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  • Entropy Change and Heat Transfer A container of gas at a temperature of <img alt="300 \mathrm{~K}" src="https://entrancecorner.oncodecogs.com/gif.latex?300%20%5Cmathrm%7

Entropy Change and Heat Transfer

A container of gas at a temperature of 300 \mathrm{~K} is heated, and its volume increases from \mathrm{0.03 \mathrm{~m}^3 \: to \: 0.06 \mathrm{~m}^3}. If \mathrm{800 \mathrm{~J}}of heat is added to the gas during the process, calculate the change in entropy of the gas.
 

Option: 1

2.67 \mathrm{~J}

 


Option: 2

1.70 \mathrm{~J}
 


Option: 3

2.200 \mathrm{~J}
 


Option: 4

2.20 \mathrm{~J}


Answers (1)

best_answer

The change in entropy \mathrm{(\Delta S)}can be calculated using the formula:

\mathrm{ \Delta S=\frac{Q}{T} }

Given:

\mathrm{ Q=800 \mathrm{~J} \quad \text { (heat added) } }

\mathrm{ T=300 \mathrm{~K} \quad \text { (temperature) } }

Calculate the change in entropy:

\mathrm{ \Delta S =\frac{Q}{T} }

\mathrm{ \Delta S =\frac{800 \mathrm{~J}}{300 \mathrm{~K}} }

\mathrm{ \Delta S \approx 2.67 \mathrm{~J} / \mathrm{K} }

Therefore, the correct option is 1.



 

Posted by

HARSH KANKARIA

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