Chemistry 0620/52 October/November 2019: question paper and mark scheme

Question

You are going to investigate the temperature changes when two different solids, N and O, dissolve in water. Read all the instructions carefully before starting the experiments. Instructions You are going to do two experiments. (a) Experiment 1 ●● Put a polystyrene cup in the 250 cm3 beaker for support. ●● Use the measuring cylinder to pour 30 cm3 of distilled water into the polystyrene cup. ●● Measure the initial temperature of the distilled water and record it in the table. ●● Add all of solid N to the distilled water, start the timer and stir the mixture with the stirring thermometer. ●● Continue to stir the mixture and measure the temperature of the mixture every 30 seconds for three minutes (180 seconds). ●● Record your results in the table. time / s 0 30 60 90 120 150 180 temperature of mixture / °C [2] (b) Experiment 2 ●● Place the other polystyrene cup in the 250 cm3 beaker for support. ●● Use the measuring cylinder to pour 30 cm3 of distilled water into the polystyrene cup. ●● Measure the initial temperature of the distilled water and record it in the table. ●● Add all of solid O to the distilled water, start the timer and stir the mixture with the stirring thermometer. ●● Continue to stir the mixture and measure the temperature of the mixture every 30 seconds for three minutes (180 seconds). ●● Record your results in the table. time / s 0 30 60 90 120 150 180 temperature of mixture / °C [2] (c) Plot your results for Experiments 1 and 2 on the grid. Draw two smooth line graphs. Clearly label your graphs. temperature of mixture / °C 0 30 60 90 120 150 180 210 240 time / s [4] (d) (i) From your graph, deduce the time taken for the initial temperature of the solution in Experiment 2 to change by 3 °C. Show clearly on the grid how you worked out your answer. …… s [3] (ii) Extend your graph for Experiment 1 to suggest the expected temperature of the mixture after 240 seconds. …… °C [1] (e) Is the energy change in Experiment 2 exothermic or endothermic? Explain your answer. . …… . …… [1] (f) State two possible sources of error in these experiments. Suggest two improvements to reduce each of these sources of error. source of error 1 …… improvement 1 . …… source of error 2 …… improvement 2 . …… [4] (g) Suggest and explain the effect on the results if Experiment 1 were repeated using 15 cm3 of distilled water. . …… . …… [2] [Total: 19]

Question

You are provided with two solids, P and Q, which are both salts. Do the following tests on solid P and solid Q, recording all of your observations at each stage. tests on solid P (a) Do a flame test on a small sample of solid P. Record your observations. . …… [1] Add the rest of solid P to about 10 cm3 of distilled water in a boiling tube. Stopper the boiling tube and shake the mixture to dissolve solid P and form solution P. Divide solution P into three approximately equal portions in two test-tubes and one boiling tube. (b) (i) Add a few drops of aqueous sodium hydroxide to the first portion of solution P in a test‑tube. Record your observations. . …… [1] (ii) Now add an excess of aqueous sodium hydroxide to the mixture. Record your observations. . …… [1] (c) (i) Add a few drops of aqueous ammonia to the second portion of solution P in a test‑tube. Record your observations. . …… [1] (ii) Now add an excess of aqueous ammonia to this mixture. Record your observations. . …… [2] (d) Add a small piece of aluminium foil and about 2 cm3 of aqueous sodium hydroxide to the third portion of solution P in a boiling tube. Gently warm the mixture. Test the gas produced with litmus paper. Record your observations. . …… . …… [3] (e) Identify solid P. . …… [2] tests on solid Q (f) Do a flame test on a small sample of solid Q. Record your observations. . …… [1] (g) Add the rest of solid Q to about 5 cm3 of distilled water in a test‑tube. Stopper the test‑tube and shake the mixture to dissolve solid Q. Add a few drops of dilute nitric acid and about 1 cm3 of aqueous silver nitrate to this solution. Record your observations. . …… [1] (h) Identify solid Q. . …… [2] [Total: 15]

Question

The table gives some information about the properties of three substances found in a hand cream. reaction with substance dilute nitric acid polystyrene beads no reaction calcium carbonate reacts and dissolves sodium fluoride dissolves Use the information in the table to plan an experiment to obtain a pure, dry sample of polystyrene beads from this mixture of substances. You are provided with a mixture of the three substances and common laboratory apparatus. . …… . …… . …… . …… . …… . …… . …… . …… . …… . …… [6] Notes for use in qualitative analysis Tests for anions anion test test result carbonate (CO32–) add dilute acid effervescence, carbon dioxide produced chloride (Cl –) acidify with dilute nitric acid, then add white ppt. [in solution] aqueous silver nitrate bromide (Br –) acidify with dilute nitric acid, then add cream ppt. [in solution] aqueous silver nitrate iodide (I–) acidify with dilute nitric acid, then add yellow ppt. [in solution] aqueous silver nitrate nitrate (NO3–) add aqueous sodium hydroxide, then ammonia produced [in solution] aluminium foil; warm carefully sulfate (SO42–) acidify, then add aqueous white ppt. [in solution] barium nitrate sulfite (SO32–) add dilute hydrochloric acid, warm sulfur dioxide produced gently and test for the presence of will turn acidified aqueous sulfur dioxide potassium manganate(VII) from purple to colourless Tests for aqueous cations cation effect of aqueous sodium hydroxide effect of aqueous ammonia aluminium (Al 3+) white ppt., soluble in excess, giving a white ppt., insoluble in excess colourless solution ammonium (NH4+) ammonia produced on warming – calcium (Ca2+) white ppt., insoluble in excess no ppt., or very slight white ppt. chromium(III) (Cr3+) green ppt., soluble in excess grey-green ppt., insoluble in excess copper(II) (Cu2+) light blue ppt., insoluble in excess light blue ppt., soluble in excess, giving a dark blue solution iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess zinc (Zn2+) white ppt., soluble in excess, giving a white ppt., soluble in excess, giving a colourless solution colourless solution Tests for gases Flame tests for metal ions gas test and test result metal ion flame colour ammonia (NH3) turns damp red litmus paper blue lithium (Li+) red carbon dioxide (CO2) turns limewater milky sodium (Na+) yellow chlorine (Cl 2) bleaches damp litmus paper potassium (K+) lilac hydrogen (H2) ‘pops’ with a lighted splint copper(II) (Cu2+) blue-green oxygen (O2) relights a glowing splint sulfur dioxide (SO2) turns acidified aqueous potassium manganate(VII) from purple to colourless