O Question 12 - Test 1 sem 2 20 2 XÔ https://ezto.mheducation.com/ext/map/index.html?_con3con&external_browser=0&launchUrl=https%Saved20_21 iEnter your answer in the provided box.The work done to compress a gas is 69.0 J. As a result, 37.0 J of heat is given off to the surroundings.Calculate the change in energy of the gas.J< Prev12 of 20Nextearch

Given, Heat given off q = 37 J , work done w = 69 J , change on energy ∆U = ?

Answered: The work done to compress a gas is 69.0…

The work done to compress a gas is 69.0 J. As a result, 37.0 J of heat is given off to the surroundings. Calculate the change in energy of the gas.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 22QRT

See similar textbooks

Related questions

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

Q: A system gains 727 kJ of heat, resulting in a change in internal energy of the system equal to +151…

Q: Burning 1.22 g of a fuel causes the water in a calorimeter to increase by 12.7°C. If the calorimeter…

A: Given, Mass of fuel = 1.22 g∆T = 12.7°CHeat capacity of calorimeter , Cc = 3.09 kJ/°cSpecific heat…

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

A: Note - Since you have asked multiple question, we will solve the first question for you. If youwant…

Q: If a system absorbs 155 kJ of heat from its surroundings and the system does 53 kJ of work on its…

Q: The heat capacity of a sample should be divided by which quantity to find the specific heat…

A: When Heat capacity is divided by mass in grams we get specific heat capacity.

Q: If a system has 48.5 J of heat added to it, and the system does 75.5 J of work on its surroundings,…

A: Given q = 48.5 J ( positive as heqat is added )w = -75.5 J ( as work is done by system )

Q: What is heat? How does heat differ from thermal energy? Under what conditions is heat transferred…

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: The temperature of the cooling water as it leaves the hot engine of an automobile is 240 °F. After…

A: Given information:

Q: A system receives 225 J of heat from the surroundings and delivers 428 J of work. What is the change…

A: The first law of thermodynamics states that "energy can neither be created nor destroyed , but can…

Q: 124 kJ of heat is absorbed in a reaction that forms nitric oxide from nitrogen and oxygen, what mass…

A: The mass of NO produced = 41.3478 g The mass of N2 reacted = 19.2984 g

Q: Apply the First Law of Thermodynamics to answer the following: If a system does 475 J of work on…

Q: If a system has 49.5 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, the relationship between work, heat and change in…

Q: A gas that works on the surroundings is equal to 432 J. At the same time, it absorbs 87 J of heat…

A: Work done by the gas on the surrounding means, the energy is reduced from the gas. Heat absorbed by…

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

Q: If 1495 J of heat is needed to raise the temperature of a 333 g sample of a metal from 55.0°C to…

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 work done to compress a gas is 67.0 J. As a result, 29.0 J of heat is given off to the…

A: Given, work done, w = +67.0 J Heat, q = -29.0 J

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

A: Given ; energy added by work = 74 J Energy given to surrounding = 26 J

Q: A system gains 617 kJ of heat, resulting in a change in internal energy of the system equal to +161…

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: What is the change in energy (in J) for a system that lost 344 J of heat to the surroundings, and…

A: Assume that work (w) is done on the system, so w will be positive.Given:Heat lost, Q = - 344 JWork…

Q: The work done to compress a gas is 122 J. As a result, 31 J of heat is given off to the…

Q: A system gains 612 kJ of heat, resulting in a change in internal energy of the system equal to +181…

A: Given,Heat gain (Q)=612kJChange in internal energy(∆U)=181kJ

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

Q: 12. The work done to compress a gas is 50 J. As a result, 20 J of heat is given off to the…

A: Work done to gas = +50 J Heat lost = -20 J

Q: resulting

A: ∆U = q + w Where : ∆U = change internal energy = +166kJ Heat(q) = +762 kJ ( positive value because…

Q: Under what conditions does the enthalpy change equal the heat of a process

Q: The work done when a gas is compressed in a cylinder is 455 J. During this process, there is a heat…

A: To find the energy change, we need to use the formula which contains change in energy, work done and…

Q: What is specific heat? Write the specific heat of water. What is the standard enthalpy?

A: Specific heat and standard enthalpy are related to the concept of thermodynamics. Heat is also known…

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

Q: The work done to compress a gas is 70 J. As a result, 25 J of heat is given off to the…

A: Work done to compress = Work done on the system And work done on the system is taken with a positive…

Q: What is the internal energy of the system that absorbs 90 J of heat and 15 J work done by the…

Q: 1.) How is energy expressed in measurements? 2) Distinguish between heat capacity and specific heat…

A: How the energy expressed in measurements has to be given.

