A gas absorbs 25kj of heat and does 12kj of work calculate (triangle) E
To calculate the change in internal energy (∆E) of a gas, we can apply the first law of thermodynamics, which states that the change in internal energy is equal to the heat added to the system minus the work done by the system. Mathematically, it can be represented as:
∆E = Q - W
where ∆E represents the change in internal energy, Q represents the heat added to the system, and W represents the work done by the system.
Given that the gas absorbs 25 kJ of heat (Q = 25 kJ) and does 12 kJ of work (W = 12 kJ), we can substitute these values into the equation:
∆E = 25 kJ - 12 kJ
Calculating the difference:
∆E = 13 kJ
Therefore, the change in internal energy (∆E) of the gas is 13 kJ.
To calculate the change in internal energy (∆E) of a system, you can use the First Law of Thermodynamics, which states that ∆E = Q - W, where Q is the heat absorbed by the system and W is the work done by the system.
Given that Q = 25 kJ (heat absorbed) and W = 12 kJ (work done), you can substitute these values into the equation:
∆E = Q - W
∆E = 25 kJ - 12 kJ
∆E = 13 kJ
Therefore, the change in internal energy (∆E) of the gas is 13 kJ.
Delta (triangle) E is the change in internal energy.
E(final)-E(initial)
25-12= 13 = E(final)
13-25=
-12kj= Delta (triangle)E