.184 x ( 96.0…

Q: A yogurt mix is heated in a stainless-steel kettle by steam at 100°C with 90% quality. Steam…

A: It involves two stages . 1) conversion of staem to water 2) then water at 100°C to 80°C Heat…

Q: 20.0 grams of water at 85ºC is added to 35.0 grams of water at 10.0ºC in an insulated container.…

Q: Calculate the amount of heat absorbed by 100 g of water that warms from 100 K to 273 K.

Q: a 16.7 g polystyrene foam cup containing 31.0 mL coffee changes in temperature from 18 degrees…

A: Given: Mass of polystyrene foam cup = 16.7 g Volume of coffee = 31 mL = 31 x 10-6 m3 Change in…

Q: 1. Determine the amount of energy required to melt 15.0 grams of ice. 2a. If a 2000g block of metal…

A: 1) Given, Mass of ice = 15.0 g Latent heat of fusion of water = ΔHf = 334 J/g Amount of…

Q: Calculate the amount of heat needed to raise the temperature of 55g of liquid water from 25 degrees…

Q: How many kilojoules of heat are absorbed when 2.00 L of water is heated from 12.5°C to 93.5°C?

A: Mass= density×volume Mass= 1×0.002=0.002gm Now Q=mc∆T Q= 0.002×4.18×(93.5-12.5) Q= 0.067×10-6kj

Q: how much heat must be lost to change 35 grams of gaseous water into ice form 155 degrees celsius to…

A: Given- heat be lost to change 35 grams of gaseous water into ice form 155 degrees celsius to -65…

Q: What is the heat generated/released when 60 g of copper (specific heat= 0.39 J/C) is cooled from 40…

A: Given, mass, m = 60 g specific heat, c = 0.39 J/g.°C temperature, ΔT = 40 - 30°C = 10°C The formula…

Q: A 15.5g piece of chromium is initially heated to 100.0 degrees C and then dropped into a beaker…

A: The mass of chromium metal piece is = 15.5 g The temperature of the chromium piece is = 100oC =…

Q: Calculate the mass of liquid water (in grams) at 100 °C that can be converted to vapor when 2400 J…

A: Calculate the number of moles of liquid water which can be converted into vapor form on absorption…

Q: 100.0 g of 4.0 degrees C water is heated until its temperature is 37 degrees C.Calculate the amount…

A: Heat required = mCsΔT m = Mass of substance Cs = Specific heat of substance ΔT = Temperature…

Q: Two 20.0 g ice cubes at −10.0 ∘C are placed into 285 g of water at 25.0 ∘C. Assuming no energy is…

A: Mass of water = 285 g Temperature of water = 25˚C. Heat capacity of water = 75.3 JK-1mol-1 Heat lost…

Q: A foundry worker places a 5.76 kg sheet of nickel at a temperature of 18°C on top of a 16.6 kg sheet…

A: The specific heat capacity for a given chemical substance or a solution refers to the amount of the…

Q: Calculate the heat (in kJ) associated with the cooling of 392 g of mercury from 75.8°C to 12.0°C. kJ

A: The mass of mercury = 392 g. Initial temperature = 75.8 0C. Final temperature = 12 0C. Temperature…

Q: If the temperature of a 500.0 -g sample of liquid water is raised 2.00 celsius, how much heat is…

A: We have to Given : m = 500.0 g Raised in…

Q: How many kilojoules of heat energy are absorbed by a 200. g block of ice from -10 C to 0 C?

A: Solution- Given Temperature- 00C to - 100C heat energy are absorbed by block of ice =200. g…

Q: Calculate the amount of heat in Joules required to convert 180g of water at 10.0 to 100.0 degrees…

A: The amount of heat required to convert one Mole of liquid into vapour phase at it's boiling point is…

Q: How much heat, in kJ, is absorbed by 50.0g of water if the temperature changes from 298K to 357K?…

A: Given, The amount of heat absorbed by 50.0g of water to increase temperature from 298 K to 357 K is:

Q: How much heat is gained by Aluminum when 52.2 g of Al is warmed from 20.3D defrees Celsius to 35.1…

A: Given, mass of Al (m) =52.2 gInitial temperature T1 =20.3°CFinal temperature T2 = 35.1°Cspecific…

Q: A 15-gram sample of lead (c = 0.128 J/g degrees celsius) is heated from 25 degrees celsius to 215…

A: The specific heat capacity for a given substance refers to the amount of heat that is needed to…

Q: Calculate the heat change in kilocalories for condensation of 8.0 kgkg of steam at 100 ∘C∘C.

