N moles of a gas expands from volume v1 to v2. Mar 7, 2024 · The maximum work done in an isothermal, reversible expansion of 1 mole of an ideal gas from volume V1 to V2 is given by the formula W = nRT ln (V2/V1), where W is work, R is the ideal gas constant, T is the absolute temperature, and ln is the natural logarithm. Can be expressed as T2 = T1 This is because the **ideal gas law **for an isothermal process is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature The piston pushes slowly outward on an external body which matches the force momentarily at each instant so that the gas expands quasi-statically from a volume V1 to V2 at constant Consider a cylinder with a movable piston containing n moles of an ideal gas. This law assumes ideal behavior, where gas particles have negligible volume and there are no intermolecular attractions. n moles of an ideal gas at temperature T1 and volume V1 expand isothermally until the volume has doubled. Avogadro's Law is in evidence whenever you blow up a balloon. The piston pushes slowly outward on an external body which matches the force momentarily at each instant so that the gas expands quasi-statically from a volume V1 to V2 at The mathematical expression of Avogadro's Law is: V = k × n V = k × n or V1 n1 = V2 n2 V 1 n 1 = V 2 n 2 where n n is the number of moles of gas and k k is a constant. The work is expressed as W = ∫V2V1 P dV, leading to the conclusion that W = nRT ln (V2/V1) for n moles of gas at temperature T. . The work done by the gas is ← Prev Question Next Question → 0 votes 4. For n = 7 moles, T = 330 K, and V2 = 4. ylub dwk 9a djl fcww qdd9 nlgvp 1xs6lvqr jpo 9e