Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the specific heat capacity of silver under these conditions is -1 0.235 J-g K . Round your answer to 2 significant digits.

Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the specific heat capacity of silver under these conditions is -1 0.235 J-g K . Round your answer to 2 significant digits.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 14P

See similar textbooks

Related questions

Q: How much heat is needed to heat 26.9 grams of metal from 19 degrees C to 101 degrees C? The specific…

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

Q: 450 Joules of energy were requiri d to raise the temperature of a 10.0g sample of aluminum from 25 C…

Q: A gas in a closed container is heated, causing the lid of the container to rise. The gas performs 3J…

A: Given: work done ( w) = - 3 J Internal energy change ( ∆U ) = + 15 J Heat absorbed ( q ) = ? By…

Q: In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used…

A: Mass of copper, MCu = 60.04 g Mass of water, Mw = 79.22 g Initial temperature of Copper, TCu = 97.70…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.73 kg sample…

A: Heat capacity is defined as the amount of heat required to change the temperature of the substance…

Q: A 55 kg block of metal has an original temperature of 15.0°C and a specific heat capacity of 0.45…

A: Specific heat capacity (C) = Q m ( T2…

Q: In the laboratory a student finds that it takes 88.1 Joules to increase the temperature of 14.5…

A: The amount of heat required to raise the temperature of a substance by one degree Celsius is called…

Q: the laboratory a student finds that it takes 29.3 Joules to increase the temperature of 13.1 grams…

A: Given -> ∆H= 29.3 joule Weight (m) = 13.1 gm T1=20.0°C T2= 37.9°C

Q: A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample…

A: Using the following equation, the mass of the metal is calculated.

Q: A 1.00 g piece of copper metal is initially at 100.0°C. It is dropped into a coffee cup calorimeter…

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: The heat capacity of platinum (Pt, 195.1 g mol-1), is 26.0 J mol-1 K-1. Calculate the energy needed…

A: Q = n S ∆T where m = mass of the given metal = 66.6 g n = W/M = 66.6 g/ 195.1 g/mol = 0.341 mol…

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: In the laboratory a student finds that it takes 921 Joules to increase the temperature of 13.8 grams…

Q: A 69.5 g piece of iron at 525°C is put into 627 grams of water at 15.0°C. What is the final…

A: Given Mass of iron = 69.5 g Mass of water = 627 g Initial temperature of iron = 525°C Initial…

Q: In the laboratory a student finds that it takes 204 Joules to increase the temperature of 12.9 grams…

Q: to reach 100°C first? Why? 9.35 A piece of titanium metal with a mass of 20.8 g is heated in boiling…

A: Since you are posted with multiple sub-parts. Also, you have mentioned answer item 9.35 only. So I…

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: A 296.0 g piece of granite, heated to 601.0°C in a campfire, is dropped into 1.15 L water (d =…

A: Mass of granite piece=296.0 g The volume of water=1.15 L=1150 mL The density of water, d = 1.00…

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: 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: 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: A 5.80-g sample of copper is heated from 55.0C to 75.0C. The amount of energy required to 23.20j .…

A: The heat capacity is the ratio of the energy supplied in the form of heat to the rise in the…

Q: A sample of gold weighing 7.7 grams is cooled then placed in a calorimeter containing 27.01 grams of…

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

Q: A calorimeter contained 75.0 g of water at 16.95 °C. A 93.3 g sample of iron at 65.58°C was placed…

A: Specific heat capacity is equal to the heat of 1g of substance required to raise the temperature by…

Q: In the laboratory a student finds that it takes 76.1 Joules to increase the temperature of 12.8…

A: Mass of copper m = 12.8 g Heat energy required Q = 76.1 Joules Initial temperature T1 = 20.5 0C…

Q: What mass of natural gas (CH4) must burn to emit 267KJ of heat? CH4 (g) + 2 O2 (g) -------> CO2…

A: Given, The mass of natural gas (CH4) must burn to emit 267KJ of heat is: CH4 (g) + 2 O2 (g)…

Q: In the laboratory a student finds that it takes 21.6 Joules to increase the temperature of 13.4…

Q: In the laboratory a student finds that it takes 54.9 Joules to increase the temperature of 11.0…

Q: he table shows the specific heat capacity of four substances. Heat Capacity Substance Aluminum 0.900…

A: Q = m . s . ∆T Where, Q = heat require to raise the temperature m = mass of substance s = specific…

Q: A 43.0-g sample of copper at 99.1 °C is dropped into a beaker containing 151 g of water at 18.7 °C.…

A: When copper is placed in water, the heat liberated from copper will be equal to the heat gained by…

