Skip to main content

of 1 mole of a monatomic gas is increased from 25°C to 300°C. 3.20 One mole of an ideal gas undergoes an isotherma expansion at 300 K from 1.00 atm to a final pressure while performing 200 J of expansion work. Calculate the final pressure of the gas if the external pressure s 0.20 atm. Heat Capacities 3.21 A 6.22-kg piece of copper metal is heated from 20.5° C to 324.3°C. Given that the specific heat of Cu is 0.385 J g1 °C-1, calculate the heat absorbed (in kJ) by the metal. 3.22 A 10.0-g sheet of gold with a temperature of 18.0°C is laid flat on a sheet of iron that weighs 20.0 g and has a temperature of 55.6°C. Given that the specific heats of Au and Fe are 0.129 J g-1 C-1 and 0.444 Jg-1 oc1, respectively, what is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. (Hint: The heat gained by the gold must be equal to the heat lost by the iron.) 3.23 It takes 330 joules of energy to raise the tempera- ture of 24.6 g of benzene from 21.0°C to 28.7°C at con stant pressure. What is the zene at constant pressure? 3.24 The molar heat of vaporization for water is 44.0 kJ mol-1 at 298 K and 40.79 kJ mol- qualitative explanation of th values. molar heat capacity of ben- 1 at 373 K. Give a e difference in these two 3.25 The constant-pressure molar heat capacit y of ni-

Question

3.22

of 1 mole of a monatomic gas is increased from 25°C to
300°C.
3.20 One mole of an ideal gas undergoes an isotherma
expansion at 300 K from 1.00 atm to a final pressure
while performing 200 J of expansion work. Calculate
the final pressure of the gas if the external pressure s
0.20 atm.
Heat Capacities
3.21 A 6.22-kg piece of copper metal is heated from
20.5° C to 324.3°C. Given that the specific heat of Cu is
0.385 J g1 °C-1, calculate the heat absorbed (in kJ) by
the metal.
3.22 A 10.0-g sheet of gold with a temperature of
18.0°C is laid flat on a sheet of iron that weighs 20.0 g
and has a temperature of 55.6°C. Given that the specific
heats of Au and Fe are 0.129 J g-1 C-1 and 0.444
Jg-1 oc1, respectively, what is the final temperature of
the combined metals? Assume that no heat is lost to the
surroundings. (Hint: The heat gained by the gold must
be equal to the heat lost by the iron.)
3.23 It takes 330 joules of energy to raise the tempera-
ture of 24.6 g of benzene from 21.0°C to 28.7°C at con
stant pressure. What is the
zene at constant pressure?
3.24 The molar heat of vaporization for water is 44.0
kJ mol-1 at 298 K and 40.79 kJ mol-
qualitative explanation of th
values.
molar heat capacity of ben-
1 at 373 K. Give a
e difference in these two
3.25 The constant-pressure molar heat capacit
y of ni-
expand button
Transcribed Image Text:of 1 mole of a monatomic gas is increased from 25°C to 300°C. 3.20 One mole of an ideal gas undergoes an isotherma expansion at 300 K from 1.00 atm to a final pressure while performing 200 J of expansion work. Calculate the final pressure of the gas if the external pressure s 0.20 atm. Heat Capacities 3.21 A 6.22-kg piece of copper metal is heated from 20.5° C to 324.3°C. Given that the specific heat of Cu is 0.385 J g1 °C-1, calculate the heat absorbed (in kJ) by the metal. 3.22 A 10.0-g sheet of gold with a temperature of 18.0°C is laid flat on a sheet of iron that weighs 20.0 g and has a temperature of 55.6°C. Given that the specific heats of Au and Fe are 0.129 J g-1 C-1 and 0.444 Jg-1 oc1, respectively, what is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. (Hint: The heat gained by the gold must be equal to the heat lost by the iron.) 3.23 It takes 330 joules of energy to raise the tempera- ture of 24.6 g of benzene from 21.0°C to 28.7°C at con stant pressure. What is the zene at constant pressure? 3.24 The molar heat of vaporization for water is 44.0 kJ mol-1 at 298 K and 40.79 kJ mol- qualitative explanation of th values. molar heat capacity of ben- 1 at 373 K. Give a e difference in these two 3.25 The constant-pressure molar heat capacit y of ni-
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
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
Not helpful? See similar books
Chemistry
Chemistry
Chemical Foundations. 1RQ
Learn more about
Solutions
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: Consider a balloon filled with 2115 L of helium at 1.00 atm pressure and 45.5°C. The temperature of…

A: Click to see the answer

Q: One mole of nitrogen gas confined within a cylinder by apiston is heated from 0C to 819C at 1.00…

A: a.

