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Sagot :
Answer:
Each of the following reactions was in equilibrium when the pressure of their containers was doubled. Chose which way the reaction shifted after the pressure change:
2NH3 (g)->N2(g) +3H2(g)
2Na3 PO4 (aq) + 3CaCl2 (aq) -> Ca3 (PO4 )2 (s) + 6NaCl(aq)
2CO(g)+O2 (g)->2CO2 (g)
2HI(g) -> H2(g) + I2(g)
Explanation:
Effect of pressure on equilibrium:
When pressure is increased on an equilibrium system,then equilibrium will shift in such a direction towards less number of moles of substrates.
For the first system,
2NH3 (g)->N2(g) +3H2(g)
increase in pressure,shifts the equilibrium towards the left side that is the formation of ammonia is favored.
For the second reaction:
2Na3 PO4 (aq) + 3CaCl2 (aq) -> Ca3 (PO4 )2 (s) + 6NaCl(aq)
The quilibrium will shift towards right.
Becuase right side less number of moles of substrates are there.
2CO(g)+O2 (g)->2CO2 (g)
For this system,the equilibrium will shift towards right side that is formation of CO2 gas is favored.
For the last system,
2HI(g) -> H2(g) + I2(g)
there is no effect of pressure.
Becuase the number of moles of substrates are same on both sides.
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