School of Chemistry UNIVERSITY OF KWAZULU-NATAL, WESTVILLE JUNE 2008 EXAMINATION CHEM181: CHEMISTRY FOR ENGINEERS 1A DURATION: 2HOURS TOTAL MARKS: 100
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1 School of Chemistry UNIVERSITY OF KWAZULU-NATAL, WESTVILLE JUNE 2008 EXAMINATION CHEM181: CHEMISTRY FOR ENGINEERS 1A DURATION: 2HOURS TOTAL MARKS: 100 External Examiner: Internal Examiner: Professor M Sankar Mr A Bissessur IMPORTANT: COMPLETE THIS SECTION IMMEDIATELY SURNAME AND INITIALS (Optional): SIGNATURE: STUDENT NUMBER: SEAT NO.: 1. This paper consists of 14 pages including the cover page, periodic table and two data sheets. Please ensure that you have them all. 2. The use of non-programmable electronic calculators is permitted. Question TOTAL Internal External STUDENTS ARE REQUESTED, IN THEIR OWN INTEREST, TO WRITE LEGIBLY
2 Page 2 QUESTION 1 25 MARKS (a) Chemical substances are classified as elements and compounds, define them in detail. (3) (b) The boiling point of Helium is -452 o F. Convert this value to degrees celsius. (c) Why is there a need to express the number of significant figures in chemical measurements? (1) (d) Express the following calculations in scientific notation: ( ) (1) (e) What is the number of significant figures in the following measurements? (a) ton (1) (b) 2900 g (1) (f) Carry out the following arithmetic operation and report off the answers to the correct number of significant figures: ( m) - ( m) (1)
3 Page 3 QUESTION 1 continued (g) What does an atom of an element consist of? (1) (h) How many protons, neutrons, and electrons are in a 138 Ba atom? (i) Give the correct notation for an isotope that contains 82 protons, 82 electrons, and 126 neutrons. (1) (j) Name the following chemical compounds: (i) Ag 2 CO 3 (1) (ii) Na 2 O 2 (1) (k) Write formulas for the following compounds: (i) nickel (II) perchlorate (1) (ii) Carbonic acid (1) (l) (i) Explain, using copper sulphate as an example, what is meant by hydrated compounds. (ii) What happens to the hydrated copper sulphate as it is heated. (1)
4 Page 4 QUESTION 1 continued (m) Give the product of the following reaction and indicate whether it is acidic, basic or amphoteric in nature: (i) 2S + 3 O 2 (ii) Give an an equation to illustrate the property identified (i) above. QUESTION 2 25 MARKS (a) Give the products and classify the type of reaction (combination, decomposition, displacement, redox or metathesis) for the following: Reaction Products Reaction classification (i) Li 2 O(s) + H 2 O(l) (1) (1) (ii) Ca(s) + H 2 O (l) (1) (1) (iii) BaCl 2 (aq)+znso 4 (aq) (1) (1) (b) Define the term molar mass and give its unit. (c) Calculate the number of moles of chloroform (CHCl 3 ) in 198 g of chloroform.
5 Page 5 QUESTION 2 continued (d) How many moles of sulfuric acid, H 2 SO 4 are needed to react with mol of NaOH by the following reaction? 2NaOH (aq) + H 2 SO 4 (aq) Na 2 SO 4 (aq) + 2 H 2 O (l) (e) Calculate the percent composition by mass of each of the elements in N 2 O 5. (3) (f) Give the empirical formula of: (i) C 4 H 10 (1) (ii) C 2 H 5 OH (1)
6 Page 6 QUESTION 2 continued (g) The compound caffeine contains the elements C, H, N and O. Combustion analysis of a 1.500g sample of caffeine produces g of CO 2 and g of H 2 O. Further analysis of another sample of caffeine showed that the compound contained % of nitrogen (N) by mass. Its molar mass was determined and found to be 194.2g mol -1. (i) Determine its empirical formula (6) (ii) Determine its molecular formula
7 Page 7 QUESTION 3 25 MARKS (a) Explain the term limiting reagent in a chemical reaction. (1) (b) Explain what is theoretical yield of a product in a chemical reaction. (1) (c) Give a mathematical expression for the calculation of percentage yield of a product. (1) (d) Aluminium sulfate can be made by the following reaction: 2AlCl 3 (aq) + 3H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 6HCl(aq) In an experiment 25.0g of AlCl 3 were mixed with 30.0g of H 2 SO 4. Eventually 28.46g of pure Al 2 (SO 4 ) 3 was produced. (i) Identify, using a calculation which reagent is in excess and by how much (in grams). (5) (ii) Calculate the percentage (%) yield of Al 2 (SO 4 ) 3. (3)
8 Page 8 QUESTION 3 continued (e) Differentiate between intermolecular and intramolecular forces. (f) Draw the Lewis dot structure for the ClO 4 - ion. (Cl = central atom, Cl = group 7, O=group 6) (g) (i) State Boyle s Law. (ii) Give the general form applicable to a gas at constant temperature that arose out of Boyle s Law. (1) (h) Calculate the volume (in L) occupied by 100 g of HCl gas generated at STP.
9 Page 9 QUESTION 3 continued (i) Write the formula and define all symbols used in the expression derived from the ideal gas equation for the calculation of density. (j) The density of a gaseous organic compound is 3.38 g/l at 40 o C and 1.97atm. Calculate its molar mass (g mol -1 ). (3) QUESTION 4 25 MARKS (a) Hydrogen gas is generated when calcium metal reacts with water. The volume of gas collected over water at 30 o C and a pressure of 988 mmhg is 641 ml. Calculate the mass (in grams) of the hydrogen gas obtained. (The pressure of water vapour at 30 o C is mmhg.) (6)
10 Page 10 QUESTION 4 continued (b) (i) Define the enthalpy of a reaction. (ii) Give an expression (defining all symbols) for the change in enthalpy for a constant pressure process. (c) Calculate the AH rxn for the reaction (see Table attached for standard enthalpy of formation): C 2 H 4 (g) + 5O 2 (g) 4CO 2 (g) + 2H 2 O (l) (3) (d) Why is it not possible to calculate the standard enthalpy of formation of some compounds directly?
11 Page 11 QUESTION 4 continued (e) Calculate the enthalpy of formation of ethane according to the equation, 2C(graphite) + 3H 2 (g) C 2 H 6 (g) from the following data: (1) C(graphite) + O 2 (g) CO 2 (g) ΔH = kj H 2 (g) + ½O 2 (g) H 2 O(g) ΔH = kj (3) 2C 2 H 6 (g) + 7O 2 (g) 4CO 2 (g) + 6H 2 O(g) ΔH = kj (6) (f) Give the raw materials (concentration not necessary) used in the production of Portland cement. (g) Explain what clinker is in the cement manufacturing process.
Students are requested, in their own interests, to write legibly.
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