What is the work performed by a gas if it expands from 4.44 L to 6.19 L against a constant external pressure of 1.26 atm? Express the final answer in joules. O -4.42 x 102j O-2.23 x 102 J -448 J -242 J

What is the work performed by a gas if it expands from 4.44 L to 6.19 L against a constant external pressure of 1.26 atm? Express the final answer in joules. O -4.42 x 102j O-2.23 x 102 J -448 J -242 J

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 106AE

See similar textbooks

Related questions

Q: A change in a system occurs such that 92.1 J of heat flows in to the system and 31.8 J of work is…

A: From the first law of thermodynamics, ∆U = Q - W where, ∆U = change in internal energy Q = heat…

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: What is the value of the work for a system if the work done by the system is it expanding from 8.50…

Q: The AE of a system that absorbs 252.4 J of heat and has 120.8 J of work done on it by the…

A: According to first law of thermodynamics ∆E=Q-W where Q = heat absorbed by system W =…

Q: When a particular gas expands against a constant external pressure of 1.00 bar, it does 5 J of work…

Q: The AU of a system that absorbs 12.4 J of heat and does 4.2 J of work on the surroundings is J. O…

A: Detail mathematical calculation is shown below to find out the change in internal energy

Q: A gas expands from a volume of 0.754 L to 3.25 L against a constant pressure of 1.15 atm. What is…

A: Nearest value is -2. 91J so first option seems to be correct.

Q: Calculate the work done (in Joules) during the combustion of hydrazine, a component of rocket fuel,…

A: For the given reaction, work done is calculated by using the formula as shown below : Work done =…

Q: 9. If 10 L of an ideal gas at a pressure of 2 atm is cooled so that it contracts 1 at constant…

Q: A gas expands from 2.00 L to 3.65 L, against a pressure of 0.485 atm, at constant temperature. What…

Q: What is the change in internal energy of the system (in J)?

A: From the first law of thermodynamic we know that , du=dq+dw where du = change in internal energy…

Q: 1. A system is compressed from 50.0 L to 5.0L at a constant pressure of 10.0 atm. What is the amount…

Q: Calculate the work (kJ) done during a reaction in which the internal volume expands from 23 L to 58…

A: Given data,Initial volume=23LFinal volume=58LPressure=0atm

Q: When 1177 J1177 J of heat energy is added to 39.1 g39.1 g of hexane, C6H14,C6H14, the temperature…

A: Heat supplied to a system and change in temperature of system due to it can be correlated as…

Q: A student runs a reaction in a closed system. During the reaction, 64.7 kJ of heat is released to…

A: According to the first law of thermodynamics, the energy of the universe remains constant. For a…

Q: 22. What is the change in internal energy (AE) when a system is heated with 35 J of energy while it…

A: According to the 1st law of thermodynamics: change in internal energy = q + W where as, q-->>…

Q: Suppose a system returns to its original internal energy after the following changes. In step 1, 25…

A: It is given that in first step system releases 37 J of energy which means q = -37 and the work is…

Q: If 749 cal is added to a gas that expands and does 817 J of work, what is the change in the internal…

Q: Calculate the value of internal energy if 670J of heat energy is absorbed by the surrounndings and…

Q: Calculate the work done by a system when a piston expands from a volume of 13.27 L to 76.55 L…

Q: When a 3.00-g sample of liquid octane (Cg H18) burns in a bomb calorimeter, the temperature of the…

A: The amount of heat released in the combustion of 3 g liquid octane gets absorbed by the calorimeter.…

Q: A piston holding a gas compresses from 4 L to 1 L under an external pressure of 3 atm. What is the…

A: The change in the volume of the gas is = 4 L - 1L = 3 L The external pressure of the gas is = 3 atm…

Q: Oxygen gas at 34.5 °C is compressed from 45.7 L to 34.5 L against a constant pressure of 750 mmHg.…

A: We need to calculate work done by the system when oxygen gas is compressed from 45.7 L to 34.5 L at…

Q: A mixture of helium and neon gas is expanded from a volume of 87.0L to a volume of 96.0L, while the…

A: Work done = pressure x change in volume

Q: A certain gas expands in volume from 2.0 L to 24.5 L at constant temperature. Calculate the work…

Q: Calculate the work done when a gas is compressed from 121.0 L to 80.0 L at a constant pressure of…

A: work don by the gas at constant pressure is given by W = -PΔV where W = work done by gas P =…

Q: A change in a system occurs such that 92. J of heat flows from the system to the surroundings and…

A: Given data :- Change in Heat (∆q) = 92.7 joule Work(w) =14.2 joule Change in internal energy (∆U) =…

Q: 31. A 345 J of work was done on the system. At the same time, the system absorbs 148 J heat from the…

A: According to the first law of thermodynamics, the energy of the universe remains constant. For a…

Q: What is the work performed when a gas expands from 0.25 L to 2.33 L against an external pressure of…

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

A: According to the first law of thermodynamics ; change in internal energy is given by the sum of heat…

Q: In your constant-volume bomb calorimeter, you have a 0.3677 g sample of Potassium. The water…

A: Calculation of change in internal energy ∆U: The heat evolved at constant volume is called change in…

Q: A0.1857 g sample of the generic hydrocarbon CxHy was burned in a constant volume calorimeter. As a…

