#1. The following reaction has Kp = 50.4 at 448 ºC. $$H_2(g) + I_2(g)\rightleftharpoons 2HI(g)$$ If a 3.00 L flask initially contains 0.0500 moles each of H2 and I2, how many moles of HI are present when the contents have reached equilibrium at 448 °C?
Let 2p be the partial pressure of HI at equilibrium. Using the ideal gas law and the equilibrium constant expression,
50.4 = 4p2/[(0.05RT/V)-p]2
The number of moles of HI present at equilibrium is n = (2p)V/RT = 0.0780.
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