Question

Calculate the work done during isothermal and reversible expansion of 2 moles of an ideal gas from 10L to 100L at 300K

Answer 1

Answer:

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Answer 2

The work done during isothermal and reversible expansion of 2 moles of an ideal gas from 10L to 100L at 300K is 11488.3 Joules

Explanation:

To calculate the work done for isothermal, reversible expansion process, we use the equation:

$W=-2.303nRT\log(\frac{V_2}{V_1})$

where,

W = work done

n = number of moles = 2 mole s

R = Gas constant = 8.314 J/mol.K

T = Temperature of the gas = $300K$

$V_1$ = initial volume = 10 L

$V_2$ = final volume = 100 L

Putting values in above equation, we get:

$W=-2.303\times 2mol\times 8.314J/mol.K\times 300K\times \log(\frac{100}{10})\\\\W=-11488.3J$

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