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Le Chatelier's Principle for Del N Equals to 0

2CaSO4s⇌ 2CaO...

Question

$2 C a S O_{4} (s) ⇌ 2 C a O (s) + 2 S O_{2} (g) + O_{2} (g), Δ H > 0$
If the above shown equilibrium is established by taking sufficient amount of $C a S O_{4} (s)$ in a closed container at 1600K, then which of the following is(are) correct? (Assume that solid $C a S O_{4}$ is present in the container in each case)

Moles of

C a O (s)

will increase with the increase in temperature

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If the volume of the container is doubled at equilibrium, then partial pressure of

S O_{2} (g)

will change at new equilibrium

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If the volume of the container is halved, then partial pressure of

O_{2} (g)

at new equilibrium will remain same

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If two moles of

H e

gas is added at constant pressure, then the moles of

C a O (s)

will increase

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Solution

The correct options are
A Moles of $C a O (s)$ will increase with the increase in temperature
C If two moles of $H e$ gas is added at constant pressure, then the moles of $C a O (s)$ will increase
D If the volume of the container is halved, then partial pressure of $O_{2} (g)$ at new equilibrium will remain same
A) As the reaction is endothermic, therefore it will go in the forward direction as the temperature increases. Hence, the moles of CaO will increase.
(C) With an increase or decrease in volume, the particle pressure of the gases will remain the same at equilibrium at a particular temperature.
(D) Due to the addition of inert gas at constant pressure, the reaction will proceed in the direction where more number of gaseous molecules are formed.

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Similar questions

$2 C a S O_{4} (s) ⇌ 2 C a O (s) + 2 S O_{2} (g) + O 2 (g), Δ H > 0$

Above equilibrium is established by taking sufficient amount of $C a S O_{4} (s)$ in a closed container at 1600 K. Then, which of the following may be correct options?
(Assume that solid $C a S O_{4}$ is present in the container in each case).

2 C a S O_{4} (s) ⇌ 2 C a O (s) + 2 S O_{2} (g) + O_{2} (g), Δ H > 0

Above equilibrium is established by taking a sufficient amount of

C a S O_{4}

(s) in a closed container at 1600 K. Then which of the following may be the correct option(s)?

(Assume that solid

C a S O_{4}

is present in the container in each case)

2 C a S O_{4} (s) ⇌ 2 C a O (s) + 2 S O_{2} (g) + O_{2} (g), Δ H > 0

Above equilibrium is established by taking sufficient amount of CaSO

_{4}

(s) in a closed container at 1600 K. Then which of the following may be correct option(s)?(Assume that solid CaSO

_{4}

is represent in the container in each case)

Q. If

K_{P}

of an equilibrium

C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g)

is 1.5 atm at

20^{o} C

then the moles of CaO formed if excess

C a C O_{3} (s)

is being placed in a 1 lt of closed container containing

C O_{2}

gas at 0.5 atm pressure at same temperature is:

Q. If

K_{p}

of an equilibrium

C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g)

is 1.5 atm at

29^{0} C

then the moles of CaO formed if excess

C a C O_{2} (S)

is being placesd in a 1 L of closed container containing

C O_{2}

gas at 0.5 atm pressure at same temperature is:

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2CaSO4(s)⇌2CaO(s)+2SO2(g)+O2(g),ΔH>0If the above shown equilibrium is established by taking sufficient amount of CaSO4(s) in a closed container at 1600K, then which of the following is(are) correct? (Assume that solid CaSO4 is present in the container in each case)