Question

one mole of an ideal gas is compressed from 500cm3 against a constant pressure of 1.216*10-5 pa.the work involved in process is 36.50 J.calculate the final volume.

Answer 1

ok apply the ideal equation gas that the PV equal to nrt and then after find the pressure in ATM then find the number of moles then apply the equation PV equal to nrt and find the volume volume equals to nrt/p.....

Answer 2

Answer:

The final volume of the gas is $200 cm^3$.

Explanation:

Initial volume of the gas = $V_1=500 cm^3=500\times 10^{-6} m^3=0.0005 m^3$

Final volume of gas = $V_2$

External pressure $p_{ext}= 1.216\times 20^{-5} pa=1.216\times 10^{-5} n/m^2$

The work involved in the system = w = 36.50 J = 36.50 N/m

$w=-p_{ext}\times (V_2-V_1)$

$36.50 N m=-1.216\times 10^{5} N/m^2\times (V_2-0.0005 m^3)$

$V_2=200\times 10^{-5] m^3=200 cm^3$

The final volume of the gas is $200 cm^3$.