Chapter 15, Problem 24c
Consider the following equilibrium: 2 H2(π) + S2(βπ) β 2 H2S(π) πΎπ = 1.08Γ107 at 700Β°C (c) Calculate the value of πΎπ if you rewrote the equation H2(π) + 1/2 S2(βπ) β H2S(π)
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Which of the following reactions lies to the right, favoring the formation of products, and which lies to the left, favoring the formation of reactants? (b) 2 HBr(π) β H2(π) + Br2(π) πΎπ = 5.8Γ10β18
Which of the following statements are true and which are false? (c) As the value of the equilibrium constant increases, the speed at which a reaction reaches equilibrium must increase.
If πΎπ = 0.042 for PCl3(π) + Cl2(π) β PCl5(π) at 500 K, what is the value of πΎπ for this reaction at this temperature?
At 1000 K, πΎπ = 1.85 for the reaction SO2(π) + 12 O2(π) β SO3(π) (c) What is the value of πΎπ for the reaction in part (b)?
Consider the following equilibrium, for which at πΎπ = 0.0752 at 480Β°C: 2 Cl2(π) + 2 H2O(π) β 4 HCl(π) + O2(π) (a) What is the value of πΎπ for the reaction 4 HCl(π) + O2(π) β 2 Cl2(π) + 2 H2O(π)?
The following equilibria were attained at 823 K:
CoO(s) + H2(g) β Co(s) + H2O(g) Kc = 67
CoO(s) + CO(g) β Co(s) + CO2(g) Kc = 490
Based on these equilibria, calculate the value of πΎπ for H2(π)ββ+ CO2(π) β CO(π) + H2O(π) at 823 K.