Equilibrium Constants and Concentrations

This video tutorial explains how to calculate equilibrium concentrations of reactants and products using the equilibrium constant (Kc). It includes two examples: one involving dinitrogen tetroxide and nitrogen dioxide, and another with ethanoic acid and ethanol. The video provides step-by-step calculations and emphasizes understanding the molar ratios and equilibrium expressions. It concludes with a call to action for further learning resources.

What is the main focus of this video tutorial?

• Calculating equilibrium concentrations of reactants and products

• Balancing chemical equations

• Studying reaction kinetics

• Understanding chemical bonding

In the first example, what is the chemical formula for dinitrogen tetroxide?

• O2N2

• N2O4

• N2O

• NO2

What is the equilibrium constant (Kc) value used in the first example?

• 3.23 x 10^-1

• 2.00 x 10^-2

• 1.06 x 10^-5

• 1.85 x 10^-3

In the second example, what does 'equimolar' mean?

• Different number of moles of reactants

• Equal mass of reactants

• Same number of moles of reactants

• Equal volume of reactants

What is the equilibrium concentration of ethanoic acid in the second example?

• 0.820 mol/dm³

• 1.64 mol/dm³

• 0.500 mol/dm³

• 2.00 mol/dm³

What is the relationship between ethanoic acid and ethanol in the reaction?

• They react in a 3:1 ratio

• They react in a 2:1 ratio

• They react in a 1:1 ratio

• They do not react

How is the concentration of the ester related to the concentration of water in the second example?

• They are unrelated

• They are equal

• Ester concentration is double

• Water concentration is double

What is the calculated concentration of the ester in the second example?

• 0.500 mol/dm³

• 0.820 mol/dm³

• 1.64 mol/dm³

• 2.00 mol/dm³

Why is the concentration of products greater than reactants in the second example?

• The equilibrium constant is less than one

• The reaction is not at equilibrium

• The reactants are in excess

• The equilibrium constant is greater than one

What is the significance of the equilibrium constant being greater than one?

• Products are favored

• The reaction is fast

• The reaction is slow

• Reactants are favored