Question

To what temperature (in °C) would you need to heat a gas that has a pressure of 1.86 atm and volume of 1.21 Lat 21.4°C to have it occupy 2.43 L at 2.19 atm?

Answer 1

He know from combination of Charles and Boyel Law - PV - Pq V₂ Where, T, TZ P, = initial pressure V = initial volume T = initial tempenature in Here, Given - Kelvin P, = 1.86 carbon P₂ = final pressure V = 1.21 L N2 = final volume Ti = 21.4°C = (21-4+273)K T2 = final temperature in Kelvin = 294.4 K P₂ = 2.19 atur V₂ = 2.43 L T2 = ?

Accondingly, or, Tzx PV = P2 V2 or, Iz = P2 V 2 * T LV or, T₂ = 2.19 ata x 2.434 * 294.4 K 1.86 stan x 1.21x or, Tz = 696.13 K :: Ty = 696.13 K = (696.13 – 273)°C = 423.13 °C. : The tempenature will be 423.13 °C. Ans.