Lechatliers principle and pressure effect

The video tutorial explains the formation of methane from carbon monoxide and hydrogen through catalytic methanation. It details the chemical reaction involving 4 moles of reactants forming 2 moles of products. The impact of pressure on the concentration of reactants and products is discussed, highlighting the greater number of collisions on the reactant side. The video compares QC and KC values, explaining how pressure changes lead to partial reactions and affect the number of gaseous products. It concludes with the incompressibility of solids and liquids in equilibrium mixtures.

What are the reactants involved in the formation of methane in the described reaction?

• Hydrogen and oxygen

• Carbon monoxide and hydrogen

• Methane and water

• Carbon monoxide and oxygen

How many moles of gaseous products are formed in the reaction?

• 3 moles

• 1 mole

• 4 moles

• 2 moles

What happens to the concentration of reactants and products when pressure is increased?

• Concentration of products decreases

• Concentration of reactants decreases

• Concentration remains unchanged

• Concentration of both reactants and products increases

Why are there more collisions between reactant molecules compared to product molecules?

• Products are more reactive

• Reactants have fewer moles

• Reactants have more moles

• Products have more moles

What is the effect of pressure on solids and liquids in an equilibrium mixture?

• Pressure increases their concentration

• Pressure causes them to react

• Pressure decreases their concentration

• Pressure has no effect