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Le Chatelier's Principle for Del N Greater Than Zero

1 mole Ca C...

Question

1 mole $C a {C O}_{3 (s)}$ is heated in 11.2 lit vessel so that equilibrium is established at 819 K. If $K_{p}$ for $C a {C O}_{3} ⇌ C a O + {C O}_{2}$ at this temperature is 2 atm, equilibrium concentration of ${C O}_{2}$ in liter $^{- 1}$ ?

1/3

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1/11.2

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1/33.6

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1/22.4

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Solution

The correct option is C 1/33.6
$C a C O_{3} (s)_{↽}^{⇀} C a O (s) + C O$ _2$ (g)
$Δ_{n g}$ =1
$K_{p} = K_{c} (R T)^{Δ_{n g}}$
$K_{c} = \frac{K_{p}}{R T}$ = $\frac{2}{0.0821 \times 81 g} = 0.029$
Now, $K_{c} = [C O_{2}]$
$[C O_{2}] = 0.029 =$ $\frac{1}{33.6}$ mol lit $^{- 1}$
Therefore , the equilibrium concentration of $C O_{2}$ is $\frac{1}{33.6}$ mol lit $^{- 1}$

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Similar questions

Q. 1 mole

C a C O_{3 (s)}

is heated in

11.2

lit vessel so that equilibrium is establihed at

819 K

. If

K_{p}

for

C O C O_{3} ⇌ C a O + C O_{2}

at this temperature is 2 atm, equilibrium concentration of

C O_{2}

(in mol-lit

^{- 1}

)

Q. For the reaction:

C a C O_{3}

(s)

⇌

CaO(s) +

C O_{2}

(g).

K_{p}

= 1 atm at

927^{0}

C. If 20g of

C a C O_{3}

were kept in a 10 liter vessel at

927^{0}

C, then calculate percentage of

C a C O_{3}

remaining at equilibrium:

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:

The equilibrium constant for the reaction,

CaCO₃(s) ⇌ CaO(s) + CO₂(g), is

Q. The process

C a {C O}_{3} ⇌ C a O + {C O}_{2}

attains equilirbium in

11.2

lit vessel at

1092 K

and

2

atm. Now, initial number of moles of

C A {C O}_{3}

cannot be?

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1 mole CaCO3(s) is heated in 11.2 lit vessel so that equilibrium is established at 819 K. If Kp for CaCO3⇌CaO+CO2 at this temperature is 2 atm, equilibrium concentration of CO2 in liter−1?

The correct option is C 1/33.6CaCO3(s)⇀↽CaO(s)+CO_2$ (g)Δng =1Kp=Kc(RT)ΔngKc=KpRT=20.0821×81g=0.029Now, Kc=[CO2][CO2]=0.029= 133.6 mol lit−1Therefore , the equilibrium concentration of CO2 is 133.6 mol lit−1

1 mole $C a {C O}_{3 (s)}$ is heated in 11.2 lit vessel so that equilibrium is established at 819 K. If $K_{p}$ for $C a {C O}_{3} ⇌ C a O + {C O}_{2}$ at this temperature is 2 atm, equilibrium concentration of ${C O}_{2}$ in liter $^{- 1}$ ?