Reaction Rates and Equilibrium Review

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

• quantity of reactant used/time taken

• quantity of reactant used - time taken

• quantity of reactant used x time taken

• quantity of reactant used + time taken

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

Tags

NGSS.HS-PS1-5

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

Tags

NGSS.HS-PS1-5

How could you measure the rate of a reaction from a graph?

• Draw a tangent to the curve and calculate the gradient.

• Subtract the value at y away from the value at x

• Divide the x axis value from the y axis value

• Use a ruler and measure the length of the curve.

What is "collision theory"?

• The idea that chemical reactions only occur when particles collide with sufficient energy

• The idea that chemical reactions only occur when particles collide

• The idea of particles react all the time

• The idea that particles cannot react unless forced

Tags

NGSS.HS-PS1-5

What factors DO NOT affect the rate of a reaction?

• Temperature

• Surface area of a solid

• Concentration or reactants in solution

• Colour of the substance

Tags

NGSS.HS-PS1-5

State the effect of increasing the surface area on the rate of a reaction

• Increases the rate

• Decreases the rate

• No effect

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.

State the effect of increasing the concentration on the rate of reaction

• Increases the rate

• Decreases the rate

• No effect

Tags

NGSS.HS-PS1-5