Response:
q < 0, w > 0, the sign of ΔE cannot be ascertained from the provided details
Explanation:
Assessing the sign of q
The water bath's temperature before the reaction is at 25 °C
Following the reaction, the water bath's temperature rises to 28 °C, suggesting that heat was released from the system during the reaction.
If heat is absorbed by the system, q is positive; if heat is released, q is negative, leading to the conclusion that q < 0 in this scenario.
Determining the sign of w
The downward movement of the piston indicates a reduction in the system's volume, meaning work was conducted on the system. When work is done on the system, w is considered positive; hence, w > 0 in this case.
Evaluating ΔE sign
According to the first law of thermodynamics, the relationship among ΔE, q, and w is represented as follows:
ΔE = q + w
In this instance, since q is negative and w is positive, the resulting sign of ΔE is determined by the relative magnitudes of q and w. Since we lack sufficient information to gauge these magnitudes, we cannot definitively determine the sign of ΔE based on the given data.
As a result, the correct option among the choices presented is c: q < 0, w > 0, the sign of ΔE cannot be discerned from the information given.
