For reactions carried out under standard-state conditions, the equation delta G

Question

For reactions carried out under standard-state conditions, the equation delta G = Delta H - T Delta S becomes Delta G = Delta H - T Delta S. Assuming Delta H and Delta S are independent of temperature, one can derive the equation: In (K_2/K_1) = Delta H/R (T_2 - T_1/T_1 T_2) where K_1 and K_2 are the equilibrium constants at T_1 and T_2, respectively. Given that at 25.0 degree C, K_c is 4.63 Times 10^-3 for the reaction N_2O_4(g) 2NO_2(g) Delta = 58.0 kJ/mol calculate the equilibrium constant at 58.0 degree C. K_c =

Explanation / Answer

T1 = 273+25 = 298 K

T2 = 273+59 = 332 K

ln (K2/K1) =del H /R (T2-T1/ T2*T1)

ln(K2/ 4.63* 10^-3) = 58/0.082 (332-298/ 332*298)

ln(K2/ 4.63* 10^-3) = 0.24

K2/ 4.63* 10^-3 = e^0.24 = 1.27

K2 =4.63* 10^-3 * 1.27 = 5.9 10^-3

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