CIE Jun 2015 v2 Paper 5 Q1

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volume of gas / cm3 This question concerns electrolysis of different compounds. (a) During the electrolysis of dilute sulfuric acid using a current of 0.75 A for 90 minutes, the volume of oxygen gas collected was recorded and is shown in the graph below. 250 200 150 100 50 volume of oxygen 10 20 30 40 50 60 70 80 90 time / min (i) Give equations for the reactions that occur at each electrode in the electrolysis of sulfuric acid.[2] (ii) (iii) On the graph above, use a ruler to draw and label a line (hydrogen) to predict the volume [1] of hydrogen that would be given off during the same experiment. On the graph above, use a ruler to draw and label a line (oxygen) to predict the volume of oxygen that would be produced if a current of 0.45 A was used instead of the 0.75 A used in the original experiment. [1]UCLES 2015 9701/52/M/J/15<br /> (b) During the electrolysis of potassium butanedioate, the following reaction occurs. 2H2O + CH2COO K+ CH2COO K+ potassium butanedioateC2H4 + 2CO2 + H2 + 2K+OH An experiment can be carried out to con rm the above equation. In order to do this, the amounts of hydrogen, ethene and carbon dioxide produced need to be measured. Hydrogen is produced at one electrode, ethene and carbon dioxide are produced at the other. The carbon dioxide can be separated from the ethene by absorbing it in an alkali before the volume of ethene is measured. (i) Using the power supply drawn below, draw a fully labelled circuit diagram and apparatus which shows how: the current could be measured, the hydrogen produced could be collected and its volume measured, the carbon dioxide could be removed using a named alkali, the volume of ethene could be measured. d.c. power supply [5]UCLES 2015 9701/52/M/J/15 [Turn over<br /> (ii) State what measurements should be taken when carrying out the experiment.[2] (iii) C coulombs of electricity resulted in V cm3 of hydrogen gas being produced during the electrolysis. In terms of C and V, state the number of coulombs, N, that would be required to produce 24 dm3 of hydrogen. (iv) In terms of N, state the number of faradays of electricity that would be required to produce 1 mol of hydrogen at room temperature and pressure. (1 faraday of electricity = 96 500 coulombs) [1] (v) Give the equation for the reaction that takes place when the carbon dioxide is absorbed by the alkali. Include state symbols.[1] (vi) Predict the organic product that would be obtained at the anode when a solution of potassium hexanedioate is electrolysed. [1] [1] [Total: 15]UCLES 2015 9701/52/M/J/15<br />

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