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Work out rate constant of first reaction, then work out the new rate from the concentration of H+ in second mixture
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Use proportion to work out the proportional difference in rate, as a proportion of the change of H+ (new rate was x10-5 / 100th of the value given in question)
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Equation for alkaline conditions: CO32- + H2O --> CO2 + 2OH- [1 mark]
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Need to react with an HCl for the conjugate base (sodium benzoate) to accept a proton and form the acid (alkaline hydrolysis makes the salt). Also the salt is ionic which is soluble in water, whereas benzoic acid isn't (even though it can form hydrogen bonds), hence the crystals will precipitate out) [2 marks]
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Percentage yield = 33% (I think) [3 marks]
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Recrystallisation - Dissolve in min amount of hot solvent, filter insoluble impurities from the hot mixture, allow to cool. Crystal will form on cooling, filter under reduced pressure. Then wash in cold solvent and dry for pure product. [2 marks]
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Equation for reaction: Lead oxide + methane --> Lead + CO2 + H2O (needs to be balanced - cant remember the numbers - could have worked it out using redox method) [1 mark]
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Safety precaution - Carry out in a fume cupboard because Pb is a toxic metal [1/2 marks]
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Methods for improvement - Heat until constant mass is obtained, heat for longer (unsure of these) [2 marks]
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Empirical formula - Pb3O4 [2 marks]
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SiO2 is giant covalent between ATOMS, other molecules was simple molecular, with London forces and permanent dipoles between MOLECULES. Giant covalent need more energy to break because they're stronger, hence a higher MP [4 marks]
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1 chiral centre at the bottom of the hexagon [1 mark]
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E/Z could happen because of the double bond, the molecule was a Z isomer, and it could never be E because it had a cyclic ring. The ring cannot be formed if the molecule was an E isomer as 2 points would never join to each other. [4 marks]
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Tests for each functional group - Alkene = Bromine water, would decolourise and form a new compound with Br attached at both sides of double bond. Alcohol = Cr2O72-/H+, was tertiary alcohol, so no colour change, the molecule/product would be the same as the original [4 marks]
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New molecule with new functional groups - had Phenol on it - had to test for a phenol (Bromine water, decolourised upon adding, forms a white ppt. - unsure about the ppt because there were limited areas for substitution) [2 marks]
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Detol Ka Calculation - 1.71x10-10 I think (can't remember the exact number) [5 marks]
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6 Marker - Use Q=mcdeltaT for the first equation, with the mass found by subtraction of the table on the left (think it was 50.7g), calc moles of copper sulphate and divide Q by the answer to get enthalpy change of solution. Use Hess's law cycle for the enthalpy of reaction - was exothermic, around -60kJmol-1 (cant remember exact)
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Standard entropy calculation - +156 [4 marks]
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Can't remember any of the other questions in this section
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Flow diagram - A: [Fe(H2O)6]3+ B: Ag2S [2 marks]
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Equation to form A: 2[Fe(H2O)6]2+ + Cl2 --> 2[Fe(H2O)6]3+ + 2Cl- [1 mark]
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Equation for Manganese Reaction - Standard redox reaction of MnO4- to Mn2+ combined with H2S to S (Overall = 2MnO4- + 5H2S + 6H+ --> 2Mn2+ + 5S + 8H2O [2 marks]
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Work out the mass of water lost, moles of water lost, and then divide this by the moles of the whole crystallised compound to get the number of waters of crystallisation (9H2O), overall compound was Fe(NO3)3
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When burnt, the oxide has to be Fe2O3 as the Iron is definitely Iron(III). Overall gas volume was 270cm3, but one of the gases remained a gas afterwards, which allows you to identify the amounts of each gas in this 270.
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Can work out the moles of the gas that formed a solid (n=v/24), and then work out this gases Mr (Mr=m/n), which gave 46. This corresponds to NO2
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The other information given allowed you to identify O2. However, this could be deduced from what was burning, as this was the only other possible gas from the burning of the salt. It could also be calculated (cant remember how I did it).