A: Given: Mass of hydrocarbon reacted = 0.1857 g. Heat of combustion of hydrocarbon =71.34 KJ/g = 71340…

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

A: According to the first law of thermodynamics, the energy of the universe remains constant. For the…

Q: 8.A sample of 1 mol ideal gas is heated at constant pressure, when the temperature is raised 1 K,…

Q: A system does 435 kJ of work(w) and loses 312 kJ of heat(q) to the surroundings. What is the change…

Q: The value of ΔE for a system that performs 213 kJ of work on its surroundings and loses 79 kJ of…

Q: Calculate q

Q: Calculate the work, w, done in kJ when a gas contracts from 40.0 L to 5.0 L against a constant…

Q: 1 mole of an ideal gas is at 6 atm pressure, occupies 3 L and has an internal energy of 2735.1 J.…

A: Here the system undergoes two different paths. Path-1 is constant volume process Path-2 is constant…

Q: - In which of the following systems is(are) work done by the surroundings on the system? Assume…

Q: A change in a system occurs such that 13.6 J of heat flows in to the system and 13.4 J of work is…

A: Given heat flowing into the system = 13.6 J work done by the surroundings = 13.4 J

Q: A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings. If the initial…

A: According to 1st law of thermodynamics:-∆u=q+wwhere,∆u= cange in internal energyq= heat given to the…

Q: Calculate the work done by a gas when its volume expands from 3.0L to 8.0L under atm. How much heat…

A: Work done (w) : w =-Pext.Vf-Viw = -1×8.0-3.0w = - 5 L.atmw = -5 ×101.325 Jw = - 506.625 J Given :…

Q: What is the change in internal energy of the system (AU) if 82 kJ of heat energy is absorbed by the…

A: According to the first law of thermodynamics, the internal energy is equal to the sum of heat…

Q: A system expands from a volume of 1.00 L to 2.00 L against a constant external pressure of 1.00 atm.…

Q: Calculate the work, in joules, done on or by the system when the volume of the system is changed…

Q: The work done to compress a sample gas is "X". At the same time, the surroundings absorb “Y" of…

Q: 2. A certain gas expands in volume from 2.0 L to 6.0 L at constant temperature. Calculate the work…

Q: Consider the following changes:a.N2 (g) → N2 (l)b.CO (g) + H2O (g) → H2 (g) + CO2 (g)c.Ca3P2 (s) +…

A: Work done: The work is a transfer of energy from one system to another system without the change in…

Q: A system does 435 kJ of work(w) and loses 312 kJ of heat(q) to the surroundings. What is the change…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Question

What is the work performed by a gas if it expands from 4.44 L to 6.19 L against a
constant external pressure of 1.26 atm? Express the final answer in joules.
O -4.42 x 102j
-2.23 x 102 J
-448 J
-242 J

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 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

As a gas cools, it is compressed from 2.50 L to 1.25 L under a constant pressure of 1.01 105 Pa. Calculate the work (in J) required to compress the gas.
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?
In which of the following systems is(are) work done by the surroundings on the system? Assume pressure and temperature are constant. a. 2SO2(g)+O2(g)2SO3(g) b.CO2(s)CO2(g) c. 4NH3(g)+7O2(g)4NO2(g)+6H2O(g) d.N2O4(g)2NO2(g) e.CaCO3(s)CaCO(s)+CO2(g)
A balloon expands from 0.75 L to 1.20 L as it is heated under a constant pressure of 1.01 105 Pa. Calculate the work (in J) done by the balloon on the environment.
Dry ice is solid carbon dioxide; it vaporizes at room temperature and normal pressures to the gas. Suppose you put 21.5 g of dry ice in a vessel fitted with a piston (similar to the one in Figure 6.9 but with the weight replaced by the atmosphere), and it vaporizes completely to the gas, pushing the piston upward until its pressure and temperature equal those of the surrounding atmosphere at 24.0C and 751 mmHg. Calculate the work done by the gas in expanding against the atmosphere. Neglect the volume of the solid carbon dioxide, which is very small in comparison to the volume of the gas phase.
A sample of benzene, C6H6, weighing 3.51 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 37.18C. If the heat capacity of the calorimeter and contents was 12.05 kJ/C, what is the value of q for burning 1.00 mol of benzene at constant volume and 25.00C? The reaction is C6H6(l)+152O2(g)6CO2(g)+3H2O(l) Is q equal to U or H?
A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 33.73C. If the heat capacity of the calorimeter and contents was 9.63 kJ/C, what is the value of q for burning 1.00 mol of ethanol at constant volume and 25.00C? The reaction is C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) Is q equal to U or H?
Calculatethe work performed by a person whoexertsa force of 30 NN = newtonstomove abox 30metersif the force were a exactly parallel to the directionofmovement, and b45to thedirection of movement. Do the relative magnitudesmakesense?
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.
When 1.0 g of fructose, C6H12O6(s), a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 1.58 C. If the heat capacity of the calorimeter and its contents is 9.90 kJ/C, what is q for this combustion?
9.42 Why is enthalpy generally more useful than internal energy in the thermodynamics of real world systems?
Calculate E for each of the following. a. q = 47 kJ, w = + 88 kJ b. q = +82 kJ, w = 47 kJ c. q = + 47 kJ, w = 0 d. In which of these cases do the surroundings do work on the system?