le Inbox 2336) I Desmos Grap mod/ibis/view.php?id 2435708 e CHE 102; x aDThermod

Question

le Inbox 2336) I Desmos Grap mod/ibis/view.php?id 2435708 e CHE 102; x aDThermodynai 1 G A Critical Rea rw stion 30 of 30 Map Map d The following equation represents the decomposition of a generic diatomic element in its standard state. Assume that the standard molar Gibbs energy of formation of Xig) is 4.30 kJ mo at 2000. K and -59.00 kJ. mor' at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature. At 2000. K, we were given. AG-4.30 kJ-mor, what is K at that temperature? Number K at 2000. K- At 3000. K, we were given: G =-59 00 k/ mor! What is K at that temperature? Number K at 3000. K- Prevous Give Up & View Solution 9 Check Answer Next Exit about us careers partners privacy policy terms of use contact us help

Explanation / Answer

Standard molar Gibbs energy (0G) and an equilibrium constant (K) are related as,

0G = -RTln(K) …………… (1)

Where,

0G = Standard molar Gibbs energy in J/mol

R = Molar gas constant = 8.314 J.K-1.mol-1

T = Temperature in K.

K = Equilibrium Constant

1)

Given data: T = 2000 K, 0Gf = 4.30 kJ/mol = 4300 J/mol

Using eq. (1),

4300 = -8.314 x 2000 ln(K)

4300 = -16628 ln(K)

ln(K) = 4300 /(-16628)

ln(K) = -0.2586

K = e-0.2586

K = 0.772

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2)

Given data: T = 3000 K, 0Gf = -59.00 kJ/mol = -59000 J/mol

Using eq. (1),

-59000 = -8.314 x 3000 ln(K)

-59000 = -24942 ln(K)

ln(K) = -59000 /(-24942)

ln(K) = 2.3655

K = e2.3655

K = 10.65

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