Factors affecting chemical reaction rates

The rate of a reaction increases as temperature__________________.

• Decreases
• Increases
• Stays the Same

Tags

NGSS.HS-PS1-5

Products will form faster if____________

• the particle size of the reactants are larger.
• temperature is decreased.
• concentration of the reactants are increased.
• the reaction is not stirred.

A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 

• catalyst
• product
• reactant
• solute

A catalyst works by

• changing the order of the reaction
• increasing the temperature
• lowering the activation energy
• making the activated complex

Tags

NGSS.HS-PS1-4

If the temperature is reduced, a reaction rate will ______

• increase

• decrease

• stay the same

If the concentration of a reactant is increased, the reaction rate will ___________.

• increase

• decrease

• stay the same

Tags

NGSS.HS-PS1-5

How does a catalyst increase the rate of a chemical reaction?

• Provides lower energy route for the reaction so that a greater number of particles have enough energy to react.

• Increased number of collisions increases the chance of a 'successful collision'

• Particles collide faster and harder so a larger proportion have greater energy than the required activation energy.

How does temperature increase the rate of a chemical reaction?

• Provides lower energy route for the reaction so that a greater number of particles have enough energy to react.

• Increased number of collisions increases the chance of a 'successful collision'

• Particles collide faster and harder so a larger proportion have greater energy than the required activation energy.

• Greater number of 'active sites' available for a reaction to take place (referring to solids)

How does concentration increase the rate of a chemical reaction?

• Provides lower energy route for the reaction so that a greater number of particles have enough energy to react.

• Increased number of collisions increases the chance of a 'successful collision'

• Particles collide faster and harder so a lagrer proportion have greater energy than the required activation energy.

• Greater number of 'active sites' available for a reaction to take place (referring to solids)

The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?

• Red, because the activation energy is larger
• Blue, because the activation energy is lower
• both reaction progress at the same rate