Question

Calculate the energy required to heat 0.40kg of water from 44.4°C to 62.6°C .Assume the specific heat capacity of water under these conditions is. 4.18J·g−1K−1. Be sure your answer has the correct number of significant digits.

Expert Solution

Want to see the full answer?

Check out a sample Q&A here
Blurred answer
Students who’ve seen this question also like:
Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN: 9780078746376
Author: Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher: Glencoe/McGraw-Hill School Pub Co
Not helpful? See similar books
Chemistry: Matter and Change
Chemistry: Matter and Change
Energy And Chemical Change. 126A
marketing sidebar icon
Want to see this answer and more?
Experts are waiting 24/7 to provide step-by-step solutions in as fast as 30 minutes!*
*Response times may vary by subject and question complexity. Median response time is 34 minutes for paid subscribers and may be longer for promotional offers.

Related Chemistry Q&A

Find answers to questions asked by students like you.

Q: Calculate the energy required to heat 0.40kg of water from 44.4°C to 62.6°C. Assume the specific…

A: The energy required to heat 0.40kg of water from 44.4°C to 62.6°C is to be calculated. Assume the…

Q: It takes 585 J of energy to raise the temperature of 125.6 g of mercury from 20.0°C to 53.5°C.…

A: Given, Heat energy, q = 585 J Mass, m = 125.6g Change in temperature, ∆T = 53.5- 20 = 33.5°C

Q: Calculate the energy required to heat 744.0mg of silver from −5.6°C to 19.1°C. Assume the specific…

A: The -5.60C and 19.10C are equal to 267.55 K and 292.25 K respectively. The mass of 744 mg of silver…

Q: 300J of heat is added to the  system and 180 J of work is done by the system through expansion. How…

A: Given that: Heat added to the system (q) = 300 J Work done by the system (w) = -180 J Internal…

Q: A copper rod with a mass of 21.0 g cools from 95.0oC to 45.0oC when placed in a water bath. If the…

A: The following equation relates that the quantities between heat and specific heat capcacity: q=mCΔT…

Q: In the laboratory a student finds that it takes 200 Joules to increase the temperature of 15.0 grams…

A: • The values provided in the question are:-    i) Mass of magnesium, m = 15.0 g  ii) Initial…

Q: 1.) The internal energy of a system increases 253 J , while the system loses 93 J of heat.…

A: Internal energy (∆E) :-         It is the energy of a thermodynamic system which is present in that…

Q: If you know that 18.5 grams of a particular mineral, with heat quantity of 1170 J, its temperature…

A: Hii There! since there are multiple question posted. we are answering first question. if you need…

Q: If you know that 18.5 grams of a particular mineral, with heat quantity of 1170 J, its temperature…

A: Given : Mass of metal = 18.5 g Initial temperature of metal = 25 oC Final temperature of metal = 92…

Q: Calculate the energy required to heat 1.20 kg of water from 49.6 °C to 60.1 °C. Assume the specific…

A: The mass of the water sample is = 12.0 kg The initial temperature of the water is = 49.6oC The final…

Q: A metal cools from an initial temperature of 150 degrees C to 50 degrees C and releases 190 J of…

A: Specific heat capacity is the amount of heat that is required to rise a temperature of 1 kg…

Q: Calculate the energy required to heat 310.0 mg of silver from -4.4 °C to 8.8 °C. Assume the specific…

A: Given mass = 310 g Specific heat = 0.235 J/g.K T1 = -4.4°C T2 = 8.8°C

Q: Ethanol weighing 3.56g is burned in a constant-volume bomb calorimeter. Consequently, the…

A: Heat capacity of Bomb calorimeter and water = 8.224 KJ/◦C

Q: When a solid dissolves in water, hest may be evolved or absorbed. The heat of dissolution…

A: Since you have posted multiple questions, the answer for first question is given below. Kindly…

Q: When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution…

A: Click to see the answer

Q: A 48.4-g sample of an unknown metal at 100.0 °C is placed in a constant-pressure calorimeter…

