Chemical Reaction Equilibrium Concepts

The video tutorial explains the concept of equilibrium in chemical reactions. It covers the forward and backward reactions, defining equilibrium as the point where the rate of the forward reaction equals the rate of the backward reaction. The tutorial also discusses how concentrations of reactants and products change until equilibrium is reached, at which point they remain constant.

What is the term used for the reaction where reactants transform into products?

• Backward reaction

• Forward reaction

• Static reaction

• Equilibrium reaction

In a chemical reaction, what does the forward direction refer to?

• Products converting back to reactants

• Reactants converting into products

• No change in reactants or products

• Reactants and products in equal concentration

At the start of a reaction, what is the initial condition regarding the rates of forward and backward reactions?

• Rates are equal

• Rate of forward reaction is zero

• Rate of backward reaction is zero

• Rates are not equal

What happens to the rates of forward and backward reactions at equilibrium?

• Rate of forward reaction becomes zero

• Rates continue to change

• Rate of backward reaction becomes zero

• Rates become equal

What is the state of reactant and product concentrations at equilibrium?

• They become infinite

• They become zero

• They remain constant

• They continue to change

Which statement is true about the equilibrium condition in a chemical reaction?

• Only reactants are present

• Only products are present

• Concentrations fluctuate continuously

• No further change in concentrations