Q: What amount of heat in Joules is required to raise the temperature 0f 10.0g of aluminum by 15.0…

A: The amount of heat Q required for increasing the temperature of a body of mass m by temperature ∆T…

Q: How many kilojoules of a heat energy are going to be required to heat a 200. g block of ice from -10…

A: Given that, Weight of ice block m = 200 g Change in temperature ∆T = 0°C - (-10°C) = 10°C Heat…

Q: 1. How much heat is lost when a 4110 g metal bar with a specific heat of 0.231 J/g°C cools from…

Q: How much heat is required to convert 24.0 g of ethanol at − 146 ∘C to the vapor phase at 78 ∘C?…

Q: How much heat is required to change 32.5 grams of liquid water into steam, from 25 degrees C to 115…

A: The conversion of 32.5 grams of water to steam with the change in temperature from 25oC to 115oC.…

Q: A 30.37 g sample of a substance is initially at 28.3 degrees Celsius. After absorbing 2235 J of…

A: The amount of heat (Q) gained or lost by a substance (with mass m) as its temperature changes (ΔT)…

Q: How much heat is required to convert solid ice with a mass of 685 g at a temperature of -11.0 °C to…

A: Given data:

Question

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

How much heat, in joules and in calories, is required to heat a 28.4-g (1-oz) ice cube from 23.0 C to 1.0 C?
A sample of ammonia (Hsolid=5.66kJ/mol) liberates5.66 kJ of heat as it solidifies at its melting point.What is the mass of the sample?
Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an insulated container. The final temperature of the mixture is 80C. All the heat flow occurs between the two liquids. The two liquids do not react with each other. Is the specific heat of liquid A larger than, equal to, or smaller than the specific heat of liquid B?
A 45-g aluminum spoon (specific heat 0.88 J/g C) at 24 C is placed in 180 mL (180 g) of coffee at 85 C and the temperature of the two become equal. (a) What is the final temperature when the two become equal? Assume that coffee has the same specific heat as water. (b) The first time a student solved this problem she got an answer of 88 C. Explain why this is clearly an incorrect answer.
A burning match and a bonfire may have the same temperature, yet you would not sit around a burning match on a fall evening to stay warm. Why not?
1. Which of the following processes requires the largest input of energy as heat? raising the temperature of 100 g of water by 1.0 °C vaporization of 0.10 g of water at 100 °C melting 1.0 g of ice at 0 °C warming 1.0 g of ice from −50 °C to 0 °C (specific heat of ice = 2.06 J/g · K)
Carbon tetrachloride, CCl4, is a liquid used as an industrial solvent and in the preparation of fluorocarbons. What is the heat of vaporization of carbon tetrachloride? CCl4(l)CCl4(g);H=? Use standard enthalpies of formation (Table 6.2).
Copper is used in building the integrated circuits, chips, and printed circuit boards for computers. When 228 J of heat are absorbed by 125 g of copper at 22.38C, the temperature rises to 27.12C. What is the specific heat of copper?
How much heat is evolved when 1255 g of water condensesto a liquid at 100°C?
If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?
If it takes 654 J of energy to warm a 5.51-g sample of water, how much energy would be required to warm 55.1 g of water by the same amount?
You have two samples of different metals, metal A and metal B, each having the same mass. You heat both metals to 95C and then place each one into separate beakers containing the same quantity of water at 25C. a You measure the temperatures of the water in the two beakers when each metal has cooled by 10C and find that the temperature of the water with metal A is higher than the temperature of the water with metal B. Which metal has the greater specific heat? Explain. b After waiting a period of time, the temperature of the water in each beaker rises to a maximum value. In which beaker does the water temperature rise to the higher value, the one with metal A or the one with metal B? Explain.