A: Click to see the answer

Q: What is the mass of a sample of alcohol, if it were to require 4,780 Joules of heat in order to…

A: Click to see the answer

Q: Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the…

A: Q = m . s . ∆T Where, Q = heat absorbed;  m = mass of metal, s = specific heat of metal and ∆T =…

Q: The quantity of heat required to change the temperature of 1 g of a substance by 1°C is defined as…

A: Click to see the answer

Q: Calculate the change in the internal energy for a certain process if 800 J of work is done on the…

A: Click to see the answer

Q: A calorimeter contained 67.0 g of water at 15.93°C. A 110.-g sample of iron at 66.42°C was placed in…

A: Click to see the answer

Q: The work done to compress a gas is 74J. As a result, 26J of heat is given off to the surroundings.

A: First law of thermodynamics states that heat energy cannot be created or destroyed. It can be…

Q: - A 150 g sample of metal at 75 °C is added to 150 g water at 15°C. The temperature of the water…

A: Given data   metal water mass 150 g 150 g t1 75 oC 15 oC t2 18.3 oC 18.3 oC   specific…

Q: A 52.7 g. piece of an unknown metal is heated up 51.4 °C when given 3492 J of heat.  What is the…

A: Formula : Heat, q = msΔT     3492 = 52.7 x s x 51.4   s = 1.289 J g-1 °C-1 Here s is specific heat…

Q: Ethanol weighing 3.56 g is burned in a constant-volume bomb calorimeter. Consequently, the…

A: Click to see the answer

Q: Ethanol weighing 3.56 g is burned in a constant-volume bomb calorimeter. Consequently, the…

A: Click to see the answer

Q: Question attached

A: The specific heat of air at constant volume is given to 0.718 kJ/kgK. This means that the 0.718 kJ…

Q: A 2.62E1 g sample of aluminum at 1.008E2 °C is added to 1.002E2 g of water at 2.22E1 °C in a…

A: For a chemical reaction or physical process to occur a certain amount of energy should be furnished…

Q: A gas absorbs 188 J of heat and then performs 310 J of work. The change in internal energy of the…

A: In chemistry, the term internal energy for a given system can be defined as the energy which is…

Q: Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the…

A: The amount of heat energy required is related to specific heat capacity as,…

Q: Calculate the energy required to heat 0.10 kg of silver from -7.5 °C to 14.8 °C. Assume the specific…

A: Click to see the answer

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 289.0mg sample…

A: given: mass = 289 mg = 0.289 g T2 = 40oC T1 = 22.1°C  Q = 8.75 J molar mass of C4H8O2 = 88.11 g/mol…

Q: A system gains 767 kJ of heat, resulting in a change in internal energy of the system equal to +201…

A: Find the solution below

Q: In the laboratory a student finds that it takes 139 Joules to increase the temperature of 13.0 grams…

A: Q = mCdT Q = heat energy required m = mass C = specific heat dT = change in temperature

Q: When determining the heat capacity of the unknown metal we assumed the heat capacity of water has a…

A: When determining the heat capacity of the unknown metal we assumed the heat capacity of the water…

Q: A piece of aluminum with a mass of 4.39 grams is heated to raise its temperature from 21.7°C to…

A: a) Since specific heat capacity of Al is 0.9 J/g.°C Since quantity of heat absorbed is given by  Q =…

Q: When 1.60 g of liquid PCI3 at 23.9 C is added to a solution of water at in a coffee cup calorimeter,…

A: Click to see the answer

Q: A piece of titanium metal with a mass of 20.8 g is heated boiling water to 99.5°C and then dropped…

A: Click to see the answer

Q: A calorimeter contained 83.0 g of water at 15.43°C. A 165-g sample of iron at 64.80°C was placed in…

A: Heat Capacity (C) is the amount of Heat required to increase the temperature of 1 gram mass of…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.43 kg sample…

A: Given, mass of sample C4H11N, m = 0.43 kg Moles  0f C4H11N = 0.43 ×103 g73 g/mol change in…

Q: Im having trouble finding J*mol^-1*K^-1.

