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Chemistry ⚗ > Chapter 8 :) > Flashcards

Chapter 8 :) Flashcards

1
Q

What is the rate of reaction?

A

How fast reactants turn into products

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2
Q

Using a graph, how do you find the rate of reaction at a specific time?

A

Draw a tangent to the curve (a straight line)
Turn this into a right angled triangle with the tangent as the hypotenuse
Calculate the gradient and add units

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3
Q

How can you find the rate of reaction without a graph?

A

How quickly the reactants are used up or how quickly products are made

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4
Q

the steeper the gradient of a tangent

A

the quicker the reaction

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5
Q

how to calculate the mean rate of reaction

A

Quantity of reactant used / time

Quantity of product formed / time

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6
Q

what are the four factors that effect the rate of reaction?

A

concentration/pressure, surface area, temperature and use of a catalyst

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7
Q

What is collision theory?

A

The idea that particles don’t just have to bump each other,they have to do so hard enough to react

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8
Q

What is activation energy?

A

The minimum amount of energy particles need before they can react

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9
Q

Why does a smaller surface area speed up a reaction?

A

More area is exposed to the liquid and are able to react

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10
Q

a smaller surface area = larger

A

surface area to volume ratio

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11
Q

What are the two reasons why temperature increases the rate of reaction?

A

particles collide more often

they collide with more energy

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12
Q

Why does heating a substance mean the particles collide more often?

A

the particles absorb the heat energy and convert it to kinetic

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13
Q

why does something fizz when it reacts?

A

release of carbon dioxide

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14
Q

how to test for carbon dioxide

A

turns limewater cloudy

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15
Q

at room temperature, if you increase it by 10 degrees, what happens to the rate of reaction

A

it doubles

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16
Q

why are reactions more common with a higher temperature?

A

more particles have a temperature higher than the activation energy

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17
Q

why does increasing the concentration increase the rate of reaction?

A

There are more of the particles so collisions are more likely

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18
Q

how to test for hydrogen

A

squeaky pop with a lighted splint

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19
Q

how does increasing the pressure increase rate of reaction?

A

the same number of particles in a smaller space so reactions are more common

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20
Q

what is a catalyst?

A

speeds up a reaction without being effected itself

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21
Q

how do catalysts work?

A

they provide another route to the products with a lower activation energy so reactants take this route and the reaction is faster

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22
Q

advantages of catalysts

A

cost effective - would be more expensive to pay for extra energy
helps environment
can be reused

23
Q

what is a reversible reaction

A

when the reactants react to make the products and the products break down to form the reactants

24
Q

what is the symbol for a reversible reaction?

A

two half arrows

25
in a reversible reaction, what is endothermic?
going from products to reactants
26
in a reversible reaction, what is exothermic?
reactants to products
27
What is a closed system
when nothing can escape (e.g bung in top of tube)
28
What is equilibrium?
When the forward reaction = reverse reaction
29
what is the forward reaction
reactants to products
30
what is the reverse reaction
products to reactants
31
why is equilibrium described as dynamic
because although you cant see it, reactions are still taking place on an atomic level
32
what was la chateliers principle
that when you alter the conditions of an equilibrium, the equilibrium shifts to cancel out the change
33
if you increase one of the reactants in an equilibrium then
the equilibrium shifts left so the reverse reaction happens faster than the forward and more reactant is made
34
under what pressure conditions will an equilibrium change?
When there are different moles of particles on each side
35
if there are the same number of moles on each side of the equilibrium and you increase the pressure, what does it do?
Nothing
36
if you increase the pressure of the reactants, what does the equilibrium do
it shifts to make more of the side that has fewer moles
37
if you increase the temperature of one side of the equilibrium, what will it do?
shift to make more of the endothermic side which results in a drop in temperature
38
decreasing the temperature makes the equilibrium favour the....
exothermic reaction
39
how to tell from a graph when a reaction has finished
the line goes flat
40
when is the reaction going fastest from a graph
when the line is steepest
41
what happend when the product of a reaction is a precipitate?
the solution goes cloudy
42
how to measure the rate of reaction when the product is a precipitate
draw a cross on paper under the conical flask | record the time for it to disappear
43
how to measure rate of reaction using MASS of gas given off
the faster the number on the balance drops, the faster the rate of reaction measure at frequent intervals
44
how to measure the rate of reaction using VOLUME of gas
use a gas syringe to capture any gas produced | more gas produced, faster the rate of reaction
45
how to measure the rate of reaction of magnesium and HCl
set up the experiment attach a gas syringe to the top of the conical flask record the volume of gas produced at regular intervals plot the data and analyse
46
how to measure rate of reaction of sodium thiosulfate and HCl
set up the experiment over a black cross time the time taken for the cross to disappear under the cloudy sulfur the smaller the time, the faster the rate of reaction
47
how to work out the limiing reactant of the equation
work out the number of moles of each of the reactant look at the equation to see how many moles of one react with the other calculate which will be used up first - the limiting reactant
48
where will dynamic equilibrium only take place
closed system
49
what is a equilibrium
when the forward reaction = the reverse
50
what is a dynamic equilibrium
when both reactions are happening but at the same rate, so there is no overall effect
51
what can anhydrous copper sulfate be used to test for
water
52
what are the three changes the equilibrium will try to counteract
temperature concentration pressure
53
what will the equilibrium do if you increase the concentration of the products
shift left to make more reactants

Chemistry ⚗ (17 decks)

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