Answer:
Step-by-step explanation:
Moles of helium ( n ) = 156.7 / 4 = 39.175
Temperature T₁ = 35.73 +273 = 308.73 K
Volume V₁ = V
Pressure P₁ = 3.55 atm
V₂ =1.75 V
a ) For isothermal change
P₁ V₁ = P₂V₂
P₂ = P₁ V₁ / V₂
= 3.55 X V / 1.75 V
= 2.03 atm.
b ) Work done by the gas = nRT ln(V₂/V₁)
= 39.175 X 8.321 X 308.73 X ln 1.75
= 56318.8 J
Work done on the gas = - 56318.8 J
c ) Since there is no change in temperature , internal energy of gas is constant
Q = ΔE + W
ΔE = 0
Q = W
Work done by gas = heat absorbed
heat absorbed = 56318.8 J
d ) Change in the internal energy of gas is zero because temperature is constant.