Kinetics can be Fun!

Systems in equilibrium have

• rates that are constant

• concentrations that are equal

• rates that are equal

Tags

NGSS.HS-PS1-6

Given N₂(g) + 3H₂(g) <--> 2NH₃(g) + 92 KJ

What would happen if temperature was raised?

• More NH₃ would be created

• More N₂ would be created

• The amount of H₂ would decrease

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

When the surface area of a reactant is increased, reactions speed up because

• there are more exposed particles to react

• the density of the particles is increased

• one of the reactants' concentrations will have increased

• the activation energy would have been lowered

What must occur for a chemical reaction to take place?

• a gas must be formed

• catalysts are required

• particles must collide effectively

Tags

NGSS.HS-PS1-5

Which arrow represents the activation energy of the forward reaction?

• A

• B

• C

• D

Given the balance equation:

KNO₃ (s) + 85 kJ ----> K⁺ (aq) + NO₃- (aq)

Which statement best describes this reaction?

• Endothermic and delta H is + 85 kj

• Endothermic and delta H is -85 kj

• Exothermic and delta H is -85 kj

• Exothermic and delta H is + 85 kj

Tags

NGSS.HS-PS1-4

Given the reaction at equilibrium:

2NO₂ (g) <--> N₂O₄ (g) + 55 kj.

Which answer best explains why there is a shift to the right when the pressure is increased?

• The reaction is exothermic

• The reaction is endothermic

• There are 2 moles of gases on the left, while there's only 1 mole of gas on the right

The presence of a catalyst would impact the following letters:

• C only

• A and D

• B and C

Tags

NGSS.HS-PS1-4

Given the balanced equation,

4Fe(s) + 3O₂(g) ---> 2Fe₂O₃ (s) + 1640 kj,

which phrase best describes the reaction?

• exothermic with a negative delta H

• endothermic with a negative delta H

• exothermic with a positive delta H

• endothermic with a negative delta H

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

The difference between the potential energy of the products and the potential energy of the reactants is defined as

• equilibrium

• catalyst

• activation energy

• heat of reaction