Question

sion 2
The equilibrium SO2Cl2(9) = SO2(g) + Cl2(g) is attained at 25°C in a closed container at constant pressure
and an inert gas helium is introduced. Which of the following statements is/are false?
Concentration of SO2, Cl2 and SO2Cl2 are changed
More Cl2 is formed
Concentration of SO2 is reduced
More SO2Cl2 is formed​

Answer 1

Answer:

Based on given options No effect on equilibrium it is correct statement and remaining are false statements.

because addition of any inert gas to the reaction mixture does not affect the reaction in any way. This is because the individual partial pressure of the reactants remain the same.

Answer 2

More $Cl_2$ is formed.

Explanation:

When an inert gas is added to the system in equilibrium at constant pressure, then the total volume will increase. Hence the pressure would decrease according to Boyle's law.  Hence, the equilibrium will shift towards the direction in which there is increase in number of moles of gases to compensate the decrease in pressure.

For the given balanced reaction:

$SO_2Cl_2(g)\rightarrow SO_2(g)+Cl_2(g)$

Thus when inert gas helium is introduced  at constant pressure, the reaction will shift towards the product side as there are more moles on product side. Thus more $Cl_2$ is formed.

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