Calculate ??, ?,S, ?,Go, and Kat 298.15 K for the reaction below. Also, calculat

Question

Calculate ??, ?,S, ?,Go, and Kat 298.15 K for the reaction below. Also, calculate K at 374 K. Cl2(g)Br2l)2 BrCI(g) ???' at 298.15 K 14.68 / kJ mol-1 Sm at 298.15 K JK-1 mol1 223.1 152.2 240.1 Enter your answers in the specified units. Do not include units with your answers (a) The standard enthalpy of reaction at 298.15 K is A,HNumberkJ mol (b) The standard entropy of reaction at 298.15 K is A,S Number JK-1 mol-1 (c) The standard Gibbs energy of reaction at 298.15 K is A,GNumber kJ mo (d) The value of the thermodynamic equilibrium constant at 298.15 K is KNumber (e) The value of the thermodynamic equilibrium constant at 374 K is KNumber

Explanation / Answer

(a)

deltaH0r = 2 * deltaH0f(BrCl) - deltaH0f(Br2) - deltaH0f(Cl2) = 2 * ( 14.68 ) - ( 0 ) - ( 0 ) = 29.36 kJ

(b)

deltaS0r = 2 * deltaS0f(BrCl) - deltaS0f(Br2) - deltaS0f(Cl2) = 2*( 240.1 ) - ( 223.1 ) - ( 152.2 ) = 104.9 J/K

(c)

deltaG0r = deltaH0r - TdeltaS0r = 29.36 - 298.15 * ( 0.1049 ) = - 1.92 kJ

(d)

deltaG0r = - R T lnK

lnK = - 1.92 / ( - 0.008314 * 298.15 )

K = e0.7746

K = 2.17

(e)

van't Hoff's equation,

ln( K2 / K1 ) = ( deltaH0 / R ) * [ ( 1 / T1 ) - ( 1 / T2 ) ]

ln( K2 / 2.17 ) = ( 29.36 / 0.008314 ) * [ ( 1 / 298.15 ) - ( 1 / 374 ) ]

ln( K2 / 2.17 ) = 2.40

K2 / 2.17 = 11.0

K2 = 24.0

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