A LevelPhysicsCIERevision Notes16. Thermodynamics16.2 The First Law of ThermodynamicsThe First Law of Thermodynamics

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The First Law of Thermodynamics (CIE A Level Physics)

Revision Note

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Ann H

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Ann H

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Physics

The First Law of Thermodynamics

  • The first law of thermodynamics is based on the principle of conservation of energy
  • When energy is put into a gas by heating it or doing work on it, its internal energy must increase:

The increase in internal energy = Energy transferred by heating + Work done on the system

  • The first law of thermodynamics is therefore defined as:

increment U space equals space q space plus thin space W

  • Where:
    • ΔU = increase in internal energy (J)
    • q = energy transferred to the system by heating (J)
    • W = work done on the system (J)
  • The first law of thermodynamics applies to all situations, not just for gases
    • There is an important sign convention used for this equation

  • A positive value for internal energy (+ΔU) means:
    • The internal energy ΔU of the system increases
    • Heat q is added to the system
    • Work W is done on the system

  • A negative value for internal energy (−ΔU) means:
    • The internal energy ΔU of the system decreases
    • Heat q is taken away from the system
    • Work W is done by the system

Worked example

The volume occupied by 1.00 mol of a liquid at 50 oC is 2.4 × 10-5 m3. When the liquid is vaporised at an atmospheric pressure of 1.03 × 105 Pa, the vapour has a volume of 5.9 × 10-2  m3. The latent heat to vaporise 1.00 mol of this liquid at 50 oC at atmospheric pressure is 3.48 × 104 J.

Determine for this change of state the increase in internal energy ΔU of the system.

Answer: 

Step 1: Write down the first law of thermodynamics

increment U space equals space q thin space plus thin space W

 

Step 2: Write the value of heating q of the system

  • This is the latent heat, the heat required to vaporise the liquid = 3.48 × 104 J

 

Step 3: Calculate the work done W

W space equals space p increment V

  • ΔV = final volume − initial volume

ΔV = 5.9 × 10-2 − 2.4 × 10-5 = 0.058976 m3

  • p = atmospheric pressure  = 1.03 × 105 Pa
  • W = work done

W = (1.03 × 105) × 0.058976 = 6074.528 = 6.07 × 103 J

  • Since the gas is expanding, this work done is negative

W = −6.07 × 103 J

 

Step 4: Substitute the values into the first law of thermodynamics

ΔU = 3.48 × 104  + (−6.07 × 103) = 28 730 = 29 000 J (2 s.f.)

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    Ann H

    Author: Ann H

    Ann obtained her Maths and Physics degree from the University of Bath before completing her PGCE in Science and Maths teaching. She spent ten years teaching Maths and Physics to wonderful students from all around the world whilst living in China, Ethiopia and Nepal. Now based in beautiful Devon she is thrilled to be creating awesome Physics resources to make Physics more accessible and understandable for all students no matter their schooling or background.