Consider the following reaction at equilibrium
pcl3 (g) + cl2 (g) ↔ pcl5 (g) ∆h = –86 kj/mol
what type of reaction is this?

me!

how will the equilibrium be affected by adding more of the product?

is the reaction endothermic or exothermic? how will the equilibrium be affected by adding heat?

how will the equilibrium be affected by increasing the pressure on the closed system?

explain the principle that you used in determining how the equilibrium is affected.

1. Equilibrium shifts to (lift side) produce more reactant.

2. Exothermic reaction, Equilibrium shifts to (lift side) produce more reactant.

3. Increasing the pressure will shift the reaction to the side with lower moles of gas (right side).

4. Le Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.

Explanation:

Le Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.

1. How will the equilibrium be affected by adding more of the product?

When more product is added:

This will increase the concentration of the products side, so the reaction will be shifted to the lift side (reactants side) to suppress the increase in the concentration of Products.

So, the right choice is: Equilibrium shifts to produce more reactant.

2. Is the reaction endothermic or exothermic? How will the equilibrium be affected by adding heat?

Since the sign of ΔH is negative, the reaction is exothermic reaction.

The reaction can be represented as:

PCl₃ (g) + Cl₂ (g) ↔ PCl₅ (g) + heat.

Adding heat:

Adding heat is like adding more product to the reaction, so the reaction will be shifted to the lift side (reactants side) to suppress the effect of adding heat.

So, the right choice is: Equilibrium shifts to the lift side (produce more reactant).

3. How will the equilibrium be affected by increasing the pressure on the closed system?

Increasing the pressure:

When there is an increase in pressure, the equilibrium will shift towards the side with fewer moles of gas of the reaction. And when there is a decrease in pressure, the equilibrium will shift towards the side with more moles of gas of the reaction.

The reactants side (left) has 2.0 moles of gases and the products side (right) has 1.0 mole of gases.

So, increasing the pressure will shift the reaction to the side with lower moles of gas (right side).

4. Explain the principle that you used in determining how the equilibrium is affected.  

Le Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.

Spontaneity tell us the direction of the reaction, but not how fast it goes. gibbs free energy brings together enthalpy, entropy and temperature in one easy formula. g = h - ts. and, finally the sign of delta g is always negative for a spontaneous reaction.

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