Reaction Rates and Equilibrium

Explain why increasing the surface area increases the rate of a reaction

• More particles are available to collide, there are therefore more frequent collisions between reactants.

• Less particles are available to collide, there are therefore less frequent collisions between reactants.

• More surface area available to react therefore more space for less frequent collisions.

• Less surface area available to react therefore less space for more frequent collisions.

Explain why increasing the concentration increases the rate of reaction

• More concentrated means more particles in solution, therefore more frequent collisions between reactants.

• Less concentrated means less particles in solution, therefore less frequent collisions between reactants.

• More particles in concentrated solutions is dangerous.

• Increased concentrated means more particles reacting, producing less product an amount of time.

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NGSS.HS-PS1-5

Explain why increasing the pressure of a gas increases the rate of a reaction

• Less space for the particles to move around in, therefore more frequent collisions

• More space for the particles to move around in, therefore more frequent collisions

• Less space for the particles to move around in, therefore less frequent collisions

• More space for the particles to move around in, therefore less frequent collisions

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NGSS.HS-PS1-5

Explain why increasing the temperature increases the rate of reaction

• Increases the speed at which particles move therefore more frequent collisions.

• Decreases the speed at which particles move therefore more frequent collisions.

• Heats the particles which then move therefore less frequent collisions.

• An increase in temperature gives the particles thermal energy.

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NGSS.HS-PS1-5

What is equilibrium?

• The point in a reversible reaction when the forward and reverse reactions are occurring at the same rate in a closed system.

• When the forwards and backwards are equal.

• The reactants and products are equal.

• When the forwards and reverse reactions happen at the same time in a closed container.

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A reaction is at equilibrium when some product is removed. What will occur?

• The forward reaction will increase as that will increase the amount of product

• The backward reaction will increase as that will increase the amount of product

• The forward reaction will increase as that will decrease the amount of product

• The background reaction will increase as that will decrease the amount of product

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The reaction below is at equilibrium. What will occur when the pressure is increased? 2H₂(g) + O₂(g) ⇌ 2H₂O(g)

• The forward reaction will increase as there are fewer molecules on the right.

• The forward reaction will increase as there are more molecules on the right.

• The backward reaction will increase as there are fewer molecules on the right.

• The backward reaction will increase as there are more molecules on the right.

What is the formula for a mean rate of reaction in terms of products?

• quantity of reactant product formed/time taken

• quantity of reactant product formed - time taken

• quantity of reactant product formed x time taken

• quantity of reactant product formed + time taken

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How can you measure the quantity of a reactant or product?

• In grams or in cm³

• In mg or in cm³

• In grams or in dm³

• In mg or in dm³

What are the two possible units for rate of reaction?

• g/s or cm³/s

• mg/s or cm³/s

• g/s or dm³/s

• mg/s or dm³/s

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NGSS.HS-PS1-5