Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction the reaction to go into forward of backward direction.
a. `COCl_(2)(g) hArr CO(g)+Cl_(2)(g)`
b. `CH_(4)(g)+2S_(2)(g) hArr CS_(2)(g)+2H_(2)S(g)`
c. `CO_(2)(g)+C(s) hArr 2CO(g)`
d. `2H_(2)(g)+CO(g) hArr CH_(3)OH(g)`
e. `CaCO_(3)(s) hArr CaO(s)+CO_(2)(g)`
f. `4NH_(3)(g)+5O_(2)(g) hArr 4NO(g)+6H_(2)O(g)`

Explanation

To determine how increasing pressure affects the given reactions, we will apply Le Chatelier's Principle, which states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change. In the case of pressure changes, the equilibrium will shift towards the side with fewer moles of gas.

Let's analyze each reaction step by step:

### Step 1: Analyze Reaction a
**Reaction:** `COCl_(2)(g) ⇌ CO(g) + Cl_(2)(g)`

- **Moles of gas on reactants side:** 1 (from COCl₂)
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