rate of reaction

Question 1

steps to core rate of reaction practical.

Answer 1

1. support a gas syringe with a stand, boss and clamp
2. using a measuring cylinder, add 50cm3 of dilute hydrochloric acid
3. add 0.4 g of calcium carbonate and immediately add syringe
4. record the time for every 10cm3 of gas produced

5 repeat with different concentrations of hydrochloric acid

Question 2

how do we measure rate of reaction?

Answer 2

. How fast the reactants are being used up
. How fast the products are being formed

Question 3

what are the two equations for rate of reaction?

Answer 3

Quantity of reactants formed divided by the time taken.

Quantity of reactants used divided by the time taken

Question 4

what is the collision theory?

Answer 4

The collision theory is the idea that for particles to react, they have to collide with one another with sufficient energy, (activation energy)

Question 5

what does the rate of reaction depend on?

Answer 5

. The amount of energy the particles have.

How often the particles collide

Question 6

how does temperature affect the rate of reaction?

Answer 6

The temperature causes the particles to move faster and so colliding more frequently. Temperature also increases the energy of particles, therefore leading to more stressful collisions.

Question 7

how does concentration affect rate of reaction?

Answer 7

If we increase the amount of concentration of particles in a given area, there is then an increased chance of more successful collisions and therefore more reactions

Question 8

how does surface area affect rate of reaction?

Answer 8

A higher surface area allows for more reactions to take place since there is more area in which they will take place

Question 9

what is a catalyst?

Answer 9

A substance that speeds up a reaction without being used up in the reaction

Question 10

how does a catalyst increase the rate of reaction

Answer 10

A catalyst reduces the activation energy and therefore allows for more successful collisions

Question 11

what is a one-way reaction?

Answer 11

A one-way reaction is there the reactants react to form a product, but the product cannot be reversed into the reactants

Question 12

What is a reversible reaction?

Answer 12

A reversible reaction is where a reactant can react to form a product, but also where the product can be reversed, and react to form the reactant

Question 13

what is equilibrium?

Answer 13

Equilibrium is where the rate of reaction in a reversible reaction even out, where the rate of reaction for the product is equal to the rate of reaction for the reactants

Question 14

what is the position of equilibrium?

Answer 14

The position of equilibrium is where more Product or reactant is being formed. Position of equilibrium lies to the right a greater concentration of product is being formed, whereas if the position of equilibrium lies to the left, a greater concentration of reactant is being formed at equilibrium.

Question 15

what can be done to encourage the forward reaction when at equilibrium?

Answer 15

If heat is added, the food reaction is encouraged, a more product is produced

Question 16

what can be done to encourage the backwards reaction when at equilibrium?

Answer 16

If cold, the backward reaction is encouraged, and more reactants are formed

Question 17

Why can equilibrium only be reached in a closed system?

Answer 17

equilibrium can only be reached in a close system as to prevent products from escaping as if products escaped. Then the rate of reaction would not even out and would therefore not be at equilibrium

Question 18

What is the correlation between exothermic and endothermic and a reversible reaction?

Answer 18

in a reversible reaction, either the forwards or backward reaction is either exothermic or endothermic. For example, in one reaction, the forward reaction might be exothermic and therefore the backward reaction could be endothermic.