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Thiosulphate question - Tetrahedral Shape, Bond angle 109.5o [2 marks]
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Dimer: flip the molecule around, and attach sulphur to sulphur with a single bond [1 mark]
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NMR: 5 peaks as there was 1 plane of symmetry for the benzene environments [1 mark]
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Temperature change from uncertainty - 1oC [1 mark]
Scroll to see replies
•
Work out rate constant of first reaction, then work out the new rate from the concentration of H+ in second mixture
•
Use proportion to work out the proportional difference in rate, as a proportion of the change of H+ (new rate was x10-5 / 100th of the value given in question)
•
Equation for alkaline conditions: CO32- + H2O --> CO2 + 2OH-
•
Need to react with an HCl for the conjugate base (sodium benzoate) to accept a proton and form the acid (alkaline hydrolysis makes the salt). Also the salt is ionic which is soluble in water, whereas benzoic acid isn't (even though it can form hydrogen bonds), hence the crystals will precipitate out)
•
Percentage yield = 33% (I think)
•
Recrystallisation - Dissolve in min amount of hot solvent, filter insoluble impurities from the hot mixture, allow to cool. Crystal will form on cooling, filter under reduced pressure. Then wash in cold solvent and dry for pure product.
•
Equation for reaction: Lead oxide + methane --> Lead + CO2 + H2O (needs to be balanced - cant remember the numbers - could have worked it out using redox method)
•
Safety precaution - Carry out in a fume cupboard because Pb is a toxic metal
•
Methods for improvement - Heat until constant mass is obtained, heat for longer (unsure of these)
•
Empirical formula - Pb3O4
•
SiO2 is giant covalent between ATOMS, other molecules was simple molecular, with London forces and permanent dipoles between MOLECULES. Giant covalent need more energy to break because they're stronger, hence a higher MP
•
1 chiral centre at the bottom of the hexagon
•
E/Z could happen because of the double bond, the molecule was a Z isomer, and it could never be E because it had a cyclic ring. The ring cannot be formed if the molecule was an E isomer as 2 points would never join to each other
•
Tests for each functional group - Alkene = Bromine water, would decolourise and form a new compound with Br attached at both sides of double bond. Alcohol = Cr2O72-/H+, was tertiary alcohol, so no colour change, the molecule/product would be the same as the original
•
New molecule with new functional groups - had Phenol on it - had to test for a phenol (Bromine water, decolourised upon adding, forms a white ppt. - unsure about the ppt because there were limited areas for substitution)
•
Detol Ka Calculation - 1.71x10-10 I think (can't remember the exact number)
•
6 Marker - Use Q=mcdeltaT for the first equation, with the mass found by subtraction of the table on the left (think it was 50.7g), calc moles of copper sulphate and divide Q by the answer to get enthalpy change of solution. Use Hess's law cycle for the enthalpy of reaction - was exothermic, around -60kJmol-1 (cant remember exact)
•
Standard entropy calculation - +156
•
Can't remember any of the other questions in this section
•
Flow diagram - A: [Fe(H2O)6]3+ B: Ag2S
•
Equation to form A: 2[Fe(H2O)6]2+ + Cl2 --> 2[Fe(H2O)6]3+ + 2Cl-
•
Equation for Manganese Reaction - Standard redox reaction of MnO4- to Mn2+ combined with H2S to S (Overall = 2MnO4- + H2S + 6H+ --> 2Mn2+ + 5S + 8H2O
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Work out the mass of water lost, moles of water lost, and then divide this by the moles of the whole crystallised compound to get the number of waters of crystallisation (7H2O), overall compound was Fe(NO3)3
•
When burnt, the oxide has to be Fe2O3 as the Iron is definitely Iron(III). Overall gas volume was 270cm3, but one of the gases remained a gas afterwards, which allows you to identify the amounts of each gas in this 270.
•
Can work out the moles of the gas that formed a solid (n=v/24), and then work out this gases Mr (Mr=m/n), which gave 46. This corresponds to NO2
•
The other information given allowed you to identify O2. However, this could be deduced from what was burning, as this was the only other possible gas from the burning of the salt. It could also be calculated (cant remember how I did it).
•
Thiosulphate question - Tetrahedral Shape, Bond angle 109.5o
•
Dimer: flip the molecule around, and attach sulphur to sulphur with a single bond
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