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For the reaction SbCl 5 (g) = SbCl 3 (g) Cl 2 (g); Delta G^ (SbCl 5 )=-334.34 k /mol; Delta G^ f(SbCl 3 )=-301.25 kJ/mol; Delta * H ^ 0 (SbC * l_{5}) = - 394.34kl / m * o * l; Delta H^ f (SbCl 3 )=-313.80 kJ/mol   Calculate the value of the equilibrium constant (K_{p}) at 800 K and 1 atm pressure . 1.91 * 10 ^ 2 1.71 * 10 ^ 2 1.31 * 10 ^ 3 1.11 * 10 ^ 3 None of the above

For the reaction SbCl 5 (g) = SbCl 3 (g) Cl 2 (g); Delta G^ (SbCl 5 )=-334.34 k /mol; Delta G^ f(SbCl 3 )=-301.25 kJ/mol; Delta * H ^ 0 (SbC * l_{5}) = - 394.34kl / m * o * l; Delta H^ f (SbCl 3 )=-313.80 kJ/mol   Calculate the value of the equilibrium constant (K_{p}) at 800 K and 1 atm pressure . 1.91 * 10 ^ 2 1.71 * 10 ^ 2 1.31 * 10 ^ 3 1.11 * 10 ^ 3 None of the above

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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For the reaction SbCl 5 (g) = SbCl 3 (g) Cl 2 (g);

Delta G^ (SbCl 5 )=-334.34 k /mol;

Delta G^ f(SbCl 3 )=-301.25 kJ/mol;

Delta * H ^ 0 (SbC * l_{5}) = - 394.34kl / m * o * l;

Delta H^ f (SbCl 3 )=-313.80 kJ/mol

 

Calculate the value of the equilibrium constant (K_{p}) at 800 K and 1 atm pressure .

1.91 * 10 ^ 2

1.71 * 10 ^ 2

1.31 * 10 ^ 3

1.11 * 10 ^ 3

None of the above

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