Arrhenius Equation : Understanding It

The video tutorial explains the relationship between reaction rate and temperature, highlighting that the rate doubles with every 10° rise in temperature. It introduces the Arrhenius equation, which connects the rate constant with activation energy and temperature, based on collision theory. The components of the equation, including the rate constant, frequency factor, and exponential factor, are detailed. The tutorial also discusses how increased temperature provides thermal energy, enhancing kinetic energy and enabling more molecules to surpass activation energy, thus increasing the reaction rate.

What happens to the rate of reaction when the temperature increases by 10°?

• It halves.

• It triples.

• It doubles.

• It remains the same.

Who first studied the influence of temperature on the rate of reaction?

• Marie Curie

• Schmandt Arrhenius

• Albert Einstein

• Isaac Newton

What does the Arrhenius equation relate?

• Rate constant and pressure

• Activation energy and pressure

• Temperature and pressure

• Rate constant and activation energy

According to collision theory, what is necessary for a reaction to occur?

• Reactant molecules must be in a vacuum.

• Reactant molecules must be at absolute zero.

• Reactant molecules must collide with sufficient energy.

• Reactant molecules must be stationary.

What is the value of the gas constant R in the Arrhenius equation?

• 8.314 Joule per Kelvin mole

• 1.38 Joule per Kelvin mole

• 9.81 Joule per Kelvin mole

• 6.022 Joule per Kelvin mole