Q: Consider a balloon filled with 2115 L of helium at 1.00 atm pressure and 45.5°C. The temperature of…

A: Click to see the answer

Q: Consider a balloon filled with 2115 L of helium at 1.00 atm pressure and 45.5°C. The temperature of…

A: Click to see the answer

Q: 13. You want to heat the air in your house with natural gas (CH4). Assume that your house has 275…

A: We have to know how we will get require to heat room from one temperature to other. Second we want…

Q: 5.40 A 50.75-g sample of water at 75.6°C is added to asample of water at 24.1°C in a…

A: The heat 'q' required to raise the temperature of a sample of mass 'm' having specific heat 'c' from…

Q: A 307-g sample of an unknown mineral was heated to 98/1°C and placed into a calorimeter containing…

A: Click to see the answer

Q: Suppose 0.100 mol of a metal (M) is combusted in excess O2lg) in a bomb calorimeter. 4M(s) + 302 –…

A: Given the moles of metal, M that undergoes combustion = 0.100 mol the heat released during the…

Q: the 10.0 g sample of metal is heated to 100.0 degrees celsius and then added to 20.0 g of water at…

A: The relationship between heat , specific heat capacity and change in temperature is given by the…

Q: Which of the following statements is/are true? I. q (heat) is a state function because ΔH is a state…

A: State function is independent of the path of transformation.  Heat increase/decrease = m×s×dt Where…

Q: The combustion of 2.474 g of propanol (C3H7OH) increases the temperature of a bomb calorimeter…

A: Click to see the answer

Q: ich represents the definition of pressure A) volume x force B) volume/density C) force/area D)…

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

Q: ich represents the definition of pressure A) volume x force B) volume/density C) force/area D)…

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

Q: Suppose 0.100 mol of a metal (M) is combusted in excess O2(g) in a bomb calorimeter. 4M(s) + 302…

A: Given: 4M + 3O2 -----> 2M2O

Q: Suppose 0.562 g of graphiteis place in bomb calorimeter with excess of oxygenat 25.00 °C and 1 atm…

A: Given : Mass of C reacting = 0.562 g Heat capacity of calorimeter = 20.70 KJ/oC Initial temperature…

Q: consider a mixture of air and gasoline vapor and a cylinder with a piston and an original volume of…

A: Click to see the answer

Q: One mole of H2O(g) at 1.00 atm and 100 C occupies a volume of 30.6L. When 1 mole of H2O (g) is…

A: Introduction: Internal energy (E) is equal to the difference between the heat transfer (Q) into a…

Q: Consider the following chemical reaction: C2H6O(l) + O2(g) -----------> CO2(g) + H2O(g)  0.8100 g…

A: Click to see the answer

Q: The atmosphere inside the room has 35 mol of CO2.The temperature decreases by 22°C.Solve for heat (…

A: The total heat absorbed by the CO2 is calculated as shown below. Q=nCO2Cm∆T

Q: An Ideal Gas system transfers 1810 kJ of heat to the surrounding and its volume is changed from…

A: Click to see the answer

Q: A 100.0-g Al metal cube at 95.0o C is added to 250.0 g of water at 22.0o C in a coffee-cup…

A: Given : Mass of Al metal = 100.0 g Initial temperature of metal = 95.0 oC Initial temperature of…

Q: Calculate q,w,ΔE, and ΔH for the process in which 77.3 g of nitrous oxide (laughing gas, N2O) is…

A: Solution:      The molar heat capacity of a substance is defined as the amount of energy added to…

Q: A balloonist is preparing to make a trip in a helium-filled bal-loon. The trip begins in early…

A: Since your question has multiple sub-parts, we will answer the first three sub-parts for you. If you…

Q: Consider an ideal gas in a piston chamber where the initial volume is 2.00L and the initial pressure…

A: A.) To calculate work of the process , we would use formula : w = Pext ∆V    B.) To calculate final…

Q: Suppose 0.562 g of graphite is place in bomb calorimeter with excess of oxygen at 25.00 °C and 1 atm…

A: Heat is a source of energy that induces a change in the temperature of any material. The heat…

Q: At constant volume, the heat of combustion of a particular compound is - 3800kJ / m * o * l . When…

A: Click to see the answer

Q: 5.38 A 0.1375-g sample of solid magnesium is burned ina constant-volume bomb calorimeter that has a…

A: Calculate the heat energy absorbed by the calorimeter,         qCal = Ccal ∆T= 3024 J0C × 1.126 0C ×…

Q: 5.38 A 0.1375-g sample of solid magnesium is burned ina constant-volume bomb calorimeter that has a…

A: The given data contains, heat capacity = 3024 j/°C. Change in temperature = 1.126°C Mass of sample =…

Q: 5.38 A 0.1375-g sample of solid magnesium is burned ina constant-volume bomb calorimeter that has a…

A: The formula of the number of moles is shown below. If the heat is released by the system then the…

Q: 5.38 A 0.1375-g sample of solid magnesium is burned ina constant-volume bomb calorimeter that has a…

A: The given data contains, mass = 0.1375 g. Heat capacity = 3024 J/°C Temperature=1.126°C

Q: 5.38 A 0.1375-g sample of solid magnesium is burned ina constant-volume bomb calorimeter that has a…

A: Given details, Ccal=3024 J∆T = 1.126°C The mass of magnesium = 0.1375 g To calculate the heat given…

Q: Consider the reaction  H2(g) + Cl2(g) → 2HCl(g) ΔH = −184.6 kJ / mol If 7.00 moles of H2 react with…

