Answered: What is the internal energy of the…

What is the internal energy of the system that releases 0.18956 BTU of energy to the surroundings in the form of heat and has 425 J of work done on it?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 36E

See similar textbooks

Related questions

Q: 4. An amount of heat equal to 2500 J is added to a system, and 1800 J of work is done on the system.…

Q: If a system has 42.0 J of heat added to it, and the system does 25.0 J of work on its surroundings,…

A: According to the first law of thermodynamics, the provided heat is used in increasing the the…

Q: if a system does 25 J of work on its surroundings and is cooled by 35 J, what is the net energy…

Q: A system does 551 kJ of work and loses 236 kJ of heat to the surroundings. What is the change in…

Q: What is the change in the internal energy of a system that absorbs 2,500 J of heat and that does…

A: The given data contains, A System absorbs 2500 J of heat work =7655 J

Q: if 0.0102 moles reacted and 476.5 J of heat were absorbed by the reaction in a coffee cup…

Q: If a system produces 123.0 kJ of heat and does 45.0 kJ of work on the surroundings, what is the AE…

Q: 4. A system receives 75 J of electrical work, delivers 274 J of expansion work, and absorbs 168 J of…

A: Givens : Work done by the system , W = 274 joules Heat absorbed by the…

Q: When 2.00 moles HCl(aq) and 0.500 moles of NaOH(aq) react, the heat released by the reaction is…

A: Given, 2.00 moles HCl(aq) and 0.500 moles of NaOH(aq) react. The chemical reaction, HCl(aq) +…

Q: A system does 566 kJ of work and loses 216 kJ of heat to the surroundings. What is the change in…

A: From the first law of thermodynamic's... Q = ∆E + W Work done by the system = positive Heat losses…

Q: What is the change in internal energy for a system if the system absorbs 537 kJ of heat and does…

A: We have given that Heat absorbed by system =q= 537KJ Work done by system is always negative W =…

Q: A system initially has an internal energy U of 501 J. It undergoes a process during which it…

Q: Suppose we have a closed, un-isolated system. When 483 J of heat was introduced to the system, it…

A: Internal energy is a state function. The symbol used for internal energy is U. The unit used for the…

Q: A system does 467 kJ of work and loses 157 kJ of heat to the surroundings. What is the change in…

A: First law of thermodynamics It states states that heat is a form of energy, and thermodynamic…

Q: A system does 566 kJ of work and loses 216 kJ of heat to the surroundings. What is the change in…

Q: A system releases 689 kJ of heat and does 105 kJ of work on the surroundings. ▾ Part A What is the…

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: During a certain chemical reaction 1,395 J of heat is released from the system and 360 J of work is…

A: Given :- work done on surrounding = 360 J heat released from system = 1395 J To be calculated :-…

Q: A gas does 135 J of work while expanding and, at the same time, absorbs 156 J of heat. What is its…

A: Given :- heat absorbed by system = 156 J work done by gas = 135 J To calculate :- ∆U(in J)

Q: The combustion of fuel in a piston cylinder causes an internal energy change of –2.843E3 kJ. The…

Q: What is the change in internal energy for a system which loses 422 J of heat, and on which 227 J of…

A: According to first law of thermodynamics the change in internal energy is expressed as shown below:

Q: A system does 556 kJ of work and loses 251 kJ of heat to the surroundings. What is the change in…

A: From the first law of thermodynamics we have, ∆E =Q + W Where, ∆E is change in internal energy…

Q: A system receives 825 J of heat and delivers 825 J of work to its surroundings. What is the change…

A: Given:Heat received by system, dQ = 825Jwork done by system, dW=825Jchange in internal energy, dU…

Q: What is the change in internal energy in joules for a system that releases 154 J of heat and does…

A: Since the relationship between work, internal energy change and heat released is given by ΔE=…

Q: A gas is compressed in a piston with 8.80E1 J of work. As a result, 4.2E1 J of heat is given off to…

A: Solving only first question in accordance with the guidelines. We will answer this question using…

Q: 3. A gas does 135 J of work while expanding, and at the same time, it absorbs 156 J of heat. What is…

A: Given: (3) work done by gas=135J Absorbed heat=156J To find: change in internal energy of the…

Q: If a system has 38.5 J of heat added to it, and the system does 75.5 J of work on its surroundings,…

A: According to the first law of thermodynamics,change in internal energy i.e∆U can be calculated by…

Q: A gas expands and does P-V work in the surroundings equal to 279 J. At the same time, it absorbs…

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

Q: An automobile engine provides 646 Joules of work to push the pistons and generates 2258 Joules of…

A: According to the thermodynamics law ∆U = Q + W Given Work done on the piston = - 646 J Heat…

Q: If a system absorbs 155 kJ of heat from its surroundings and the system does 45 kJ of work on its…

A: Given, Amount of heat absorbs by the system q = 155 kJ work done by the system W = 45 kJ We are…

Q: What is the AE of a system if 184 kJ of work is done on the system and it loses 267 kJ of heat?

A: We use the first law of thermodynamic for calculating the change in internal energy. This low state…

Q: 2. What is the work done by a system whenabsorbs 47 J of heat and gain 12 J of energy?

