What will be the work done (in Latm). When 40g of aragon
assuming ideal gas absorb heat and there is an increasing temperature from 1072.5°c to 1073.5°c at constant pressure?
Answers
The work done at constant pressure is 0.082 Latm.
We have to find the work done, when 40g of Argon assuming ideal gas absorb heat and there is an increasing temperature from 1072.5°C to 1073.5°C at constant pressure.
No of mole of Argon = weight of Argon/atomic weight of Argon = 40/40 = 1 mol
Change in temperature, ΔT = (1073.5°C - 1072.5°C) = 1°C
At constant pressure,
work done, W = P(V₂ - V₁)
Also we know from gas equation, PV₁ = nRT₁ ⇒ V₁ = nRT₁/P
PV₂ = nRT₂ ⇒ V₂ = nRT₂/P
∴ Work done, W = P(nRT₂/P - nRT₁/P) = nR(T₂ - T₁) = nRΔT
R is universal gas constant. i.e., R = 0.082 Latm/mol/°C
∴ Work done , W = 1 mol × 0.082 Latm/mol/°C × 1°C = 0.082 Latm
Therefore the workdone at constant pressure would be 0.082 Latm.
Also read similar questions : An ideal gas with adiabatic exponent γ is heated at constant pressure. It absorbs q amount of heat. Fraction of heat abs...
https://brainly.in/question/6265588
Calculate the work done when two moles of an ideal gas expand isothermally from 5 atmosphere pressure to 2 atmospheric p...
https://brainly.in/question/26024162