When 20 g of CaCO3 were put in a 10 litre flask and heated to 800- C - 35- of CaCO3 remained unreacted at equilibrium- KP for decomposition of CaCO3 will be

The correct option is D 1.145 atm The equilibrium reaction is CaCO_3(s) ⇔ CaO(s) + CO_2(g) .The following table lists the quantities of various speci ...

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Byju's Answer

Standard XII

Chemistry

Derivation of Kp and Kc

When 20 g o...

Question

When $20 g$ of $C a C O_{3}$ were put in a $10 l i t r e$ flask and heated to $800^{\circ} C$ , $35 %$ of $C a C O_{3}$ remained unreacted at equilibrium.
$K_{P}$ for decomposition of $C a C O_{3}$ will be

1.145 a t m

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0.145 a t m

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2.146 a t m

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3.145 a t m

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Solution

The correct option is D $1.145 a t m$
The equilibrium reaction is $C a C O_{3} (s) \Leftrightarrow C a O (s) + C O_{2} (g)$ .
The following table lists the quantities of various species.

$C a C O_{3}$
$C a O$
$C O_{2}$
Initial mass (g)
$20$
$0$
$0$
Initial moles
$0.2$
$0$
$0$
Moles at equilibrium
$0.35 \times 0.2$
$0.13$
$0.13$
The ideal gas equation is $P V = n R T$ .
The partial pressure of $C O_{2} = P = \frac{n R T}{V} = \frac{0.13 \times 0.0821 \times 1073}{10} = 1.145$ atm.
The expression for the equilibrium constant $(K_{P})$ $= P_{C O_{2}} = 1.145$ atm.

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	$C a C O_{3}$	$C a O$	$C O_{2}$
Initial mass (g)	$20$	$0$	$0$
Initial moles	$0.2$	$0$	$0$
Moles at equilibrium	$0.35 \times 0.2$	$0.13$	$0.13$

When 20 g of CaCO3 were put in a 10 litre flask and heated to 800∘C , 35% of CaCO3 remained unreacted at equilibrium. KP for decomposition of CaCO3 will be

When $20 g$ of $C a C O_{3}$ were put in a $10 l i t r e$ flask and heated to $800^{\circ} C$ , $35 %$ of $C a C O_{3}$ remained unreacted at equilibrium.
$K_{P}$ for decomposition of $C a C O_{3}$ will be