CH9_Page_21

# CH9_Page_21 - Since the equilibrium constant is so small we...

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Unformatted text preview: Since the equilibrium constant is so small, we would expect the partial pressure of chlorine to be veryr loinr at equilibrium, so we can neglect it to simplify this expression. 31] [7}31-5 K 2—2 =3.2x1o-3‘ [ﬂ] 2 Pg! ={1.5}[3.2x1o-54}= 4.3x we bar PH“ = 15:]! =1.5 bar 9.?” {a} According to Le Chateiier’s principle, an increase in the partial pressure Ct}2 'will shift the equilibrium to the left, increasing the partial pressure of CH‘. {b} According to Le Chatelier"s principle, a decrease in the partial pressure of CH4 will shift the eqrdlihrium to the left, decreasing the partial pressure of (302. {c} The equilibrium constant for the reaction is unchanged, because it is unaffected by any change in concentration. {d} According to Le |Eitratelier‘s principle, a decrease in the concentration of H10 will shift the equilibrium to the right, increasing the concentration of C02. 936 The questions can all be answered qualitativelyr using Le Chatelier’s principle: - (a) Adding a reactant will promote the formation of products; the amount of HI should increase. {13) I: is solid and already.»' present in excess in the original equilibrium. Adding more solid will not affect the equilibrium so the amount chlz will not change. {-2) Removing a product will shift the reaction toward the formation of more products; the amount of C]: should increase. 27'"? ...
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