Estimate the value of the equilibrium constant at 640 K for each of the following reactions....

Estimate the value of the equilibrium constant at 640 K for each of the following reactions. ΔH∘f and S∘ for BrCl(g) is 14.6 kJ/mol and 240.0 Jmol⋅K, respectively. for the following

1. 2NO2(g)⇌N2O4(g)

2.Br2(g)+Cl2(g)⇌2BrCl(g)

Expert Solution

queen_honey_blossom answered 2 years ago

Estimate the value of the equilibrium constant at 505 K for each of the following reactions....

Estimate the value of the equilibrium constant at 505 K for each of the following reactions. 2CO(g)+O2(g)⇌2CO2(g) 2H2S(g)⇌2H2(g)+S2(g)

Estimate the value of the equilibrium constant at 675 K for each of the following reactions....

Estimate the value of the equilibrium constant at 675 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K. 3 significant figures in answer. A. 2NO2(g)⇌N2O4(g) ΔH∘f for N2O4(g) is 9.16 kJ/mol. B. Br2(g)+Cl2(g)⇌2BrCl(g) ΔH∘f for BrCl(g) is 14.6 kJ/mol.

Q.26 Estimate the value of the equilibrium constant at 620 K for each of the following...

Q.26 Estimate the value of the equilibrium constant at 620 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K. Part A 2NO2(g)⇌N2O4(g). ΔH∘f for N2O4(g) is 9.16 kJ/mol. Express your answer using three significant figures. K = Part B Br2(g)+Cl2(g)⇌2BrCl(g) .ΔH∘f for BrCl(g) is 14.6 kJ/mol. Express your answer using three significant figures. K =

Use the standard reduction potentials to calculate the equilibrium constant for each of the following reactions:...

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At 850.0 K, the value of the equilibrium constant Kp for the hydrazine synthesis reaction below...

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At 850. K, the value of the equilibrium constant Kp for the hydrazine synthesis reaction below...

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Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25...

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Each of the following reactions is allowed to come to equilibrium and then the volume is...

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The equilibrium constant, K, for the reaction shown below has a value 1.8 x 105. In...

The equilibrium constant, K, for the reaction shown below has a value 1.8 x 105. In this reaction which is the strongest acid and which is the strongest base? CH3CO2H(aq) + H2O (l) --->H3O+(aq) + CH3CO2-(aq) please explain why?

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