Q: A system releases 648 kJ of heat and does 150 kJ of work on the surroundings. What is the change in…

A: Given,System releases 648 kJWork on the surrounding = 150 kJ

Q: A system receives 425 J of heat and delivers 425 J of work toits surroundings. What is the change in…

A: According to first law of thermodynamics, ∆U = ∆Q - ∆W

Q: A system gains 727 kJ727 kJ of heat, resulting in a change in internal energy of the system equal to…

A: As we know; deltaU = Q + W where delta U is change in internal energy Q = heat produced W =…

Q: A chemical reaction is run in which 152 Joules of heat are generated and 461 Joules of work are done…

A: Given: In a chemical reaction 152 Joules of heat are generated and 461 Joules of work are done by…

Q: When 745 J of energy in the form of heat is transferred from the environment to a gas, the expansion…

A: According to first law of thermodynamics dU = dQ + dW Where dU is change in internal energy, dQ is…

Q: In a gas expansion, 74 J of heat is absorbed from the surroundings, and the energy of the system…

A: Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and…

Q: For a process, 153 J of heat was released by the system and 267 J of work was done on the system.…

A: Thermodynamics is branch of chemistry in which we deal with heat absorbed and heat released in to…

Q: A system receives 575 J of heat and delivers 425 J of work. Calculate the change in the internal…

A: Given data The system absorption heat energy= 575 J The work done by the system = 425 J Internal…

Q: The air in an inflated balloon (the system) absorbs 115 J of heat. As it expands, it does 88 kJ of…

Q: If the molar mass of water is 18.02 g/mol and the specific heat of water is 4.184 J/g.◦C, calculate…

A: The molar mass of water = 18.02 g/mol. The specific heat of water = 4.184 J/g.◦C Molar heat capacity…

Q: If a system absorbs 155.0 kJ of heat from its surroundings and the system does 35.0 kJ of work on…

A: Since we know that according to the first law of Thermodynamics ∆E = q + w Where , ∆E = change in…

Q: What is the change in internal energy for a system if the system absorbs 322 kJ of heat and has…

A: Given that, Heat absorbed by the system q = 322 KJ Work done on the system w = 750.0 KJ

Q: What is the ratio of the net work done by the system during the cycle and the heat absorbed from a…

A: Second Law of thermodynamics : It is impossible for a system operating in a cycle connected to a…

Q: of

A: According to 1st law of thermodynamics Change in internal energy= Q-W Q= heat added to the system…

Q: A gas expands and does 25.6 J of work on the surroundings. At the same time, the gas absorbs 89.6 J…

A: Solution W = 25.6J Since work is done by the system on the surrounding q = 89.6J Heat absorbed that…

Q: A system absorbs 1.54E2 kJ of heat and the surroundings do 1.118E2 kJ of work on the system. What is…

A: 2.618E2 = 2.618 * 10^2 kJ

Q: A system does 501 kJ of work and loses 216 kJ of heat to the surroundings. What is the change in…

Question

What is the internal energy of the system that releases 0.18956 BTU of energy to the surroundings in the form of heat and has 425 J of work done on it?

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

Analysis

VIEW

Calculation

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 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

A gas is cooled and loses 82 J of heat. The gas contracts as it cools, and work done on the system equal to 29 J is exchanged with the surroundings. What are q, w, and U?
The temperature of the cooling water as it leaves the hot engine of an automobile is 240 F. After it passes through the radiator it has a temperature of 175 F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g oC.
Consider the following reaction in the vessel described in Question 57. A(g)+B(g)C(s)For this reaction, E=286 J, the piston moves up and the system absorbs 388 J of heat from its surroundings. (a) Is work done by the system? (b) How much work?
Nitrogen gas (2.75 L) is confined in a cylinder under constant atmospheric pressure (1.01 105 pascals). The volume of gas decreases to 2.10 L when 485 J of energy is transferred as heat to the surroundings. What is the change in internal energy of the gas?
Consider the following reaction in a vessel with a movable piston. R(g)+T(g)X(g)As the reaction takes place, the piston loses 1072 J of heat. The piston moves down and the surroundings do 549 J of work on the system. What is E?
When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?
How much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?
Explain the difference between heat capacity and specific heat of a substance.
A piece of lead of mass 121.6 g was heated by an electrical coil. From the resistance of the coil, the current, and the Time the current flowed, it was calculated that 235 J of heat was added to the lead. The temperature of the lead rose from 20.4C to 35.5C. What is the specific heat of the lead?
Natural gas companies in the United States use the therm as a unit of energy. One therm is 1105 BTU. (a) How many joules are in one therm? (1J=9.48104BTU) (b) When propane gas, C3H8, is burned in oxygen, CO2 and steam are produced. How many therms of energy are given off by 1.00 mol of propane gas?
What mass of acetylene, C2H2(g), must be burned to produce 3420 kJ of heat, given that its enthalpy of combustion is 1301 kJ/mol? Compare this with the answer to Exercise 5.91 and determine which substance produces more heat per gram.
For each of the following reactions, the enthalpy change given is that measured when the numbers of moles of reactants and products taking part in the reaction are as given by their coefficients in the equation. Calculate the enthalpy change when 1.00 gram of the underlined substance is consumed or produced. Ca(s)+Br2(l)CaBr2(s)H=683kJ 6Fe2O3(s)4Fe3O4(s)+O2(g)H=+472kJ 2NaHSO4(s)2NaOH(s)+2SO2(g)+O2(g)H=+806kJ