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CHEMSITRY > 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)
turns this into a right angled triangle with the tangent as the hypotenuse
calculate the gradient and add the 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 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 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

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15
Q

at room temperature if you increase it by 10 degrees what happened 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 on a glowing splint

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19
Q

how does increasing the pressure increase the 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

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

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 reactants

24
Q

what is the symbol for a reversible reaction

A

two half arrows

25
Q

in a reversible reaction what is endothermic

A

going from products to reactants

26
Q

in a reversible reaction what is exothermic

A

reactants to products

27
Q

what is a closed system

A

when nothing can escape

28
Q

what is equilibrium

A

when the forward reaction = reverse reaction

29
Q

what is the forward reaction

A

reactants to products

30
Q

what is the reverse reaction

A

products to reactants

31
Q

why is equilibrium described as dynamic

A

because although you cant see it, reactions are still taking place on an atomic level

32
Q

what was la chateliers principle

A

that when you alter the conditions of an equilibrium, the equilibrium shifts to cancel out the change

33
Q

if you increase one of the reactants in an equilibrium then…

A

the equilibrium shifts left so the reverse reaction happens faster than the forward and more reactant is made

34
Q

under what pressure conditions will an equilibrium change

A

when there are different moles of particles on each side

35
Q

if there are the same number of moles on each side of the equilibrium and you increase the pressure, what does it do

A

nothing

36
Q

if you increase the temperature of one side of the equilibrium what will it do

A

shift to make more of the endothermic side which results in a drop in temperature

37
Q

decreasing the temperature makes the equilibrium favour the

A

exothermic reaction

38
Q

how to tell from a graph when a reaction has finished

A

the line goes flat

39
Q

when is the reaction going fastest from a graph

A

when the line is steepest

40
Q

what happened when the product of a reaction is a precipitate

A

the solution goes cloudy

41
Q

how to measure the rate of reaction when the product is a precipitate

A

draw a cross on paper under the conical flask record the time for it to disappear

42
Q

how to measure rate of reaction using mass of gas given off

A

the faster the number on the balance drops, the faster rate of reaction measure at frequent intervals

43
Q

how to measure the rate of reaction using volume of gas

A

use a gas syringe to capture any gas produced more gas produced, faster rate of reaction

44
Q

how to measure the rate of reaction of magnesium and HCl

A

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

45
Q

how to measure rate of reaction of sodium thiosulfate and HCl

A

set up the experiment over a black cross time the time taken for the cross to disappear under the cloudy sulphur

46
Q

how to work out the limiting reactant of the equation

A

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

47
Q

where will dynamic equilibrium only take place

A

close system

48
Q

what is a dynamic equilibrium

A

when both reactions are happening but at the same rate, so there is no overall effect

49
Q

what can anhydrous copper sulfate be used to test for

A

water

50
Q

what are the three changes the equilibrium will try to counteract

A

temperature concentration pressure

51
Q

what will the equilibrium do if you increase the concentration of the products

A

shift left to make more reactants

CHEMSITRY (13 decks)

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