A: The given temperature in Kelvin scale can be written as follows,-9oC = 264.15 K11.3oC = 284.45…

Q: Determine the internal energy change if 718 J of heat are transferred to the system and 437 J of…

A: Click to see the answer

Q: A student heats 62.33 grams of chromium to 99.36 °C and then drops it into a cup containing 82.16…

A: Given, mass of chromium =62.33 graminitial  temperature of chromium =99.36 °Cmass of water =82.16…

Q: An electrical heater is used to supply 210.0 J of energy to a 15.0 g sample of water, originally at…

A: Given:Heat energy (Q) = 210.0 J.Mass of water (m) = 15.0 g.Initial temperature of water = 295…

Q: In the laboratory a student finds that it takes 83.3 Joules to increase the temperature of 14.0…

A: Given data 83.3joule needed  Mass of solid iron in 14.0gram Initial temperature = 21.7°c final…

Q: An experiment is carried out where 12.2g of NaOH is dissolved in 240.0g of water in a coffee cup…

A: The experiment is the measurement of heat of dissolution of NaOH.

Q: A lead pellet having a mass of 26.47 g at 89.98 °C was placed in a constant-pressure calorimeter of…

A: Given data: The mass of the lead pellet=26.47 g. The temperature of the lead pellet=89.93°C. The…

Q: A 1.3 kg block of iron at 29 °C is rapidly heated by a torch such that 15 kJ is transferred to it.…

A: Given data : Mass of iron block = 1.3 kg = 1300 g Specific heat of iron CFe=0.450J/g°C Total heat…

Q: During a certain chemical reaction 255 J of heat is absorbed by the system and 275 J of work is done…

A: To Solve this problem we will use the first law of thermodynamics .

Q: Calculate the energy required to heat 133.0 mg of silver from -6.9 °C to 17.7 °C. Assume the…

A: The specific heat can be defined as the amount of heat per unit mass that is needed to raise the…

Knowledge Booster
Chemistry
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.
Recommended textbooks for you
  • Chemistry: Matter and Change
    Chemistry
    ISBN:9780078746376
    Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
    Publisher:Glencoe/McGraw-Hill School Pub Co
    General Chemistry - Standalone book (MindTap Cour...
    Chemistry
    ISBN:9781305580343
    Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
    Publisher:Cengage Learning
    World of Chemistry
    Chemistry
    ISBN:9780618562763
    Author:Steven S. Zumdahl
    Publisher:Houghton Mifflin College Div
  • Chemistry: Principles and Reactions
    Chemistry
    ISBN:9781305079373
    Author:William L. Masterton, Cecile N. Hurley
    Publisher:Cengage Learning
    Chemistry for Today: General, Organic, and Bioche...
    Chemistry
    ISBN:9781305960060
    Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
    Publisher:Cengage Learning
    Chemistry by OpenStax (2015-05-04)
    Chemistry
    ISBN:9781938168390
    Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
    Publisher:OpenStax
  • Chemistry: Matter and Change
    Chemistry
    ISBN:9780078746376
    Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
    Publisher:Glencoe/McGraw-Hill School Pub Co
    General Chemistry - Standalone book (MindTap Cour...
    Chemistry
    ISBN:9781305580343
    Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
    Publisher:Cengage Learning
    World of Chemistry
    Chemistry
    ISBN:9780618562763
    Author:Steven S. Zumdahl
    Publisher:Houghton Mifflin College Div
    Chemistry: Principles and Reactions
    Chemistry
    ISBN:9781305079373
    Author:William L. Masterton, Cecile N. Hurley
    Publisher:Cengage Learning
    Chemistry for Today: General, Organic, and Bioche...
    Chemistry
    ISBN:9781305960060
    Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
    Publisher:Cengage Learning
    Chemistry by OpenStax (2015-05-04)
    Chemistry
    ISBN:9781938168390
    Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
    Publisher:OpenStax