The video tutorial explains how activation energy and temperature influence chemical reaction rates. By maintaining a constant activation energy and varying temperature, it demonstrates that reaction rates double with a 10°C increase. The Arrhenius equation is applied to show that the rate constant is proportional to the exponential factor, which increases with higher temperatures and lower activation energies. The rate law is discussed, concluding that reducing activation energy and increasing temperature enhances the rate constant and reaction rate.

What happens to the fraction of molecules undergoing reactions when the temperature is increased by 10°?

• It decreases by half.

• It doubles.

• It triples.

• It remains the same.

According to the Arrhenius equation, what is the rate constant directly proportional to?

• The pressure of the system.

• The exponential factor.

• The concentration of reactants.

• The activation energy.

How can the F value be increased according to the Arrhenius equation?

• By keeping the temperature constant.

• By lowering the activation energy and increasing the temperature.

• By decreasing the absolute temperature.

• By increasing the activation energy.

What does the rate law of a reaction express?

• The rate of reaction is directly proportional to the rate constant.

• The rate of reaction is independent of the rate constant.

• The rate of reaction is inversely proportional to the rate constant.

• The rate of reaction is inversely proportional to the concentration of reactants.

What is the effect of lowering activation energy and increasing temperature on the rate of reaction?

• It decreases the reaction rate.

• It increases the rate constant.

• It has no effect on the rate constant.

• It decreases the rate constant.