The equilibrium constants for the following reactions at 1400 K are given- 2 H 2 Og- 2 H 2 g- O 2 g- K 1 -2-1- 10 -13 2 CO 2 g- 2COg- O 2 g- K 2 -1-4- 10 -12Then- the equilibrium constant K for the reaction- H 2 g-C O 2 g- COg- H 2 Og- is-

The correct option is C 2.6 (I) #160; #160; 2 H _ 2 O( g ) ⇌ 2 H _ 2 ( g ) + O _ 2 ( g ) ∴ K _ 1 =( p _ H _ 2 ) #160; ^ 2 . p _ O _ 2 ( ...

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Characteristics of Equilibrium Constant

The equilibri...

Question

The equilibrium constants for the following reactions at $1400 K$ are given:

$2 H_{2} O (g) ⇌ 2 H_{2} (g) + O_{2} (g); K_{1} = 2.1 \times 10^{- 13}$
$2 {C O}_{2} (g) ⇌ 2 C O (g) + O_{2} (g); K_{2} = 1.4 \times 10^{- 12}$

Then, the equilibrium constant $K$ for the reaction, $H_{2} (g) + C O_{2} (g) ⇌ C O (g) + H_{2} O (g)$ , is:

2.04

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20.5

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2.6

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6.67

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Solution

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H_{2 (g)} + C O_{2 (g)} ⇌ H_{2} O_{(g)} + C O_{(g)}

1395 K

1395 K

2 H_{2} O_{(g)} ⇌ 2 H_{2} + O_{2 (g)}; K_{1} = 2.1 \times 10^{- 13}

2 C O_{2 (g)} ⇌ 2 C O_{(g)} + O_{2 (g)}; K_{2} = 1.4 \times 10^{- 12}

2 H_{2} O (g) ⇋ 2 H_{2} (g) + O_{2} (g); K_{1} = 6.4 \times 10^{- 8}

2 C O_{2} (g) ⇋ 2 C O (g) + O_{2} (g); K_{2} = 1.6 \times 10^{- 6}

H_{2} (g) + C O_{2} (g) ⇋ C O (g) + H_{2} O (g)

H_{2} (g) + {C O}_{2} (g) ⇌ H_{2} O (g) + C O

2 H_{2} O (g) ⇌ 2 H_{2} (g) + O_{2} (g) K_{1} = 2.1 \times 10^{- 13}

2 {C O}_{2} (g) ⇌ 2 C O (g) + O_{2} (g) K_{2} = 1.4 \times 10^{- 12}

K_{1}

K_{2}

C O C l_{2} (g) ⇌ C O (g) + C l_{2} (g)

K_{1} = 0.329

2 C O (g) + O_{2} (g) ⇌ 2 C O_{2} (g)

K_{2} = 2.24 \times 10^{22}

2 C O C l_{2} (g) + O_{2} (g) ⇌ 2 C O_{2} (g) + 2 C l_{2} (g)

K_{3}

823

C o O (s) + H_{2} (g) ⇌ C o (s) + H_{2} O (g); K = 67

C o O (s) + C O (g) ⇌ C o (s) + {C O}_{2} (g); K = 490

2 {C O}_{2} (g) + 2 H_{2} (g) ⇌ 2 C O (g) + 2 H_{2} O (g)

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