U1- Stoichiometry, Gravimetric Analysis and Gases Flashcards

1
Q

limiting reactant

A

reactant that is completely consumed in reaction

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2
Q

gravimetric analysis

A

technique which the amount of an analyte can be determined through the measurement of mass before and/or after a physical or chemical change

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3
Q

precipitate

A

A solid that is formed in a reaction between two dissolved substances or gases​

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4
Q

analyte

A

The ion or solution being analysed​

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5
Q

residue

A

The solid remaining in the filter paper during filtration​

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6
Q

filtrate

A

The liquid that passes through the filter paper during filtration​

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7
Q

dry to constant mass

A

A process in which a solid is weighed, dried and re-weighed until the mass no longer changes. This ensures that all of the excess water has been completely removed.​

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8
Q

validity

A

whether evidence supports the argument

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9
Q

sources of error in a gravimetric analysis (6)

A

solubility (or insolubility) of precipitate
variation of solubility w temp
losses through splashes, inefficient rinsing and inefficient filtering
extend of drying of solid
is all of the active ingredient precipitated out? (solved by adding excess reagent)
measurement errors

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10
Q

how could solubility of precipitate of gravimetric analysis impact results

A

incomplete precipitation –> lower experimental content then expected –> decreased measurement mass

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11
Q

how could variation in solubility with temperature impact gravimetric analysis results

A

incomplete precipitation –> lower experimental content then expected –> decreased measurement mass

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12
Q

how could losses thru splashing, inefficient rinsing and inefficient filtering impact gravimetric analysis results

A

incomplete transfer of precipitate –> lower exp content than expected –> decreased measured mass

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13
Q

how could the extent of drying the solid impact gravimetric results

A

water in precipitate –> higher experimental content than expected –> increased measured mass

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14
Q

how could not all the active ingredient not being precipitated out impact results of the gravimetric analysis

A

incomplete precipitate –> lower exp content than expected

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14
Q

how could not all the active ingredient not being precipitated out impact results of the gravimetric analysis

A

incomplete precipitate –> lower exp content than expected

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15
Q

how could measurement errors impact gravimetric analysis results

A

random outcome due to inaccuracies w measurements of mass, volume ect

16
Q

properties of ideal gases

A

constant and random motion,
very far apart
negligible attractive or repulsive forces bw particles
collisions bw particles are perfectly elastic (X loss of k nrg)

17
Q

pressure conversions:

kPa to mmHg to atm

A

100kPa = 750mmHg = 0.987atm

18
Q

Boyle’s Law

A

for a fixed amount of gas at constant temperature, pressure is inversely proportional to volume.
P1V1 = P2V2

19
Q

Charles Law

A

For a given amount of gas at constant pressure, volume is directly proportional to the absolute temperature
V1/T1 = V2/T2

20
Q

standard temperature and pressure (STP)

A

0C / 273K

100kPa

21
Q

standard lab conditions (SLC)

A

25C / 298K
100kPa
molar gas v= 22.7L/mol

22
Q

molar gas volume

A

equal volumes of all gases measured at the same temperature and pressure contain the same number of particles

23
Q

why does the solution (silver nitrate) you mix with the analyte need to be in excess
eg Ag+(aq)+ Cl-(aq)> AgCl(s), add Silver Nitrate in excess to mineral water being analysed.(analysis of chloride ions)

A

so that there are more than enough silver ions to precipitate all of the ions out of the solutions

24
Q

atom economy

A

Mr of desired products/ Mr of total products x100

25
Q

% yield

A

actual yield/ theoretical yield x100