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DanielleElmas [232]
3 years ago
5

Suppose a system receives a "deposit" of work from the surroundings and loses a "withdrawal" of heat to the surroundings. Can we

determine the sign of ΔE for this process?
A. No, because we are not given specific values for w and q.
B. No, because it an open system.
C. Yes, because we know the signs of w and q.
D. No, because we do not know the temperature of the system
Chemistry
1 answer:
Mars2501 [29]3 years ago
7 0

Answer:

A. No, because we are not given specific values for w and q.

Explanation:

The change of internal energy of a system is:

ΔE = q + w

where q represents heat and w represents work.

It is necessary to know the magnitude and the sign of q and w in order to know if the system's internal energy is increasing or decreasing.

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2 years ago
C3H8(g) + 5O2(g) ⟶ 3CO2(g) + 4H2O(g) H = -2220 kJ If 865.9 g of H2O is produced during this combustion, how much heat is generat
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Answer:

3 × 10⁴ kJ

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Step 1: Write the balanced thermochemical equation

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Step 2: Calculate the moles corresponding to 865.9 g of H₂O

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