Question

work done by 16 gms of methane gas when it undergoes isothermal reversible expansion from 1 lit to 10 lit at 27 degree celsius

Answer 1

Answer:

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Answer 2

Question:

Work done by 16 g of methane gas when it undergoes isothermal reversible expansion from 1 L to 10 L at 27°C.

Answer:

Work done by the system = - 5744.13 joules

GIVEN:

Mass = 16 g

T = 27°C

${v_2}=10\:L\\{v_1}=1\:L$

TO FIND:

Work done by the system.

Formula:

W = - 2.303 n × R × T × log($\frac{v_2}{v_1}$)

n = number of moles

R = universal gas constant

T = Tempetature in kelvin

v = volume

NEEDED VALUES:

n = mass / molecular mass

molecular mass of C$H_4$ = 12 + 4 = 16 mol/g

n = 16/16

n = 1 mole

1° C = 273 K

27° C = 273 + 27 = 300K

EXPLANATION:

W = - 2.303 × 1 × 8.314 × 300 × log(10/1)

log (10/1) = 1

W = - 2.303 × 1 × 8.314 × 300 × 1

W = - 5744.13 joules

Work done by the system = - 5744.13 joules

Work done by the system is always negative in chemical thermodynamics.

NOTE: CALCULATION IS GIVEN IN ATTACHMENT.