Q: In the laboratory a general chemistry student finds that when 5.26 g of CsClO4(s) are dissolved in…

Q: If 1495 J of heat is needed to raise the temperature of a 327 g sample of a metal from 55.0°C to…

A: The weight of metal is 327 g.The given temperature values are 55.0 ˚C and 66.0 ˚C. The value of q is…

Q: If a system absorbs 155.0 kJ of heat from its surroundings and the system does 75.0 kJ of work on…

A: Answer :- The change in internal energy of the system is +80.0 kJ.…

Q: Both glucose and fructose are simple sugars with the same molecular formula of C6H12 O6 . Sucrose…

A: For part a:

Q: What is the working definition of enthalpy change? A) The change in energy that occurs when…

A: Enthalpy change (∆H) is a state function.

Q: of

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

Q: 5. A system compresses when 457 J of work was done on it at the same time it decreases it energy to…

A: Given, A system 457 J of work done when it compresses, at the same time it decreases energy to 234…

Q: What is heat? How does heat differ from thermal energy? Under what condition is heat transferred…

A: Heat: Heat is a form of energy that is transferred from one body to another because of difference in…

Q: A gas expands and does work on the surroundings equal to 4.92 L atm. At the same time, it releases…

A: Given: Work done (W) = 4.92 L atm Heat released by the system according to sign convention (q) = -…

Q: If a system absorbs 155.0 kJ of heat from its surroundings and the system does 95.0 kJ of work on…

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

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 piece of aluminum with a mass of 250. g is at an initial temperature of 5.0 C. If 24.1 kJ is supplied to warm the Al, calculate its final temperature. Obtain the specific heat capacity of Al from Table 4.1. Table 4.1 Representative Specific Heat Capacities
How many moles of isooctane must be burned to produce loo U of heat under standard state conditions?
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
In the “Chemistry in Focus” segment Firewalking: Magic or Science?, it is claimed that one reason people can walk on hot coals is that human tissue is mainly composed of water. Because of this, a large amount of heat must be transferred from the coals to change the temperature of the feet significantly. How much heat must be transferred to 100.0 g of water to change its temperature by 35 °C?
Consider the following cyclic process carried out in two steps on a gas: Step 1: 45 J of heat is added to the gas, and 10. J of expansion work is performed. Step 2: 60. J of heat is removed from the gas as the gas is compressed back to the initial state. Calculate the work for the gas compression in Step 2.
A7.50-gpiece of iron at 100.0C is dropped into 25.0g of water at 22.0C. Assuming that the heat lost by the iron equals the heat gained by the water,determine thefinal temperature of the iron/watersystem. Assume a heat capacity of water at 4.18 J/g.K and of iron at 0.452J/g.K.
The bomb calorimeter in Exercise 102 is filled with 987 g water. The initial temperature of the calorimeter contents is 23.32C. A 1.056-g sample of benzoic acid (Ecomb = 26.42 kJ/g) is combusted in the calorimeter. What is the final temperature of the calorimeter contents?
A 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 21.8C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, and volumes are additive.
Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A coffee-cup calorimeter at 25C contains 15.0 mL of water at 25C. A 2.00-g sample of MgSO4 is dissolved in the water and 1.51 kJ of heat are evolved. (You can make the following assumptions about the solution: volume=15.0 mL, density=1.00 g/mL, specific heat=4.18J/gC.) (a) Write a balanced equation for the solution process. (b) Is the process exothermic? (c) What is qH2O? (d) What is the final temperature of the solution? (e) What are the initial and final temperatures in F?
An aluminum kettle weighs 1.05 kg. (a) What is the heat capacity of the kettle? (b) How much heat is required to increase the temperature of this kettle from 23.0 C to 99.0 C? (c) How much heat is required to heat this kettle from 23.0 C to 99.0 C if it contains 1.25 L of water (density of 0.997 g/mL and a specific heat of 4.184 J/g C)?
You have the six pieces of metal listed below, plus a beaker of water containing 3.00 102 g of water. The water temperature is 21.00 C. (a) In your first experiment you select one piece of metal and heat it to 100 C, and then select a second piece of metal and cool it to 10 C. Both pieces of metal are then placed in the beaker of water and the temperatures equilibrated. You want to select two pieces of metal to use, such that the final temperature of the water is as high as possible. What piece of metal will you heat? What piece of metal will you cool? What is the final temperature of the water? (b) The second experiment is done in the same way as the first. However, your goal now is to cause the temperature to change the least, that is, the final temperature should be as near to 21.00 C as possible. What piece of metal will you heat? What piece of metal will you cool? What is the final temperature of the water?
9.26 Gas furnaces have achieved impressive efficiency levels largely through the addition of a second heat exchanger that condenses water vapor that would otherwise escape out the exhaust system attached to the furnace. How does this process improve efficiency?