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At a particular temperature, K = 1.00×102 for the reaction:
H2(g) + F2(g) 2HF(g)
In an experiment, at this temperature, 1.10 mol of H2 and 1.10 mol of F2 are introduced into a 1.08-L flask and allowed to react. At equilibrium, all species remain in the gas phase.
What is the equilibrium concentration (in mol/L) of H2?
What is the equilibrium concentration (in mol/L) of HF?
To the mixture above, an additional 3.63×10-1 mol of H2 is added.
What is the new equilbrium concentration (in mol/L) of HF?
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What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps? What would be the total work if the process were carried out reversibly?
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