Cambridge & Pearson Edexcel Past Paper Questions
Browse 35,704 questions from Cambridge O-Level & A-Level and Pearson Edexcel IGCSE & IAL exams. Click any question to practice.
The table shows three sets of reagents and reaction conditions. Which sets of reagents and conditions can be used to produce 2-chloro-2-methylpropa...
The compound 'leaf alcohol' is partly responsible for the smell of new-mown grass. leaf alcohol CH3CH2CH=CHCH2CH2OH What will be formed when ‘leaf ...
Compound X: • does not react with Tollens' reagent • forms a yellow precipitate with alkaline I2(aq) • does not react with sodium. What could be th...
Which compound can undergo nucleophilic addition?
C2H5COOCH3 is reacted with aqueous acid. The products from this reaction are reacted with LiAlH4 to form two molecules Y and Z. What are the identi...
A sample of propanoic acid of mass 3.70 g reacts with an excess of magnesium. A second sample of propanoic acid of mass 3.70 g reacts with an exces...
Which statement about H2C=C(CH3)CH2CO2CH3 is correct?
Vitamin C has the structure shown. [Figure showing the structure of Vitamin C] The mass spectrum of vitamin C has a molecular ion peak with an m/e ...
Cobalt, rhodium and iridium are metals in the same group of the Periodic Table.
Chlorine is one of the elements in Group 17 of the Periodic Table.
The Group 14 elements show a change from non-metallic to metallic character down the group. (a) Table 3.1 shows some properties of two Group 14 ele...
Propanone, CH₃COCH₃, is an important organic reagent. [Figure 4.1] shows some reactions of propanone and its derivatives. propanone O // H₃...
Vanadium, niobium and tantalum are metals in the same group of the Periodic Table.
Oxygen is a Group 16 element.
Nitrogen and phosphorus are elements in Group 15 of the Periodic Table.
Bromoalkanes are used widely in industry, although there is increasing concern about their environmental impact. Fig. 4.1 shows a reaction scheme i...
The Group 14 elements show a change from non-metallic to metallic character down the group.
2 Acids react with carbonates to produce carbon dioxide gas. Na2CO3(s) + H2SO4(aq) → Na2SO4(aq) + CO2(g) + H2O(l) This reaction can be used to dete...
When a metal carbonate reacts with a suitable acid, carbon dioxide is produced. You will determine the relative formula mass, M₁, of a metal carbon...
Disodium phosphate, (Na+)2(HPO42¯), reacts with an acid to form monosodium phosphate, Na+(H2PO4¯).
Predict and explain the variation in enthalpy change of hydration for the ions F¯, Cl-, Br¯ and I-.
A and B react together to give product AB. A + B → AB When the concentrations of A and B are both 0.0100 moldm¯³, the rate of formation of AB is 7....
Transition metal atoms and transition metal ions form complexes by combining with ligands.
The shapes of four different complexes, P, Q, R and S, are shown in Table 5.1. The symbol J represents an atom or ion of a transition element. The ...
Benzene, C6H6, reacts with chloroethane, C2H5Cl, in the presence of a suitable catalyst to form ethylbenzene, C6H5C2H5. In the presence of the cata...
A reaction scheme is shown in Fig. 7.1. The reagents needed for reaction 2 and reaction 3 are stated. Reaction 5 takes place when C2H5NH2 is mixed ...
An aqueous solution of phenol, C6H5OH, is acidic at 298 K.
The equation for reaction 1 is shown. reaction 1 X → 2Y Reaction 1 is first order with respect to the concentration of X. The half-life of the reac...
Fig. 2.1 shows an incomplete energy cycle. [Figure 2.1]
The pH of a saturated solution of calcium hydroxide is 12.35 at 298 K. Show that the concentration of hydroxide ions in a saturated solution of cal...
Transition metal atoms and transition metal ions form complexes by combining with species called ligands.
Ni²⁺ ions form a number of different complex ions, including [Ni(H₂O)₆]²⁺, [Ni(NH₃)₆]²⁺ and [Ni(en)₃]²⁺. The abbreviation en represents 1,2-diamino...
Fig. 6.1 shows two reactions of ethanedioic acid, HOOCCOOH. [Figure 6.1]
Benzene reacts with chlorine gas to form chlorobenzene. This reaction can be described as the reaction between benzene molecules and Cl⁺ ions. The ...
The amino acid serine, HOCH₂CH(NH₂)COOH, exists in two optically active forms. These optical isomers, isomer P and isomer Q, are shown in Fig. 8.1....
Transition metal atoms and transition metal ions form complexes by combining with ligands. Co2+ ions form complex ion G. Each G ion contains two Co...
An aqueous solution of phenol, C6H5OH, is acidic at 298 K. Phenol can be produced from phenylamine in a two-step synthesis. [reaction scheme: pheny...
A student uses the following method to determine the percentage by mass of the painkiller aspirin, C9H8O4(s), in some tablets. step 1 Grind five t...
Crystal violet, C25H30N3Cl(s), is a purple dye. Some light is absorbed when it passes through C25H30N3Cl(aq). Absorbance is the proportion of light...
Solution X is dilute hydrochloric acid of unknown concentration. A student uses titration with aqueous sodium carbonate, Na2CO3(aq), to determine t...
A group of students uses the following method to investigate the change in mass that takes place when metal M combines with sulfur to form a metal ...
What is the electrons in boxes notation for the Fe3+ ion?
Which equation has an energy change that is equal to the first ionisation energy of bromine?
The reaction of hydrogen sulfide with sulfur dioxide gives sulfur as one of the products. The two relevant redox equations are shown. H2S(aq) S(s) ...
The bonding between two atoms of nitrogen in an N2 molecule involves the hybridisation of atomic orbitals to form sp orbitals. Which row is correct?
Three bond angles are labelled on the molecule shown. [Figure 6] What is the order of decreasing size of the bond angles x, y and z?
X and Y are different elements in Period 3. Atoms of X and Y each have only one completely filled orbital in their highest occupied energy sub-shel...
A pure sample of a gas has a density of 2.62g dm⁻³ at 101000 Pa and 25°C. The gas behaves ideally under these conditions. Which expression gives th...
When 0.47 g of a hydrocarbon is completely burnt in air, the energy released heats 200 g of water from 23.7 °C to 41.0°C. What is the amount of ene...
One commercially available 'heat pad' contains iron, activated carbon and water. The 'heat pad' is activated by air. This causes the pad to get hot...