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Thermodynamics Unit Internal Energy, Work and Heat 1. The internal energy of a system increased by 982 J when it absorbed 492 J of heat. Was work done by or on the system? How much work was done? What is ΔV if pressure is constant at 1 atm? €
Internal Energy, Work and Heat. 1. The internal energy of a system increased by 982 J when it absorbed 492 J of heat. Was work done by or on the system? How much work was done? What is ΔV if pressure is constant at 1 atm? 2. A gas in a cylinder was placed in a heater and gained 5500 kJ of heat.
Calculate the work done on the system when it loses 900 J of heat, and its internal energy decreases by 500 J. Solution: Using the first law of thermodynamics: \[W = \Delta U – Q = (-500) – (-900) = 400\, \text{J} \]
1. The internal energy of a system increased by 982 J when it absorbed 492 J of heat. Was work done by or on the system? How much work was done? What is ΔV if pressure is constant at 1 atm? 2. A gas in a cylinder was placed in a heater and gained 5500 kJ of heat.
Heat is the energy transferred from one object to another as the result of a temperature difference between them. Temperature is a measure of the kinetic energy of a molecular motion. Energy is the capacity to do work or supply heat. Work is defined as the distance moved times the force that opposes the motion (w =.
3.4 First law of thermodynamics – internal energy The first law of thermodynamics expresses that energy is conserved, when all forms of energy, including heat, are taken into account.
Describe the work done by a system, heat transfer between objects, and internal energy change of a system; Calculate the work, heat transfer, and internal energy change in a simple process
