Increase in temperature of the reactants can do one of the following

• Slow collision frequency
• Allow less effective collision between the particles
• Neutralise the reaction
• increase collision between the particles thus increasing the rate.

B represents

• energy absorbed
• energy released
• activation energy

A chemical reaction that requires energy to happen

• Exothermic

• Endothermic

• Explosive

• Hot reaction

For the reaction...
SO_2(g) + O_2(g) <−>  SO_3(g)
If the concentration of SO_2(g)  is increased, the equilibrium of the reaction will ___________.

• shift to the left
• shift to the right
• not shift

For the reaction...
SO_2(g) + O_2(g) <−>  SO_3(g)
If the equilibrium shifts to the right, the concentration of O_2(g) will ___________.

• increase
• decrease
• remain the same

Define chemical equilibrium.

• A reaction is reversible.
• The concentration of the reactants is equal to the concentration of the products.
• The rate of a forward reaction is equal to the rate of the reverse reaction.
• The reaction stops and no further change in concentration occurs.

N₂O₄(g) ↔ 2 NO₂(g)

What is the concentration equilibrium constant expression?

• K_eq = [NO₂]²/[N₂O₄]

• K_eq = [N₂O₄]/[NO₂]²

• K_eq = [N₂O₄]²/[NO₂]

• K_eq = [NO₂]/[N₂O₄]²

What is the equilibrium-constant expression for 
CO₂(g) + H₂(g) ↔ CO(g) + H₂O(l)

• K_c= [CO][H₂O] / [CO₂][H₂]  
• K_c= [CO₂][H₂] / [CO]
• K_c= [CO₂][H₂] / [CO][H₂O]
• K_c= [CO] / [CO₂][H₂]  

What is the equilibrium expression for:
Fe₃O₄(s) + 4H₂(g) <--> 3Fe(s) + 4H₂O(g)

• ([Fe]³[H₂O]⁴ ) / ([Fe₃O₄][H₂]⁴)
• ([Fe₃O₄][H₂]⁴)/ ([Fe]³[H₂O]⁴)
• [H₂O]⁴ / [H₂]⁴
• ([Fe][H₂O]) / ([Fe₃O₄][H₂])

Why does increased concentration increase the rate of reaction?

• the activation energy is lowered
• collisions occur with greater energy
• the frequency of collisions is increased