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Which of the ...

Question

Which of the following reactions will get affected by increase in pressure? Also mention whether the change will cause the reaction to go to the right or left direction.
$C H_{4} (g) + 2 S_{2} (g) ⇌ C S_{2} (g) + 2 H_{2} S (g)$
$C O_{2} (g) + C (s) ⇌ 2 C O (g)$
$4 N H_{3} (g) + 5 O_{2} (g) ⇌ 4 N O (g) + 6 H_{2} O (g)$
$C_{2} H_{4} (g) + H_{2} (g) ⇌ C_{2} H_{6} (g)$
$C O C l_{2} (g) ⇌ C O (g) + C l_{2} (g)$
$C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g)$

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Solution

According to Le-Chatlier's principle,
When pressure increases, equilibrium shifts in the direction where pressure decreases
i) $C H_{4 (g)} + 2 S_{2 (g)} ⇌ C S_{2 (g)} + 2 H_{2} S_{(g)} n_{p} = n_{r}$
No effect
ii) $C O_{2 (g)} + C_{(s)} ⇌ 2 C O_{(g)}, n_{p} > n_{r}$
Backward reaction is favored
iii) $4 N H_{3 (g)} + 5 O_{2 (g)} ⇌ 4 N O_{(g)} + 6 H_{2} O_{(g)} n_{r} > n_{p}$
Backward reaction is favored
iv) $C_{2} H_{4 (g)} + H_{2 (g)} ⇌ C_{2} H_{6 (g)} n_{p} > n_{r}$
Forward reaction is favored
v) $C O {C l}_{2 (g)} ⇌ C O_{(g)} + {C l}_{2 (g)}, n_{p} > n_{r}$
Shifts to backward direction
vi) $C a C O_{3 (s)} ⇌ C a O_{(s)} + C O_{2 (g)}, n_{p} > n_{r}$
Backward reaction is favored

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Q. Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
(i)

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

{C H}_{4} (g) + 2 S_{2} (g) ⇌ {C S}_{2} (g) + 2 H_{2} S (g)

{C O}_{2} (g) + C (s) ⇌ 2 C O (g)

2 H_{2} (g) + C O (g) ⇌ {C H}_{3} O H (g)

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

4 {N H}_{3} (g) + 5 O_{2} (g) ⇌ 4 N O (g) + 6 H_{2} O (g)

Which of the following reactions will get affected by increasing the pressure?

Also, mention whether change will cause the reaction to go into forward or backward direction.

(i)

(ii)

(iii)

(iv)

(v)

(vi)

Which of the following reactions will get affected by increasing the pressure?
Also, mention whether change will cause the reaction to go into forward or backward direction.
(i) $C O C l_{2} (g) \leftrightarrow C O (g) + C l_{2} (g)$
(ii) $C H_{4} (g) + 2 S_{2} (g) \leftrightarrow C S_{2} (g) + 2 H_{2} S (g)$
(iii) $C O_{2} (g) + C (s) \leftrightarrow 2 C O (g)$
(iv) $2 H_{2} (g) + C O (g) \leftrightarrow C H_{3} O H (g)$
(v) $C a C O_{3} (s) \leftrightarrow C a O (s) + C O_{2} (g)$
(vi) $4 N H_{3} (g) + 5 O_{2} (g) \leftrightarrow 4 N O (g) + 6 H_{2} O (g)$

Which of the following reactions will get affected by increasing the pressure?

Also, mention whether change will cause the reaction to go into forward or backward direction.

(i)

(ii)

(iii)

(iv)

(v)

(vi)

2 C O (g) ⇌ C (s) + C O_{2} (g); K_{p_{1}} = 10^{- 14} a t m^{- 1}

1120 K

C O (g) + C l_{2} (g) ⇌ C O C l_{2} (g); K_{p_{2}} = 6 \times 10^{- 3} a t m^{- 1}

K_{c}

for the following reaction at

1120 K

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

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