Two gases A and B are placed in container that has a piston. A and B react to form product C. As the reaction occurs, the system loses 1450 J heat to the surrounding. The gas expands and the piston moves upward and the system does 1080 J work. Calculate the change in the internal energy.
By the first law of thermodynamics, we have:
ΔU = Q - W
where ΔU is the change in internal energy, Q is the heat transferred, and W is the work done.
In this problem, Q = -1450 J (heat is lost by the system) and W = 1080 J (work is done by the system). Therefore:
ΔU = -1450 J - 1080 J
ΔU = -2530 J
The change in internal energy is -2530 J.
To calculate the change in internal energy, we need to apply the first law of thermodynamics, which states:
ΔU = Q - W
where:
ΔU is the change in internal energy
Q is the heat added/subtracted to the system
W is the work done by/on the system
In this case, the system loses 1450 J of heat (Q = -1450 J) and does 1080 J of work (W = 1080 J). Plugging these values into the formula, we can find the change in internal energy:
ΔU = -1450 J - 1080 J
Therefore, ΔU = -2530 J.
The change in internal energy is -2530 J.