Please help me! I am stuck. Consider the following reaction at equilibrium PCl3 (g) + Cl2 (g) PCl5 (g) H = -86 kJ/mol What type of reaction is this?

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Please help me! I am stuck.

Consider the following reaction at equilibrium

PCl3 (g) + Cl2 (g) ↔ PCl5 (g)   ∆H = -86 kJ/mol

What type of reaction is this?

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. 

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