more... Flashcards

1
Q

what are exothermic reactions

A

reactions that give out heat as the reactants change to products so the temp changes

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2
Q

what are endothermic reactions

A

reactions that take in heat as reactants change to products so the temp drops

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3
Q

what is enthalpy change

A

heat energy change measured under a constant pressure

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4
Q

what are standard conditions

A

100KPa

298K

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5
Q

what is the standard state of an element

A

physical state under standard conditions

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6
Q

what is the definition of standard enthalpy change of combustion

A

the enthalpy change when one mole of substance is completely burned in oxygen under standard conditions, with all reactants and products in their standard states

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7
Q

what does standard enthalpy change refer to

A

heat change measured at 100KPa and 298K

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8
Q

what is the definition of standard enthalpy change of formation

A

the enthalpy change when one mole of substance is formed from its elements under standard conditions, with all reactants and products in their standard states

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9
Q

what equation would you use to calculate the heat change for a reaction

A

Q=Mc > T

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10
Q

what is Hess’s Law

A

the enthalpy change for a reaction is the same, whatever route is taken from reactants to products

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11
Q

how is an enthalpy change different from a heat change

A

an enthalpy change is an energy change measured under a stated temp and constant stated pressure

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12
Q

what is the unit of energy

A

Joules

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13
Q

what is the most stable form of Carbon, and what state symbol is it given

A

Graphite (s)

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14
Q

what value is given to deltaH of elements

A

zero, no energy is needed to form an element from its element

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15
Q

why will the value calculated for an enthalpy change be different using mean bond enthalpies compared to thermochemical cycles

A

mean bond enthalpies are averages, and the true value will differ. thermochemical cycle is ‘correct’ answer

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16
Q

are mean bond angels positive or negative? why?

A

Positive because energy must be put in to break bonds

17
Q

when drawing enthalpy diagrams, what do we take as 0

A

elements

18
Q

what Is meant by the bond dissociation enthalpy

A

the enthalpy change required to break a covalent bond, with all species in the gaseous state

19
Q

what is the difference between heat and temp.

A

temp- average kinetic energy of the particles in a system

heat- total amount of energy of all particles present

20
Q

do endothermic reactions have positive or negative values

A

positive

21
Q

explain the trend in electronegativity that we see in the halogens

A

halogens become more electronegative as we move up the group because the distance between the nucleus and the bonding electrons decreases, so does shielding

22
Q

what sort of agents are halide ions

A

reducing agents

23
Q

what happens to the ability of halide

ions to act as reducing agents as we move down the group? why?

A

increases because more shielding and size of atom means outer elecrons are less strongly attracted to the nucleus and so are easily lost

24
Q

why is the reaction of sodium bromide with concentrated sulphuric acid different from the reaction of sodium chloride with it

A

bromide ions are stronger reducing agents than chloride ions so are able to reduce the sulphuric acid to sulphur dioxide

25
Q

how can we predict if one halogen will displace another halogen ion

A

a halogen will displace the ion of a halogen that is below it in the periodic table

26
Q

explain the trend in boiling point that we see in the halogens

A

Bp increases as we move down the group. because larger atoms have more electrons an so stringer van der waals forces between molecules

27
Q

how do halogens normally react

A

by gaining electrons

28
Q

what sort of agent are halogens

A

oxidising

29
Q

what happens to the ability of halogens to act as oxidising agents as we move down the group? why?

A

decreases because increased shielding and size of atom means electrons are less strongly attracted to the nucleus

30
Q

why are the products from the reaction of NaBr with conc H2SO4 different from Nal?

A

iodide ions are stronger reducing agents than bromide ions, so reduce the sulphur further

31
Q

what reagent would you use to distinguish between halide ions

A

Acidified silver nitrate

32
Q

what acid would you chose to acidify silver nitrate

A

nitric acid

33
Q

why do we acidify silver nitrate before testing halogen ions

A

to remove ions that would form precipitates and interfere with results eg carbonate

34
Q

what colour precipitates are formed when halide ions react with acidified silver nitrate

A

AgF- none
AgCL- white
AgBr- cream
AgI- yellow

35
Q

what is the trend in solubility of the silver halides as we move down the group

A

becomes less soluble
AgCl- dissolves in dilute ammonia
AgBr- dissolves in conc. ammonia
AgI- insoluble in conc. ammonia

36
Q

what do we call a reaction in which an element is both oxidised and reduced

A

disproportionation

37
Q

what is the formula of chloric(1) acid

A

HClO

38
Q

why is chlorine added to water

A

it produces chloric (1) acid which kills bacteria by oxidation and is also a bleach

39
Q

what is the formula of sodium chlorate? what are the oxidation numbers if the elements in it

A

NAClO-
NA +1
Cl +1
O -2