MARIYA INTERNATIONAL SCHOOL Work sheet II Term II Level 8 Chemistry [Paper IV] Name: 1. Chemists use the concept of the mole to calculate the amounts of chemicals involved in a reaction. a) Define mole. b) 3.0 g of magnesium was added to 12.0 g of ethanoic acid. Mg + 2CH3COOH (CH3COO)2 Mg + H2 The mass of one mole of Mg is 24 g. The mass of one mole of CH3COOH is 60 g. i. Which one, magnesium or ethanoic acid, is in excess? You must show your reasoning. ii. How many moles of hydrogen were formed?
iii. Calculate the volume of hydrogen formed, measured at r.t.p. 2. In an experiment, 25.0cm 3 of aqueous sodium hydroxide, 0.4mol /dm 3, was neutralized by 20.0cm 3 of aqueous oxalic acid, H2C2O4. 2NaOH + H2C2O4 Na2C2O4 + 2H2O Calculate the concentration of the oxalic acid in mol /dm 3 i. Calculate the number of moles of NaOH in 25.0 cm 3 of 0.4 mol /dm 3 solution.
ii. Use your answer to (i) and the mole ratio in the equation to find out the number of moles of H2C2O4 in 20 cm 3 of solution. iii. Calculate the concentration, mol /dm 3, of the aqueous oxalic acid. 3. Propene reacts with hydrogen iodide to form 2 - iodopropane. CH3 CH = CH2 + HI CH3 CHI CH3 1.4 g of propene produced 4.0 g of 2 - iodopropane. Calculate the percentage yield. Moles of CH3 CH=CH2 reacted =.. Maximum moles of CH3 CHI CH3 that could be formed = Mass of one mole of CH3 CHI CH3 = 170 g Maximum mass of 2 - iodopropane that could be formed = Percentage yield % =..
4. 6.0g of ethanoic acid, Mr = 60, was reacted with 5.5 g of ethanol, Mr = 46. Determine which is the limiting reagent and the maximum yield of ethyl ethanoate, Mr = 88. Number of moles of ethanoic acid =... Number of moles of ethanol =... The limiting reagent is... Number of moles of ethyl ethanoate formed =... Maximum yield of ethyl ethanoate =...
5. What is the maximum mass of silver(i) chromate(vi) which could be obtained from 20cm 3 of aqueous silver(i) nitrate, concentration 0.2 mol /dm 3? 2AgNO3 (aq) + K2CrO4 (aq) Ag2CrO4 (s) + 2KNO3 (aq) Number of moles of AgNO3 used =... Number of moles of Ag2CrO4 formed =... Mass of one mole of Ag2CrO4 = 332 g Mass of Ag2CrO4 formed =... g
6. Strontium chloride-6-water can be made from the insoluble compound, strontium carbonate, by the following reactions. SrCO3 (s) + 2HCl SrCl2 (aq) + CO2 (g) + H2O (l) SrCl2 (aq) + 6H2O SrCl2. 6H2O In the above experiment, 50.0cm 3 of hydrochloric acid of concentration 2.0mol/dm 3 was used. 6.4 g of SrCl2.6H2O was made. Calculate the percentage yield. Number of moles of HCl used =... Number of moles of SrCl2.6H2O which could be formed =... Mass of one mole of SrCl2.6H2O is 267g Theoretical yield of SrCl2.6H2O =...g Percentage yield =...%
7. Dilute hydrochloric acid reacts with sodium carbonate solution. i. Calculate how many moles of hydrochloric acid were used.... mol ii. Use your answer to (i) and the equation for the reaction to calculate the number of moles of sodium carbonate that reacted.... mol iii. Use your answer to (ii) to calculate the concentration of the sodium carbonate solution in mol / dm 3.... mol / dm 3
iv. In another experiment, 0.020 mol of sodium carbonate were reacted with excess hydrochloric acid. Calculate the maximum volume (at r.t.p.) of carbon dioxide gas that could be made in this reaction. 8. Calcium chloride can be made by reacting calcium carbonate with hydrochloric acid.... dm 3 An excess of calcium carbonate was added to 50.0 cm 3 of 0.500 mol / dm 3 hydrochloric acid. The solution was filtered to remove the excess calcium carbonate. (a) How many moles of HCl were used in this reaction? (b) Deduce the number of moles of carbon dioxide gas made in this reaction.... mol... mol
(c) Calculate the mass of carbon dioxide made in this reaction.... g (d) Calculate the volume, in dm 3, of carbon dioxide made in this reaction at room temperature and pressure (r.t.p.).... dm 3 9. Chlorine, bromine and iodine are halogens. (a) Chlorine can be made in the laboratory by heating manganese (IV) oxide with concentrated hydrochloric acid. Calculate the volume of 8.00 mol / dm 3 HCl (aq) needed to react with 3.48 g of MnO2. moles of MnO2 used... mol
moles of HCl needed... mol volume of HCl needed... cm 3 10. 7.26 g of a hydrate, Cu(NO3)2.xH2O, formed 2.4 g copper(ii) oxide. Number of moles of CuO formed =... Number of moles of Cu (NO3)2.xH2O in 7.26 g =... Mass of 1 mole of Cu (NO3)2.xH2O =... g Mass of 1 mole of Cu (NO3)2 is 188 g The value of x in this hydrate =...