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13 Dec 2019

Estimate the value of the equilibrium constant at 640K for eachof the following reactions. ?H?fand S? forBrCl(g) is 14.6 kJ/mol and 240.0 Jmol?K, respectively.

Part A- 2NO2(g)?N2O4(g)
Part B-Br2(g)+Cl2(g)?2BrCl(g)

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Hubert Koch
Hubert KochLv2
17 Dec 2019

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Related questions

For the reaction given below, the value of the equilibrium constant at 400K is 7.0

Br2(g) + Cl2(g) ßà 2BrCl(g)

At equilibrium the concentration of Br2 and Cl2 are each 1 mol/L. What is the equilibrium concentration of BrCl?

a. 49 mol/L

b. 1.0 mol/L

c. 7.0 mol/L

d. 2.6 mol/L

Use data from Appendix IIB to calculate the equilibrium constants at 25 ∘C for each reaction.

Br2(g)+Cl2(g)⇌2BrCl(g)
ΔG∘f for BrCl(g) is -1.0 kJ/mol

Express your answer using two significant figures.

K= ?

78. Estimate the value of the equilibrium constant at 655 K for each reaction in Problem 74. (AH; for BrCl is 14.6 kJ/mol.) 74. Use data from Appendix IIB to calculate the equilibrium constants at 25 °C for each reaction. AG for BrCl(g) is -1.0 kJ/mol. a. 2 NO2(8) = N204(8) b. Br2(g) + Cl2(8) = 2 BrCl(g)

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