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  • A closed system containing 5 moles of an ideal gas undergoes a process in which the initial temperature is 300 K, the final temperature is 450 K, and the heat transfer to the system is 1200

A closed system containing 5 moles of an ideal gas undergoes a process in which the initial temperature is
300 K, the final temperature is 450 K, and the heat transfer to the system is 1200 J. Determine the change
in entropy (S) of the gas during this process.

Given:

Initial temperature\mathrm{\left(T_1\right)} = 300 K
Final temperature\mathrm{\left(T_2\right)} = 450 K
Heat transfer (Q) = 1200 J
The gas is ideal.

The specific gas constant (R) for the ideal gas is approximately  8.314 \mathrm{~J} /(\mathrm{mol} \cdot \mathrm{K}) \text {. }

Option: 1

5 \mathrm{~J} / \mathrm{K}


Option: 2

4 \mathrm{~J} / \mathrm{K}


Option: 3

6 \mathrm{~J} / \mathrm{K}


Option: 4

7 \mathrm{~J} / \mathrm{K}


Answers (1)

best_answer

The change in entropy (?S) of the gas during a process can be calculated using the heat transfer (Q) and
the initial and final temperatures \mathrm{\left(T_1 \text { and } T_2\right) \text { : }}

\mathrm{\Delta S=\frac{Q}{T} \quad \text { (for an ideal gas) }}

Substitute the given values:

Q = 1200 J, T =\mathrm{ T_1} = 300 K

Calculating the value of ?S:    \mathrm{\Delta S=\frac{1200 \mathrm{~J}}{300 \mathrm{~K}}=4 \mathrm{~J} / \mathrm{K}}

The change in entropy (?S) of the gas during this process is \mathrm{4 \mathrm{~J} / \mathrm{K} .}
So, option B is correct

Posted by

manish painkra

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