Learning the Mechanisms : Investigating the Breakdown of Ammonia and Reaction Rates

The video tutorial explains the decomposition of ammonia into nitrogen and hydrogen, highlighting that the rate of hydrogen formation is three times that of nitrogen. It details how to compute the rate of nitrogen formation using ammonia decomposition and equates rate expressions for decomposition reactions. Finally, it defines the rate of reaction for general reactions, emphasizing the role of stoichiometric coefficients.

What is the relationship between the rate of formation of hydrogen and nitrogen in the decomposition of ammonia?

• The rate of formation of hydrogen is twice the rate of formation of nitrogen.

• The rate of formation of hydrogen is half the rate of formation of nitrogen.

• The rate of formation of hydrogen is equal to the rate of formation of nitrogen.

• The rate of formation of hydrogen is thrice the rate of formation of nitrogen.

How is the rate of formation of nitrogen expressed in terms of ammonia decomposition?

• As minus delta NH3 by delta T.

• As delta NH3 by delta T.

• As minus half delta NH3 by delta T.

• As half delta NH3 by delta T.

What is the purpose of equating rate expressions in a decomposition reaction?

• To relate the rates of formation of different products.

• To compare the rates of different reactions.

• To determine the activation energy.

• To find the equilibrium constant.

In a balanced chemical reaction, how is the rate of reaction defined?

• As the rate of change of concentration of any reactant or product divided by a stoichiometric coefficient.

• As the rate of change of concentration of any reactant or product.

• As the rate of change of concentration of any reactant or product multiplied by a stoichiometric coefficient.

• As the rate of change of concentration of any reactant or product without considering stoichiometric coefficients.

What role do stoichiometric coefficients play in determining the rate of reaction?

• They are used to calculate the equilibrium constant.

• They are used to balance the chemical equation.

• They are used to multiply the rate of change of concentration in the rate of reaction.

• They are used to divide the rate of change of concentration in the rate of reaction.