Consider the equilibrium below:
AgCl(s) Ag1+(aq) + Cl1-(aq) | Ho = 66 kJ |
Use LeChatelier's principle to predict the effect on the chloride ion concentration caused by each of the following actions:
Action | Effect on [Cl1-] |
---|---|
adding silver chloride | ---Select--- increases unchanged decreases |
adding silver ion | ---Select--- increases unchanged decreases |
adding water | ---Select--- increases unchanged decreases |
heating | ---Select--- increases unchanged decreases |
AgCl(s) <=> Ag+(aq) + Cl-(aq)
Adding silver chloride , No change
Adding silver ion , decrease
Adding water, molarity decreases so increment in chloride ion
Heating increases because reaction is endothermic
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Consider the equilibrium below: AgCl(s) Ag1+(aq) + Cl1-(aq) Ho = 66 kJ Use LeChatelier's principle to...
Consider the following equilibrium: AgCl(s) Ag1+(aq) + Cl1-(aq) Ho = 66 kJ Use LeChatelier's principle to predict the effect on the chloride ion concentration caused by each of the following actions: Action Effect on [Cl1-] adding silver chloride ---Select--- increases unchanged decreases adding silver ion ---Select--- increases unchanged decreases adding water ---Select--- increases unchanged decreases heating ---Select--- increases unchanged decreases
Consider the equilibrium below: A + B C + D + E Ho < 0 Use LeChatelier's principle to predict the effect on the concentration of the equilibrium concentration of E caused by each of the following actions: action result on [E] adding C ---Select--- increases remains unchanged decreases removing D ---Select--- increases remains unchanged decreases increasing the temperature ---Select--- increases remains unchanged decreases
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