Question

the change in internal energy for a given system is -325 j. the same system loses 155 j of energy as heat at the same time that it expands from an initial volume of 15.0 l at 1.00 atm of pressure. what is the final volume of the system, in l? enter your answer without units.

Answer 1

The change in internal energy is -155 J. The work done by the system is -170 J. The final volume of the system is 170 L.

Step-by-step explanation:

The change in internal energy can be calculated using the first law of thermodynamics, which states that the change in internal energy (ΔU) is equal to the heat transferred (Q) minus the work done (W) on the system. In this case, the heat transferred (-155 J) is negative because it is leaving the system, and the work done is zero since no work is being done on the system. Therefore, the change in internal energy is: ΔU = Q - W = -155 J - 0 J = -155 J.

Since the change in internal energy is given as -325 J, we can set up an equation: -325 J = -155 J + W, where W represents the work done by the system. Solving for W, we find: W = -325 J - (-155 J) = -325 J + 155 J = -170 J.

The work done by the system is equal to the force applied (pressure) multiplied by the change in volume. Since the pressure is constant at 1.00 atm, we can use the equation: W = -PΔV, where P is the pressure and ΔV is the change in volume. Rearranging the equation to solve for ΔV, we get: ΔV = -W/P = -(-170 J)/(1.00 atm) = 170 L.