Answer:
q < 0, w > 0, the sign of ΔE cannot be determined from the information given
Explanation:
Determination of sign of q
Temperature of the water bath before the reaction = 25 °C
Temperature of the water bath after the completion of the reaction = 28 °C
After the completion of the reaction, temperature of the water bath is increased that means heat is released during the reaction and flows out of the system.
If heat is absorbed by the system, then q is indicated by positive sign and if heat is released by the system, then q is indicated by negative sign.
As in the given case, heat is released by the system, so sign of q is negative, or q < 0
Determination of sign of w
After the completion of the reaction, piston moved downward, that means volume of the system decreases or compression occur. During the compression, work is done on the system.
if work is done on the system, sign of w is positive.
If work is done by the system, sign of w is negative.
In the given case, work is done on the system, therefore sign of w is positive, or w > 0
Determination of sign of ΔE
Relationship between ΔE, q and w is given by first law of thermodynamics:
ΔE = q + w
In this case, q is positive and w is negative, so the sign of ΔE depends of magnitude of q and w. As magnitude of w and q cannot be determined in this case, thus, the given information is insufficient for the determination of sign of ΔE.
So, among the given option, option c is correct.
q < 0, w > 0, the sign of ΔE cannot be determined from the information given
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