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Two moles of Helium gas (\gamma=5 / 3) are initially at temperature 27^{\circ} \mathrm{C} and occupy a volume of 20 litres. The gas is first expanded at constant pressure until the volume is doubled. Then it undergoes an adiabatic change until the temperature returns to its initial value.

Question :  What are the final pressure of gas?

Option: 1

\quad 0.44 \times 10^{5} \mathrm{~N} / \mathrm{m}^{2}


Option: 2

\quad 0.84 \times 10^{5} \mathrm{~N} / \mathrm{m}^{2}


Option: 3

\quad 0.94 \times 10^{5} \mathrm{~N} / \mathrm{m}^{2}


Option: 4

\quad 0.34 \times 10^{5} \mathrm{~N} / \mathrm{m}^{2}


Answers (1)

best_answer

 final pressure

\mathrm{P}_{\mathrm{C}}=\frac{\mathrm{nRT}_{\mathrm{C}}}{\mathrm{V}_{\mathrm{C}}}=\frac{2 \times 8.3 \times 300}{113.13 \times 10^{-3}}=0.44 \times 10^{5} \mathrm{~N} / \mathrm{m}^{2}

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