work done by performing a reversible, isothermal compression of 2 moles of an ideal gas at T = 300K from V1 = 2L to V2 = 1L.

i get -3456 j/mol, but im not overly confident

Thanks

Question

work done by performing a reversible, isothermal compression of 2 moles of an ideal gas at T = 300K from V1 = 2L to V2 = 1L. 

i get -3456 j/mol, but im not overly confident

Thanks

anonymous · Answer

@styx_83
How did you arrive at your answer?

anonymous · Answer

$$w=-\int\limits_{V1}^{V2}PdV  $$
$$pV=nRT$$
$$w=-\int\limits_{V1}^{V2}\frac{ nRT }{ V } dV =-nRT ln \frac {V_2}{V_1}  $$
$$w =-2\cdot 8.314 \cdot 300 \cdot \ln 2 = - 3.458 kJ/mol$$

anonymous · Answer

You have calculated the total work by multiplying by 2.  
$$w=W/n= 3458/2 = 1729j/mole$$

I assume you are using gram molecular wgt also

anonymous · Answer

@gleem Yes, I have made a mistake. What I have written is actually for 2 mols.