0620/62 · May/June 2026
Download PDFAlkanes are flammable hydrocarbons. Table 1.1 gives the boiling points of three alkanes. Table 1.1
| alkane | boiling point |
| hexane | 69 |
| pentane | 36 |
| undecane | 196 |
A student uses the apparatus shown in Figure 1.1 to separate a mixture of the three alkanes in Table 1.1.
Name the items of apparatus in Figure 1.1 labelled A and B. A ............................................................................................................................................... B ...............................................................................................................................................
Draw an arrow on Figure 1.1 to show where the apparatus should be heated.
Explain why a Bunsen burner should not be used to heat the apparatus.
Write a W on Figure 1.1 to show where water enters the apparatus labelled A.
State which alkane is collected first. Give a reason for your answer. alkane ....................................................................................................................................... reason .......................................................................................................................................
State what, if anything, is left in the flask at the end of the experiment. Explain your answer. left in flask ................................................................................................................................. explanation ...............................................................................................................................
A student investigates the volume of gas made in 75 seconds when dilute ethanoic acid reacts with solid sodium hydrogencarbonate. The student does five experiments using the apparatus shown in Figure 2.1. Experiment 1 • Use a measuring cylinder to pour of dilute ethanoic acid into a conical flask. • Use a measuring cylinder to pour of distilled water into the conical flask. Swirl the flask to mix the contents. • Set up the apparatus as shown in Figure 2.1. Ensure the inverted measuring cylinder is full of water. • Remove the stopper from the conical flask. • Add of solid sodium hydrogencarbonate to the conical flask. Do not mix the contents of the flask. Immediately replace the bung and start the stop-watch. • Measure the volume of gas collected in the inverted measuring cylinder at 75 seconds. • Rinse the conical flask with distilled water. Experiment 2 • Repeat Experiment 1 using of distilled water instead of . Experiment 3 • Repeat Experiment 1 using of distilled water instead of . Experiment 4 • Repeat Experiment 1 using of distilled water instead of . Experiment 5 • Repeat Experiment 1 using of distilled water instead of .
Use the information in the descriptions of the experiments and the measuring cylinder diagrams to complete Table 2.1.
Complete a suitable scale on the y-axis and plot your results from Experiments 1 to 5 on Figure 2.2. Draw a line of best fit.
The mean rate of reaction is calculated using the equation shown. Calculate the mean rate of reaction in Experiment 3. Give units for the mean rate you have calculated. mean rate of reaction = ............................................................... units ...............................................................
State which Experiment, 1, 2, 3, 4 or 5, has the highest mean rate of reaction.
Use your graph in Figure 2.2 to predict the volume of gas collected in 75 seconds if the volume of distilled water is . Show your working on Figure 2.2. volume = ...............................................................
State why a measuring cylinder is used rather than a measuring cylinder to measure the volume of the dilute ethanoic acid.
The volume of the dilute ethanoic acid can be measured using a volumetric pipette. State one advantage of using a volumetric pipette rather than a measuring cylinder to measure the volume of the dilute ethanoic acid.
Some of the gas made in the reaction escapes from the conical flask before the stopper is replaced in the flask. State the effect, if any, the gas escaping has on the volume of gas collected in 75 seconds.
Deduce in which experiment the most gas would escape. Explain your answer. experiment ........................................................................................................................ explanation ........................................................................................................................
Sketch a line on Figure 2.2 to show the results that would be obtained if the experiment is repeated with of dilute ethanoic acid instead of .
A student tests two substances: solid C and solution D.
State the conclusion that can be made from the observation made in test 2.
Identify the three ions in solid C.
Tests on solution D Solution D is aqueous ammonium bromide. The student divides solution D into two approximately equal portions. Record the expected observations. To the first portion of solution D, the student adds aqueous sodium hydroxide in excess. observations .............................................................................................................................
The student gently warms the product from 3(c). Any gas given off is tested. observations .............................................................................................................................
To the second portion of solution D, the student adds about of dilute nitric acid followed by a few drops of aqueous silver nitrate. observations .............................................................................................................................
Tin is a metal that is between copper and iron in the reactivity series. The ore cassiterite contains the compound tin(IV) oxide, . Tin(IV) oxide is insoluble in water and reacts with dilute acids to form an aqueous solution of a salt. The ore cassiterite contains no other compounds that are insoluble in water and no other compounds that react with acids to form aqueous solutions. Describe how you could obtain a sample of tin metal starting with a large lump of the ore cassiterite. You are provided with common laboratory apparatus and chemicals.