For the reaction CaCO 3 s - CaO s - CO 2 g the partial pressure of CO 2 at equilibrium depends on-A- the mass of CaOB- the mass of CaCO 3C- temperatureD- Both a and b

The correct option is C temperature CaCO3(s) nbsp;⇋ nbsp;CaO (s) + CO2 (g) K_c = [CaO(s)][ CO_2 (g)] /[CaCO_3 (s)] Since concentration of nbsp; CaCO_3(s) ...

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Byju's Answer

Standard XII

Chemistry

Le Chatelier's Principle for Del N Lesser Than Zero

For the react...

Question

For the reaction $C a C O_{3}$ (s) $⇋$ $C a O$ (s) + $C O_{2}$ (g) the partial pressure of $C O_{2}$ (at equilibrium) depends on:

the mass of $C a O$

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the mass of $C a C O_{3}$

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Both a and b

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temperature

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Solution

The correct option is D
temperature

CaCO₃(s) $⇋$ CaO (s) + CO₂ (g)
$K_{c}$ = $\frac{[C a O (s)] [C O_{2} (g)]}{[C a C O_{3} (s)]}$
Since concentration of $C a C O_{3}$ (s) and $C a O (s)$ are constant, therefore modified equilibrium
constant for the thermal decomposition of calcium carbonate will be $K_{c}$ = [ $C O_{2}$ (g)]

or $K_{p}$ = $p_{C O_{2}}$

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Similar questions

For the reaction $C a C O_{3}$ (s) $⇋$ $C a O$ (s) + $C O_{2}$ (g) the partial pressure of $C O_{2}$ (at equilibrium) depends on:

Q. For the reaction

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

the pressure of

C O_{2} (g)

depends on

Q. For the equilibrium :

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

, the pressure of

C O_{2}

is 1 atm at equilibrium in a container of

V

litre, at temperature

T

. Which one is not correct?

The equilibrium constant for the reaction,

CaCO₃(s) ⇌ CaO(s) + CO₂(g), is

Q. What is minimum mass (in g) of

C a C O_{3} (s)

will be required to establish the equilibrium

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

1000 K

in a

4 L

container previously containing

C O_{2}

0.82 a t m

. Equilibrium constant

K_{P}

for the dissociation reaction

1.64 a t m

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For the reaction CaCO3(s) ⇋ CaO(s) + CO2(g) the partial pressure of CO2 (at equilibrium) depends on:

The correct option is D temperature CaCO3(s) ⇋ CaO (s) + CO2 (g) Kc = [CaO(s)][CO2(g)][CaCO3(s)] Since concentration of CaCO3(s) and CaO(s) are constant, therefore modified equilibrium constant for the thermal decomposition of calcium carbonate will be Kc= [CO2(g)] or Kp = pCO2

For the reaction $C a C O_{3}$ (s) $⇋$ $C a O$ (s) + $C O_{2}$ (g) the partial pressure of $C O_{2}$ (at equilibrium) depends on: