A reversible reaction is one where the products can react to form the reactants.
If a chemical reaction occurs in a closed container where the reactants and products can't escape it will reach an equilibrium.
At an equilibrium the rate of the forward reaction will equal the rate of the backwards reaction. This means that the concentrations of the products and reactants won't change.
If you remove a product from a reversible reaction the equilibrium will shift to the right. This means more reactants are converted into products. This will also happen if you add more reactants.
Increasing the temperature will move the reaction in the direction of the endothermic reaction. Increasing the pressure will move the equilibrium to the side with the least number of moles of gas molecules.
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