A: Given,

Q: The specific heat capacity of lead at 25°C is 1.290×10-1 J/g/K. Answer the following: (a) For a…

A: Click to see the answer

Q: A quantity of 1.922 g of me thinks was burned in a constant-volume bomb calorimeter. Consequently…

A: Molar heat of the combustion of methanol is the amount of heat energy released when 1 mol of…

Q: A gas expands against a constant external pressure of 2.00 atm until its volume has increased from…

A: Constant pressure = 2 atm Vf  = 10 L Vi = 6L Volume change ΔV =

Q: The atmosphere insde the room has 35 mol CO2. The temperature decreases by 22 celcius. Solve for…

A: Given,  n = 35 mole ∆T = 22 celcius C = 37.27 J/degree celcius mole

Q: V. The thermochemical equation for the incomplete combustion of carbon into carbon monoxide is…

A: Given:  Reaction (1):  C(s) + O2(g) ---> CO2(g)                      ∆H1 = -393.5 kJ  Reaction…

Q: Calculate ΔE for a gas that releases 4.93 kJ of heat at the same time as it is compressed from 11.60…

A: The relationship between ΔE and heat and work is given by  ΔE = q + w  where w = work done on system…

Q: The combustion of fructose (C6H12O6, MW = 180.16 g/mol) takes place according to the following…

A: The combustion of fructose results in the production of heat. This heat is utilized by the bomb…

Q: A gas is allowed to expand, at constant temperature, from a volume of 1.0L to 15 L against an…

A: a) To determine the value of q, As 500 J of heat is given to the surroundings, i.e heat is released…

Q: Constants Periodic Table The molar heat capacity of silver is 25.35 J/mol temperature of 8.00 g of…

A: With data's given Each part is solved with heat formula and specific heat, energy is calculated as…

Q: 2.53 g of solid NaOH is dissolved in 100.00 g of water (total mass of solution = 102.53 g) in a…

A: The reaction given is NaOH(s) → NaOH(aq)                     ∆H° = - 43.0 kJ/mol  Hence we can say…

Q: Calculate q, w, AE, and AH for the process in which S1.3 g of nitrous oxide (laughing gas, N2O) is…

A: Heat capacity denotes the amount of heat required to increase the temperature by 1°C. The…

Q: Automobile airbags contain solid sodium azide, NaN3,NaN3, that reacts to produce nitrogen gas when…

A: Given information, Mass of NaN3 = 32.5 g Pressure of the gas = 1.00 atm Temperature of gas =  22°C =…

Q: A 30.9 g sample of copper at 99.8 °C is carefully placed into an insulated container containing 196…

A: Click to see the answer

Q: A 47.70 mL volume of 1.00 M HCl was mixed with 47.30 mL of 2.00 M NaOH in a coffee cup calorimeter…

A: The specific heat capacity of a given substance can be defined as the amount of heat which is needed…

Q: Which of the following constants is/are needed to calculate the amount of ener required to heat…

A: The answer to the following question is-

Q: (a) When a 0.235-g sample of benzoic acid is combustedin a bomb calorimeter (Figure 5.19), the…

A: Given 0.235 g sample of benzoic acid is combusted .Temperature rises=1.642°CHeat combustion of…

Q: A cylinder confines 2.00 L gas under a pressure of 1.00 atm.The external pressure is also 1.00 atm.…

A: Click to see the answer

Q: When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of FeCl2(s) and 8.60 kJ of heat is…

A: Given, Produced mass of FeCl2 is 3.22 g Produced heat is 8.60 kJ Molar mass of FeCl2 is 126.751…

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
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
    Chemistry
    Chemistry
    ISBN:9781259911156
    Author:Raymond Chang Dr., Jason Overby Professor
    Publisher:McGraw-Hill Education
    Principles of Instrumental Analysis
    Chemistry
    ISBN:9781305577213
    Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
    Publisher:Cengage Learning
  • Organic Chemistry
    Chemistry
    ISBN:9780078021558
    Author:Janice Gorzynski Smith Dr.
    Publisher:McGraw-Hill Education
    Chemistry: Principles and Reactions
    Chemistry
    ISBN:9781305079373
    Author:William L. Masterton, Cecile N. Hurley
    Publisher:Cengage Learning
    Elementary Principles of Chemical Processes, Bind...
    Chemistry
    ISBN:9781118431221
    Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
    Publisher:WILEY
  • Chemistry
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
    Chemistry
    Chemistry
    ISBN:9781259911156
    Author:Raymond Chang Dr., Jason Overby Professor
    Publisher:McGraw-Hill Education
    Principles of Instrumental Analysis
    Chemistry
    ISBN:9781305577213
    Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
    Publisher:Cengage Learning
    Organic Chemistry
    Chemistry
    ISBN:9780078021558
    Author:Janice Gorzynski Smith Dr.
    Publisher:McGraw-Hill Education
    Chemistry: Principles and Reactions
    Chemistry
    ISBN:9781305079373
    Author:William L. Masterton, Cecile N. Hurley
    Publisher:Cengage Learning
    Elementary Principles of Chemical Processes, Bind...
    Chemistry
    ISBN:9781118431221
    Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
    Publisher:WILEY