The given reaction is
"H_2(g) +I_2(g) \\rightleftharpoons 2HI(g)"
The change in concentration of reactant or product is govern by Le chatlier's principle
- If hydrogen gas is added to reactant side equilibrium is shift in forward direction and thus purple colour changes to colourless due to formation of more HI.
- If HI is removed from system then reaction will move toward forward and thus it become colourless.
Now consider the second reaction as follows
"CaCO_3 (s)+ Heat \\rightleftharpoons CaO(s)+ CO_2)(g)"
- As the number of mole of gases in product side is more so on increasing the pressure of CO2 it will shift reaction toward backward direction and thus more reactant will form as per Le chatlier's principle.
- As we know that reaction is endothermic reaction so on increasing the temperature equilibrium will shift toward forward direction .
- And on decreasing the temperature equilibrium will shift toward backward direction and thus more reactant will form.
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