Quiz Collision Theory and Chemical Equilibrium

Define collision theory

• Molecules must collide in the correct orientation and with enough energy for a reaction to occur.

• Molecules need enough activation energy for a reaction to occur.

• Atoms are constantly colliding and reacting.

• The minimum amount of energy needed to speed up the rate of a reaction.

Tags

NGSS.HS-PS1-5

Define rate of reaction

• Rate of reaction is the amount of energy needed for a reaction to occur with enough time.

• Rate of reaction is the energy required to break a bond.

• Rate of reaction is the time it takes for a reaction to reach equilibrium.

• Rate of reaction is the use of a catalyst to speed up reaction time.

Tags

NGSS.HS-PS1-5

Explain how a catalyst increases the rate of reaction.

• Increases the activation energy, which provides an alternate path for the reaction.

• Lowers the activation energy, which provides an alternate path for the reaction.

• Lowers the energy of reactants, which provides an alternate path for the reaction.

• Lowers the energy of products, which provides an alternate path for the reaction.

Tags

NGSS.HS-PS1-4

NGSS.HS-PS1-5

Identify 5 factors that affect the rate of reaction.

• Temperature

  Concentration

  Pressure

  Energy

  Catalyst

• Surface area

  Concentration

  Energy

  Pressure

  Catalyst

• Temperature

  Pressure

  Concentration

  Surface area

  Catalyst

• Pressure

  Surface area

  Density

  Energy

  Catalyst

Tags

NGSS.HS-PS1-5

Explain why increasing the temperature of a reaction increases the rate of reaction.

• Molecules gain kinetic energy with higher temperature. This means molecules will be moving faster, increasing the number of effective collisions that occur with enough energy to activate a reaction.

• Molecules gain kinetic energy with higher temperature. This means molecules will be closer to each other, increasing the probability that they will collide in the correct orientation and react.

• Molecules gain kinetic energy with higher temperature. This means molecules will be moving faster, increasing the probability that they will collide in the correct orientation and react.

• Molecules gain kinetic energy with higher temperature. This means molecules will instantly have enough energy to collide and cause a chemical reaction.

Tags

NGSS.HS-PS1-5

Describe how the rate of reaction changes if you shrink the container size that a gas substance is held in.

• The reaction rate will stay the same

• The reaction rate will speed up

• The reaction rate will slow down

Tags

NGSS.HS-PS1-5

If the reactant particles collide with less than the activation energy, the particles will rebound, and no reaction will occur.

• True

• False

More molecule collisions usually corresponds to a: 

• Faster reaction rate  

• Slower reaction rate

• Constant reaction rate 

• None of the above

Tags

NGSS.HS-PS1-5

Explain why decreasing the concentration of reactants decreases the rate of reaction. (Assume no change in temperature occurs).

• With less molecules available to react, the number of effective collisions that could potentially occur decreases.

• With less molecules available to react, the number of effective collisions that could potentially occur increases due to more space being available.

• Molecules will be moving faster due to having more space; this increases the probability that they will collide in the correct orientation and react.

• Molecules will be moving slower due to having more space; this decreases the probability that they will collide in the correct orientation and react.

Tags

NGSS.HS-PS1-5

Identify two factors that determine if a reaction is at equilibrium.

• Forward reaction rate is faster than the reverse reaction rate and amounts of reactants are greater than the products

• Forward and reverse reaction rates are equal and amounts of reactants and products are constant

• Forward reaction rate is slower than the reverse reaction rate and amounts of reactants are greater than the products

• Forward reaction rate is faster than the reverse reaction rate and amounts of products are greater than the reactants

Tags

NGSS.HS-PS1-6