22. The First Law of Thermodynamics

First Law of Thermodynamics

22. The First Law of Thermodynamics

First Law of Thermodynamics

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The First Law of Thermodynamics

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Alternate Equation of the First Law of Thermodynamics

Patrick Ford

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Calculating Work Done on Monoatomic Gas

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First Law of Thermodynamics

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The First Law Thermodynamics - Physics Tutor

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Simplifying the First Law of Thermodynamics | Physics by Parth G

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First Law of Thermodynamics

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FIRST LAW OF THERMODYNAMICS | Easy and Short

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The First Law of Thermodynamics: Internal Energy, Heat, and Work

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Multiple Choice

A gas in a cylinder held at a constant pressure 1.80×10⁵ Pa expands from a volume of 1.2 m³ to 1.6 m³. The internal energy of the gas decreases from 4.40×10⁵ J to 3×10⁵ J. How much heat was transferred to the gas?

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Multiple Choice

The internal energy of a system decreases by 500 J, and 230 J of work is done on the system. What is the heat transfer into or out of this system?

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Textbook Question

An experimenter adds 970 J of heat to 1.75 mol of an ideal gas to heat it from 10.0°C to 25.0°C at constant pressure. The gas does +223 J of work during the expansion. (b) Calculate γ for the gas.

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Textbook Question

Boiling Water at High Pressure. When water is boiled at a pressure of 2.00 atm, the heat of vaporization is 2.20 * 10^6 J/kg and the boiling point is 120°C. At this pressure, 1.00 kg of water has a volume of 1.00 * 10^-3 m^3 , and 1.00 kg of steam has a volume of 0.824 m^3. (b) Compute the increase in internal energy of the water.

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Textbook Question

A gas in a cylinder is held at a constant pressure of 1.80 * 10^5 Pa and is cooled and compressed from 1.70 m^3 to 1.20 m^3. The internal energy of the gas decreases by 1.40 * 10^5 J. (c) Does it matter whether the gas is ideal? Why or why not?

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Textbook Question

Five moles of an ideal monatomic gas with an initial temperature of 127°C expand and, in the process, absorb 1500 J of heat and do 2100 J of work. What is the final temperature of the gas?

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Textbook Question

Propane gas (C3H8) behaves like an ideal gas with g = 1.127. Determine the molar heat capacity at constant volume and the molar heat capacity at constant pressure

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Textbook Question

Heat Q flows into a monatomic ideal gas, and the volume increases while the pressure is kept constant. What fraction of the heat energy is used to do the expansion work of the gas?

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Textbook Question

Boiling Water at High Pressure. When water is boiled at a pressure of 2.00 atm, the heat of vaporization is 2.20 * 10^6 J/kg and the boiling point is 120°C. At this pressure, 1.00 kg of water has a volume of 1.00 * 10^-3 m^3 , and 1.00 kg of steam has a volume of 0.824 m^3. (a) Compute the work done when 1.00 kg of steam is formed at this temperature.

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Textbook Question

A gas in a cylinder expands from a volume of 0.110 m^3 to 0.320 m^3 . Heat flows into the gas just rapidly enough to keep the pressure constant at 1.65 * 10^5 Pa during the expansion. The total heat added is 1.15 * 10^5 J. (a) Find the work done by the gas.

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Textbook Question

Six moles of an ideal gas are in a cylinder fitted at one end with a movable piston. The initial temperature of the gas is 27.0°C and the pressure is constant. As part of a machine design project, calculate the final temperature of the gas after it has done 2.40 * 10^3 J of work.

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Textbook Question

A rapidly spinning paddle wheel raises the temperature of 200 mL of water from 21°C to 25°C . How much (a) heat is transferred?

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Textbook Question

An experiment you're designing needs a gas with r = 1.50. You recall from your physics class that no individual gas has this value, but it occurs to you that you could produce a gas with r = 1.50 by mixing together a monatomic gas and a diatomic gas. What fraction of the molecules need to be monatomic?

Textbook Question

n moles of a diatomic gas with Cv = 5/2 R has initial pressure pᵢ and volume Vᵢ. The gas undergoes a process in which the pressure is directly proportional to the volume until the rms speed of the molecules has doubled. b. How much heat does this process require? Give your answer in terms of n, pᵢ and Vᵢ.

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