In: Chemistry
On the basis of LeChâtelier’s Principle, explain why Ag2CO3 dissolves when HNO3 is added.
Ag2CO3(s) + 2 HNO3(aq) <----> 2 AgNO3(aq) + H2O(l) +
CO2(g)
In a sealed container, the reaction will proceed when HNO3 is added
to Ag2CO3 until equilibrium is reached. We will then have a
balanced equilibium, which is dynamic [still proceeding so rate
forward = rare backward] and concentrations of each chemical remain
constant. CO2 will be present here at a certain concentration and
pressure for example.
However, if you carry out the reaction in a beaker or test tube, it
is no longer a closed system and we can apply LeChatelier's
Principle. He said 'when a constraint is applied to a system in
equilbrium, the system will oppose that constraint'
So in the test tube, the CO2 starts escaping and the concentration
and pressure of CO2 drops. What does the system do?.. well by Le
chatelier it opposes this and tries to up the concentration and
pressure of CO2 by producing more. You've let it escape the system
says, so I'll make more. So more Ag2CO3 and HNO3 react. Once again
the CO2 escapes the tube and more is produced to counteract this.
This continues until one of the reactants is all used up and the
reaction has in fact gone from left to right rather than remaining
in equilibrium.
References:
https://in.answers.yahoo.com/question/index?qid=20100130210953AAVkV4Z