Q: In the laboratory a student finds that it takes 666 Joules to increase the temperature of 10.7 grams…

A: The heat required (q) to raise the temperature of 'm' g of a substance is given as: q=mc∆Twhere, c…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.19 kg sample…

Q: A 531.1 g sample of ammonia releases 777.1 joules of heat. The specific heat capacity of ammonia is…

A: Here we are required to find the change in the temperature when certain mass of ammonia releases…

Q: In the laboratory a student finds that it takes 34.1 Joules to increase the temperature of 14.2…

A: To Calculate the specific heat of a substance we can use it's mass , temperature change and the the…

Q: 1. A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and is temperature changes from…

A: Since you have posted multiple questions, we will solve only the first question for you according to…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.76 kg sample…

A: To find molar heat capacity.

Q: A 46.0-g sample of copper at 99.0 °C is dropped into a beaker containing 159 g of water at 18.0 °C.…

A: When the hot metal is dunked into the water, the heat is released by the metal and equal heat is…

Q: 25.0

A: We will use heat energy formula

Q: A 753.2 g sample of silver releases 683.2 joules of heat. The specific heat capacity of silver is…

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: 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: A 88.8 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C…

A: Mass of water is calculated as follows

Q: energylost by the Fewill be th the heat enérgy gained by- Mass of water 50.003 g Temperature of…

A: Given that :

Q: A 0.491 kg sample of an unknown metal loses 4.08 kJ of heat. If the change in its temperature was…

A: Using the formula Q=mCΔT we can find specific heat capacity.

Q: In the laboratory a student finds that it takes 706 Joules to increase the temperature of 13.3 grams…

A: The mass of water is = 13.3 g The increase in the temperature of the water is = (36.4-23.0)oC =…

Q: Iron bar of mass 869 g cools from 94 degree C to 5 degree C. Calculate the heat released by the…

A: Given : Mass of iron = 869 g Initial temperature of iron = 94 oC And final temperature of iron = 5…

Q: A 35.2-g sample of metal X requires 1251 Jof energy to heat the sample by 25.0 °C.Calculate the…

A: Given information:

Question

O THERMODYNAMICS
Using specific heat capacity to find heat
Calculate the energy required to heat 486.0 mg of silver from -9.6 °C to -3.7 °C. Assume the specific heat capacity of silver under these conditions is
0.235 J-gK'. Round your answer to 2 significant digits.
Explanation
Check
O 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Ac
I olo
III

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

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

A 237-g piece of molybdenum, initially at 100.0 C, is dropped into 244 g of water at 10.0 C. When the system comes to thermal equilibrium, the temperature is 15.3 C. What is the specific heat capacity of molybdenum?
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
9.11 Analyze the units of the quantity (pressurevolume) and show that they are energy units, consistent with the idea of PV-work.
If the heat capacity varies withtemperature, abetter form ofequation 2.9 isto solve q=TiTfnCT-t A 50.0-g sample of white phosphorus is heated from 298 K to 350K. If its molar heat capacity is CT- = 56.990.1202T J/mol.K, how much heat is needed?
The statement Energycan beneithercreatednor destroyedis sometimes used as an equivalent statement of the first law of thermodynamics. There areinaccuracies to the statement, however. Restate it tomake it less inaccurate.
Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume each peanut, with an average mass of 0.73 g, is 49% peanut oil and 21% starch; the remainder is noncombustible We further assume peanut oil is palmitic acid, C16H32O2, with an enthalpy of formation of 848.4 kJ/mol. Starch is a long chain of C6H10O5 units, each unit having an enthalpy of formation of 960 kJ.
You have a l.00-mole sample of water at 30.C and you heat it until you have gaseous water at 140.C. Calculate q for the entire process. Use the following data. Specificheatcapacityofice=2.03J/CgSpecificheatcapacityofwater=4.18J/CgSpecificheatcapacityofsteam=2.02J/Cg H2O(s)H2O(l)Hfusion=6.02KJ/mol(at0C)H2O(l)H2O(g)Hvaporization=40.7KJ/mol(at100.C)
The distance between downtown San Francisco and downtown Oakland is 9 miles. However, a car driving between the two points travels 12.3miles. Of these distances, which one is analogous to a state function? Why?
Calculate the specific heat of a material if 288J of energy were required to heat 50.5g of the material from 298K to 330K. What are the units?
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
Define the terms system and surroundings. What does it mean to say that a system and its surroundings are in thermal equilibrium?
Aballoon filled with 0.505 mole of gascontracts reversibly from 1.0L to 0.10 L ata constant temperature of 5.0C. In doing so, it loses 2690J of heat. Calculate w, q, U, and H for the process.