Sulfur trioxide decomposes at high temperature in a sealed

Chapter 10, Problem 9PE

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Calculating K from Initial and Equilibrium Concentrations

A closed system initially containing \(1.000 \times \mathrm{MH}_{2}\) and \(2.000 \times M I_{2}\) at \(448^{\circ} \mathrm{C}\) is allowed to reach equilibrium, and at equilibrium the HI concentration is \(1.87 \times 10^{-3} \mathrm{M}\). Calculate \(K_{c}\) at \(448^{\circ} \mathrm{C}\) for the reaction taking place, which is

\(\mathrm{H}_{2}(g)+I_{2}(g) \rightleftharpoons 2 H I(g)\)

Sulfur trioxide decomposes at high temperature in a sealed container: \(2 \mathrm{SO}_{3}(g) \rightleftharpoons 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g)\). Initially, the vessel is charged at 1000 K with \(\mathrm{SO}_{3}(\mathrm{~g})\) at a partial pressure of 0.500 atm. At equilibrium the \(\mathrm{SO}_{3}\) partial pressure is 0.200 atm. Calculate the value of \(K_{p}\) at 1000 K.

Equation Transcription:

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Text Transcription:

1.000 x MH_2

2.000 x MI_2

K_c

448 degree C

1.87 x 10^3 M

H_2(g) + I_2(g) right left harpoons 2HI(g)

SO_3(g)

SO_3

K_p