C8 - Rates, Equilibrium and Organic Chemistry

Question 1

Rate of Chemical Reaction

Answer 1

How long it takes for the reactants to turn into products

Question 2

Rate of Reaction Profiting

Answer 2

Companies want to speed up chemical reactions quickly but safe so that they can profit quickly

Question 3

Measuring Mass of Reaction Mixture

Answer 3

• Put it in concealed conical flask on scales

- When reaction takes place, record the time and mass and regular intervals

Question 4

Measuring Volume of Gas

Answer 4

• Reactions sometimes produce gas which can tell you the time it took for reaction to take
• Do this by collecting gas in a syringe and measure the volume at time intervals

Question 5

Measuring Light Passing Through a Solution

Answer 5

• Some reactions in a solution allows a solid to not dissolve while in the water
• This makes the solution go cloudy , we can use it measure rate of reaction

Question 6

Measure Mean Rate of Reaction

Answer 6

Quantity of Reaction Used (or Product Formed) / Time

Question 7

Collision Theory

Answer 7

Reactions only occur when particles are oriented correctly and have enough energy to collide with other particles

Question 8

What Activation Energy

Answer 8

Minimum amount of energy to start a reaction

Question 9

Surface Area

Answer 9

• Smaller the object is, the more S.A : Vol it will have
• A cube of sugar will take longer dissolve than a lump of powdered sugar as it has solution surrounding each sugar molecule
• Larger the S.A, quicker the reaction

Question 10

Why high S.A has faster reactions

Answer 10

More particles = more chance of collisions

Question 11

Temperature

Answer 11

• Increase allows particles to move more often with more energy
• Decrease makes particles have less energy and move slower

Question 12

Concentration

Answer 12

Increase of reactants in solution means collisions will occur more frequently

Question 13

Pressure

Answer 13

Particles are more closely packed together, making collisions occur more frequently

Question 14

Catalyst

Answer 14

• Cheaper than other ways of speeding reactions
• Catalysts can be reused, some different catalysts can only work for some reactions
• Reduces the activation energy, giving reactants a quicker path to collide with

Question 15

Reversible Reactions

Answer 15

Products can revert back to the reactants while giving back the same amount of energy taken

Question 16

Types of Reactions

Answer 16

Reactants to Products (Endothermic) (Forward Reaction)

Products to Reactants (Exothermic) (Reverse Reaction)

Question 17

Conservation of Energy

Answer 17

Energy cannot be created of destroyed, only transferred

Question 18

Dynamic Equilibrium

Answer 18

• When amount of Products produced is the same amount of Reactants produced in a reversible reaction
• Shown on a graph with rate of reaction for Forward and Reverse Reactions on the same point