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Chemistry > C8- Rates and equilibrium > Flashcards

C8- Rates and equilibrium Flashcards

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1
Q

4 ways to monitor progress of a reaction

A

-Volume of mass produced
-Mass of gas lost
-Changes in colour or opacity
-Time for solid to disappear

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2
Q

How to calculate the rate of reaction at a specific time on a graph

A

-Draw a tangent to the curve at specific time
-Draw a right-angled triangle
-Calculate gradient by change in y / change in x
-Include units

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3
Q

Steeper gradient, reaction is…?

A

Steeper the gradient, faster the rate of reaction

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4
Q

3 types of practicals to calculate rate of reaction

A

Measure decreasing mass
Measure increasing volume of gas
Measure decreasing light passing through

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5
Q

Two equations for rate of reaction

A

Amount of reactant used / time
Amount of product made / time

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6
Q

Describe rate of reaction graph

A

-Fastest rate at beginning, maximum number of moles (0s)
-Rate decreases over time as reactants are used up
-Rate reaches 0 when one reactant is used up

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7
Q

5 factors that affect rate of chemical reactions

A

-Temperature
-Surface area of solids
-Concentration of solutions
-Pressure of gases
-Including catalyst

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8
Q

Collision theory

A

For a reaction to occur, reactant particles must collide with sufficient energy

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9
Q

Activation energy

A

Minimum energy that particles must have before they can react

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10
Q

3 general ways to increase rate of reaction

A

-Increase frequency of collisions
-Increase energy of collisions
-Reduce energy required for a reaction

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11
Q

What category does a higher SA:volume ratio increase?

A

Increases frequency of collisions

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12
Q

How to investigate the rate of reaction by volume of gas produced?

A

Measure 20cm3 of 1mol/dm3 HCl into beaker, add carbonate chips. Quickly place a bung connected to gas syringe, start timer. Wait 30s, record volume of gas. Repeat w powder. Higher vol of gas, faster rate of reaction.

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13
Q

Why does increasing SA:Volume ratio increase rate of reaction?

A

-Increases proportion of particles on surface
-Higher frequency of successful collisions
-Increase rate of reaction

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14
Q

What does a higher temperature increase?

A

Increases frequency of collisions
Increases energy of collisions

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15
Q

What has the greatest effect on the rate of reaction: Increased frequency of collisions or increased energy of collisions?

A

An increased proportion of particles exceeding the activation energy

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16
Q

Why does an increased temperature increase rate of reaction?

A

-Particles have more KE
-Move faster, collide more frequently
-Larger proportion of particles have the activation energy
-Greater frequency of successful collisions

17
Q

What does a higher concentration of reactants increase? and why?

A

More particles moving around in the same volume, increase frequency of collisions.

18
Q

What does a higher pressure increase? and why?

A

Same number of particles in smaller volume, closer together.
Increase frequency of collisions

19
Q

Catalyst

A

Chemical substance that increases rate of reaction without being used up

20
Q

How does a catalyst increase rate of reaction?

A

Provide an alternative reaction pathway, with a lower activation energy

21
Q

2 key advantages of catalysts

A

-Save money, no paying to provide high energy
-Help environment, burning less fossil fuels

22
Q

Reversible reaction
and key symbol?

A

Where the products can react together to make the original reactants again
Two half arrows

23
Q

Reversible reaction observations with ammonium chloride

A

When heated ammonium chloride forms ammonia gas and hydrogen chloride, they then cool at top of tube before reacting with each other again to form ammonium chloride solids at the top

24
Q

How to investigate the effect of concentration on the rate of reaction

A

Measure 20cm3 of thiosulfate with a concentration of 8mol/dm3. Place thiosulfate in conical flask on top of a cross. Add 5cm3 HCl to conical flask, swirl once, start stopclock. When cross no longer visible, stop stopclock. Record time taken, calculate rate by using 1/time for reaction. Repeat with dif concs. Plot time against conc on a graph

25
Q

In reversible reactions what type of reaction are they?
Therefore the energy transferred each way?

A

One is endothermic and the other is exothermic
Amount of energy transferred to surroundings is the same amount taken back in

26
Q

What happens when copper sulfate is heated?

A

Copper sulfate contains water, when heated, the water evaporates to produce white anhydrous copper sulfate

27
Q

How to show the heating of copper sulfate is reversible?

A

Heat copper sulfate, collect condensed vapour
Stop heating when solid is white
Add water to white solid
Observe colour change back to blue

28
Q

What is an equilibrium rate of reaction?

A

The rate of forward reaction equals the rate of reverse reaction

29
Q

3 conditions for a dynamic equilibrium

A

Closed system
Rate of forward reaction=rate of reverse reaction
Moles/amount of each reactant and product remain constant

30
Q

Le Chatelier Principle

A

When a change acts on a system at dynamic equilibrium, the position of equilibrium shifts to minimise the change

31
Q

How can pressure affect gases at dynamic equilibrium?
If they have equal moles on each side?

A

Increase in pressure, equilibrium shifts in favour of the side with fewer moles
Equilibrium won’t shift

32
Q

How can temperature affect the dynamic equilibrium?

A

Increased temperature, equilibrium shifts in favour of endothermic side

33
Q

How can the amount of substances affect the dynamic equilibrium?

A

Increased reactants or decreased products–> equilibrium shift to right

34
Q

How can a catalyst affect the dynamic equilibrium?

A

Offers alternative reaction pathway, rates of reactions increase equally, equilibrium reached quicker but position not changed

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