Revealing the Dynamics : The Effect of Pressure and Concentration on Reaction Rates

The video tutorial explains how the rate of chemical reactions is influenced by various factors such as the nature of reactants, concentration, temperature, catalysts, and surface area. It highlights the difference in reaction rates between ionic and phase-different reactants, using examples like sodium chloride and silver nitrate. The tutorial also discusses how higher concentrations and pressures increase reaction rates by enhancing collision frequency, illustrated through experiments with zinc chloride and ammonia formation.

Why do ionic compounds generally react faster than reactions involving different phases?

• They have more atoms.

• They are always in the same phase.

• They require less energy.

• They involve rapid electron exchange.

What is the main reason for the slow reaction rate in the formation of ammonia from nitrogen and hydrogen?

• The low concentration of reactants.

• The presence of a catalyst.

• The breaking of triple bonds in nitrogen.

• The high temperature required.

How does the concentration of reactants affect the rate of a chemical reaction?

• Higher concentration changes the product.

• Higher concentration increases the rate.

• Higher concentration has no effect.

• Higher concentration decreases the rate.

In the experiment with zinc and hydrochloric acid, why was the reaction faster in beaker one?

• It had a catalyst present.

• It had a higher concentration of hydrochloric acid.

• It had a larger surface area of zinc.

• It had a higher temperature.

What effect does increasing the partial pressure of reactants have on the rate of ammonia formation?

• It decreases the rate.

• It has no effect.

• It increases the rate.

• It changes the product.