Question

n = 4.33 mol of Hydrogen gas is initially at T = 378 K temperature and pi = 2.88

Answer 1

Given n = 4.33 mol

         T = 378 K

      P i = 2.88 x 10 ⁵ Pa

     P f = 9.94 x 10 ⁵ Pa

Initial volume V i = nRT / P i

Where R = Gas constant = 8.314 J / mol - K

Substitute values you get V i = 0.04724 m ³

Final volume V f = P i x V i / P f

                         = 0.0136 m ³

(b).Work done W = nRT ln ( V f / V i )

                         = nRT ln(3.45 )

                         = nRT (1.238 )

                        = 16857 J

(c).Heat emitted Q = W      Since in isothermal process change in internal energy U = 0

                           = 16857 J

(d).Entropy S = Q / T

                    = 44.59 J / K

(e) In adiabatic process P ^1-r T ^r = constant

Pi ^1-r Ti ^r = Pf ^1-r Tf ^r

From this you find T f value