# What causes a reaction to form more products?

## What causes a reaction to form more products?

Changes in Concentration According to Le Chatelier’s principle, adding additional reactant to a system will shift the equilibrium to the right, towards the side of the products. If we add additional product to a system, the equilibrium will shift to the left, in order to produce more reactants.

### What kind of reaction is 2SO2 G O2 G → 2SO3 G?

Answer : It is a combination reaction.

#### What happens to the equilibrium 2SO2 G O2 G ⇋ 2SO3 G if the volume of the system is increased )))?

What happens to the equilibrium 2SO2(g)+O2(g)⇋2SO3(g) if the volume of the system is increased? What happens to the equilibrium if the volume of the system is increased? It will shift to the right.

What would be the effect on equilibrium if more SO2 is added?

What will happen to the equilibrium when more 2SO2 (g) is added to the following system? Solution: Adding more reactants shifts the equilibrium in the direction of the products; therefore, the equilibrium shifts to the right.

What increases yield in a reaction?

Le Châtelier’s Principle states that a change in pressure, temperature, or concentration will push the equilibrium to one side of the chemical equation. So, if you manipulate the conditions to favour the product side, you increase the yield.

## What is the value of Kc for the reaction 2SO2 g )+ O2 G ← − → 2SO3 G?

The equilibrium constant Kc for the reaction: 2SO2 (g) + O2 (g) → 2SO3 (g) is 800 at 527oC.

### What would happen to the position of the equilibrium if oxygen is added to the system 2SO3 G ⇌ 2SO2 G O2 G?

2SO3(g) ↔ 2SO2(g) + O2(g) (a) Sulfur dioxide is added to the system. Equilibrium will shift to favor reactants.

#### What is the expression for the equilibrium constant for the reaction described by the following equation 2SO2 g O2 )( G → 2SO3 G?

The equilibrium constant for the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) is Kc = 1.7 × 106.