A thermochemical system does 10 kJ of work and gains 25 kJ of heat. The total energy change in the system, represented by ΔE, is calculated by adding the heat and work together, giving a value of 35 kJ.
In a thermochemical system, work and heat are two forms of energy transfer.
1. Work (w) refers to the energy transferred when a force is applied to move an object over a distance. In this case, the system does 10 kJ of work, which means that it has transferred 10 kilojoules of energy by doing mechanical work.
2. Heat (q) refers to the energy transferred due to a temperature difference. In this case, the system gains 25 kJ of heat, meaning that it absorbs 25 kilojoules of energy from its surroundings.
It is important to note that in a thermochemical system, the energy change (ΔE) is equal to the sum of heat (q) and work (w) done by or on the system. Therefore, ΔE = q + w.
Substituting the given values, we have:
ΔE = 25 kJ + 10 kJ
ΔE = 35 kJ
Therefore, the energy change in the system is 35 kilojoules.
In summary, a thermochemical system does 10 kJ of work and gains 25 kJ of heat. The total energy change in the system, represented by ΔE, is calculated by adding the heat and work together, giving a value of 35 kJ.
The complete question could be A thermochemical system does 10 kJ work and gains 25 kJ heat. kJ; ΔΕ = q= kJ; w= kJ