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

Option: 1

\mathrm{0.44\times10^{5}\: N/m^{2}}


Option: 2

\mathrm{0.84\times10^{5}\: N/m^{2}}


Option: 3

\mathrm{0.94\times10^{5}\: N/m^{2}}


Option: 4

\mathrm{0.34\times10^{5}\: N/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
 

Posted by

Divya Prakash Singh

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