Cambridge & Pearson Edexcel Past Paper Questions

Aqueous bromine reacts with methanoic acid to form hydrogen bromide and carbon dioxide gas. Br₂(aq) + HCO₂H(aq) → 2HBr(aq) + CO₂(g) The table shows...

Naphtha is a mixture which contains only hydrocarbon molecules.

Propene, C₃H₆, reacts with H₂O in the presence of an acid catalyst to form an alcohol with molecular formula C₃H₈O.

A Group 2 metal combines with bromine to form a crystalline solid, MBr2. Excess aqueous AgNO3 is added to a solution of MBr2 and a precipitate form...

The strength of interaction between particles determines whether the substance is a solid, liquid or gas at room temperature.

A large excess of 2-bromo-2-methylpropane is added to 0.0010mol of NaOH(aq), which contains a few drops of phenolphthalein indicator. A stopwatch i...

The table shows the structural formulae of four compounds, A, B, C and D, with molecular formula C4H8. structural formula | name A CH3CH2CH=CH2 | B...

S is a secondary alcohol with molecular formula C4H10O. [Reaction scheme diagram] S C4H10O step 1 PBr3 T C4H9Br step 2 U C4H9CN step 3 dilute acid ...

The elements in Group 17 are known as the halogens.

Methanol, CH3OH, is soluble in water because it forms hydrogen bonds with water molecules.

Separate samples of R, S, T and U are added to cold water. The identity of each sample is unknown. However, each sample is known to be pure and can...

1,3-dichloropropan-2-ol can be made by reacting M. [Figure showing M reacting to form 1,3-dichloropropan-2-ol]

Compound X contains the same functional groups as citric acid. [Figure showing the skeletal structure of citric acid] The table describes some of t...

Iron(II) sulfate crystals, FeSO4•xH2O, contain water of crystallisation. You will carry out a titration to determine the value of x in the formula,...

In Question 1 you used a titration method to determine the value of x in a hydrated salt. In Question 2 you will use a gravimetric method. In this ...

When anhydrous sodium carbonate dissolves in water the following reaction occurs. Na2CO3(s) + aq → 2Na+(aq) + CO32-(aq) The enthalpy change for thi...

2 In this experiment you will determine the value of x in the formula for hydrated sodium thiosulfate, Na₂S₂O₃•xH₂O. In this formula x is an intege...

The carbonates and hydroxides of Group 2 elements show similar trends in thermal stability. Suggest and explain the variation in the trend in the t...

Explain why chromium complexes are coloured.

Define the term transition element.

Samples of [Cu(H2O)6]2+ are reacted separately with an excess of aqueous sodium hydroxide or with an excess of aqueous ammonia. Give the following ...

Dinitrogen pentoxide, N₂O₅, is dissolved in an inert solvent (solv) and the rate of decomposition of N₂O₅ is investigated. This reaction produces n...

Compare and explain the relative acidities of butanoic acid, ethanol, ethanoic acid and water. > most acidic > least acidic

3-aminobenzoic acid can be synthesised from methylbenzene in three steps. [Figure showing reaction scheme from methylbenzene to M (step 1), M to N ...

The sketch graph for the titration of ethanoic acid, CH₃CO₂H, with sodium hydroxide is shown. [Figure showing titration curve, pH vs volume of NaOH...

The carbon-13 (¹³C) NMR spectrum of compound A, C₈H₈O₂, contains six peaks. Compound A reacts with an excess of bromine water to give compound B, C...

An aqueous solution of chromium(III) contains the green [Cr(H2O)6]3+ complex ion.

State and explain the trend observed in the thermal stability of the Group 2 nitrates. ...............................................................

Define the term standard electrode potential. ........................................................................................................

Define the term lattice energy. ......................................................................................................................

Describe and explain the relative basicities of phenylamine, ethylamine and 4-nitrophenylamine. most basic ..........................................

There are four possible structural isomers of C8H10 that contain a benzene ring. Draw the skeletal formulae of the four structural isomers in the a...

In aqueous solution, chlorine dioxide, ClO2, reacts with hydroxide ions as shown. 2ClO2 + 2OH- → ClO3- + ClO2- + H2O A series of experiments is car...

State and explain the relative rate of hydrolysis of acyl chlorides, alkyl chlorides and aryl chlorides. fastest ....................................

Dinitrogen pentoxide, N2O5, is dissolved in an inert solvent (solv) and the rate of decomposition of N2O5 is investigated. This reaction produces n...

3-aminobenzoic acid can be synthesised from methylbenzene in three steps. [Figure reaction scheme from methylbenzene to 3-aminobenzoic acid via M a...

The sketch graph for the titration of ethanoic acid, CH3CO₂H, with sodium hydroxide is shown. [Figure titration curve]

Hydrogen peroxide decomposes slowly at room temperature to give water and oxygen. 2H2O2(aq) → 2H2O(l) + O2(g) The initial rate of this reaction can...

A student is given 250.0 cm³ of solution containing a mixture of Fe2+ and Fe3+ ions. The student is asked to find the total mass of iron ions and t...

A student is asked to find the enthalpy change for the reaction between anhydrous magnesium sulfate and water. MgSO4(s) + 7H2O(l) → MgSO4•7H2O(s) T...

A student is asked to determine the acid dissociation constant, Kₐ, for butanoic acid, CH3CH2CH2COOH. Kₐ = [CH3CH2CH2COO⁻][H⁺] / [CH3CH2CH2COOH] Th...

Equations involving four enthalpy changes are shown. Na(g) → Na⁺(g) + e⁻ ΔH = W Na(g) → Na²⁺(g) + 2e⁻ ΔH = X Na(s) → Na(g) ΔH = Y Na(s) → Na²⁺(g) +...

This question refers to isolated gaseous atoms in the ground state. In which atom are all electrons paired?

Which sample contains the most iodine?

When a small sample of hydrocarbon Q is completely combusted, it produces 3.52 g of carbon dioxide and 1.44 g of water. What could be the structure...

Ethane and ethene are both hydrocarbon molecules. What is a feature of both molecules?

Elements J and L are both in Group 15. J and L each form a gaseous covalent hydride in which their oxidation number is –3. In the liquefied forms o...

Which gas will behave least like an ideal gas at 150 °C and 101 kPa?

When an evacuated glass bulb of volume 200 cm³ is filled with a gas at 300 K and 101 kPa, the mass of the bulb increases by 0.68 g. The gas obeys t...

The standard enthalpy of formation of NO₂(g) is +33.2 kJ mol⁻¹. The standard enthalpy of formation of N₂O₄(g) is +9.2 kJ mol⁻¹. What is the standar...