1001MSC End-of-Trimester Exam Buster 2020 PDF

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1001MSC PASS EOT EXAM BUSTER Time allowed: 60 minutes

45 marks total

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Please note – this exam buster is not necessarily the structure of your real exam, nor does it cover all the content required for your exam. Do not use this as your only study material

Multiple Choice Questions Answer questions (25 marks)

1. Which of the following would be a possible precipitate formed after a double – displacement reaction? A. Na2 SO4 B. PbSO4 C. BaCl2 D. NH4 NO3 2. What volume will 3.00L of gas occupy if the pressure is changed from 760. mmHg to 560. mmHg? Presume that the temperature remains at 280K. In your answer, please specify which law is most relevant to solve this. A. 4.07L, Charles’ Law B. 3.45L, Boyle’s Law C. 4.07L, Boyle’s Law D. 3.45L, Charles’ Law 3. What volume of hydrogen gas, collected at 40℃ and 1.5atm will be collected when 25g of calcium is combined with an excess of hydrofluoric acid? [Assume atm∗L ] that R = 0.0821 mol∗K

A. 9.25L B. 14.21L C. 15.8L D. 10.7L

4. Butane [C4 H10 ] is burnt in an environment with an excess of oxygen. Assume that the only available products left is CO2 and H2 O. If 29.16g of butane was available for said reaction, how many litres of CO2 can be expected to form at STP (273K, 1atm)? A. 44.8L B. 22.4L C. 11.2L D. 33.6L 5. Refer to the following diagram to answer this question.

In general, it is known that an electronegativity difference between bonded atoms of greater than 1.9 results in bonds that are more ionic than covalent. The compound PCl3 is hence going to be: A. Ionic B. Covalent C. Metallic D. Hydrogen

6. Which of the following has an atom within the compound possessing more than an octet in its valence shell? A. NO B. BF3 C. PCl5 D. HF 7. Which of the following electron configurations describe an atom of chlorine? A. 1s2 2s 2 B. 1s2 2s 2 2p5 C. 1s2 2s 2 2p5 3s2 3p5 D. [Ne]3s2 E. [Ne]3s2 3p5 8. What is the chemical formula of the compound gallium phosphate? A. GaPO4 B. GaPO3 C. GaP4 D. Ga2 PO3 E. Ga(PO3 )2 9. Name the following compounds: PCl5 and Fe2 (SO4 )3 A. Monophosphorus pentachloride, Iron (III) sulphate B. Phosphorus pentachloride, Iron (III) trisulphate C. Phosphorus pentachloride, Iron sulphate D. Phosphorus pentachloride, Iron (III) sulphate E. Phosphorus chloride, Iron (III) sulphate

The following information is required to answer multiplechoice questions 10 and 11. Consider the following reaction: HCl + NaOH → NaCl + H2 O. In an experiment, 1.8066 ∗ 1024 atoms of hydrochloric acid reacted with 79.99g of sodium hydroxide. It was then found that 86.50g of sodium chloride was produced. (NA = 6.022*1023).

10. What was the limiting reactant? A. HCl B. NaOH C. NaCl D. H2 O E. There is no limiting reactant 11. What was the percent yield for sodium chloride? A. 0.925 B. 37% C. 0.53 D. 74% E. 100% 12. What is the oxidation number of carbon in bicarbonate, HCO3 − ? A. -1 B. -3 C. +3 D. -4 E. +4

13. Which of the following rules to assign oxidation number is incorrect? A. All elements in their free state have an oxidation number of zero. B. H is +1, except in metal hydrides where it is -1. C. O is -2, except in peroxides where it is +2 and in oxygen difluoride it is -1. D. In covalent compounds the negative oxidation number is assigned to the most electronegative atom. E. The algebraic sum of the oxidation numbers of the elements in a compound/polyatomic ion is equal to its overall charge 14. The half-life of Radium-226 is 1690 years. If I currently have 268.00 grams, how much would I have in 13520 years? A. 2.09375g B. 1.046875g C. 0.523438g D. 33.5000g E. 16.7500g 15. What is the equation for alpha decay of 226 88 𝑅𝑎 4 He A. 222 86 Rn + 2 4 B. 224 84 Po + 2He 0 C. 226 89 Ac + −1e− 4 D. 222 85 At + 2He 0 E. 226 87 Fr + −1e−

16. Given the equations i) CaCO3(s) ⇌ CaO(s) + CO2(g) ii) Mg(s) + 2H2O(g) ⇌ Mg(OH)2(aq) + H2(g) iii) 2NH3(g) ⇌ N2(g) + 3H2(g) Which of them will be product favoured if volume is decreased? A. i and iii B. iii only C. ii only D. i, ii and iii E. ii and iii 17. How many atoms of carbon would be present in 3 mol of ethanoic acid (CH3COOH)? [NA = 6.022*1023] A. 3 × 6.022×1023 B. 8 × 6.022×1023 C. 2 × 6.022×1023 D. 4 × 6.022×1023 E. 6 × 6.022×1023 18. Which is not an example of a primary function of proteins? A. Transport B. Contraction C. Structure D. Hereditary Information E. Regulation

19. Which of the following is the correct empirical formula for a compound with the molecular formula C21H35O14? A. C3H5O7 B. C7H12O6 C. C3H5O2 D. C7H5O7 E. C2H3O 20. Assuming Ka of 1.8*10-5, what is the pH of 0.9M of CH3COOH at equilibrium? A. pH = 1.8 B. pH = 1.2 C. pH = 2.4 D. pH = 4.74 21. Which of the following is NOT a strong acid? A. HCl B. H2SO4 C. HNO3 D. H2CO3 22. Find the molarity of NaOH solution if 30mL of NaOH neutralises 35mL of 0.2M HCl solution? A. 0.4 M B. 0.20 M C. 0.23 M D. 2.3 M

23. What is the concentration of Sr(OH)2 in a solution with a pH = 11.00? A. 2.0 x 10-11 B. 1.0 x 10-11 C. 5.0 x 10-4 D. 1.0 x 10-3 24. HClO is a weak acid with Ka of 2.9 × 10-8, What concentration of NaClO is required to be combined with 1.4M HClO to produce a buffer of pH 6.2? A. 30.5M B. 0.0643M C. 0.0482M D. 28.8M

OPTIONAL QUESTION THAT MAY HELP WITH CTR 25. Osmolarity refers to the concentration of a solution expressed as the total number of solute particles per litre. The formula for calculating plasma osmolarity is OsmolarityPlasma = 2[Na+ ] + [Glucose] + [Urea] Where [X] represents the concentration of X, and all units are expressed in mmol/L. Bart’s electrolyte panel came up with the following results. Ion Sodium Potassium Bicarbonate Glucose Urea

Reading 143 mmol/L 5 mmol/L 28 mmol/L 5 mmol/L 3 mmol/L

Due to septic shock, fluid replacement therapy is initiated for him. Which of the following is the best graphic representation of what his cells will look like if the intra – venous solution has an osmolarity of 310 mmol/ L?

A.

B.

C.

D. None of the above

Short Answer Questions Answer questions 1 – 7 (20 marks) 1. Refer to the following table in order to answer the following question.

A. In a previous laboratory session, someone has placed a piece of paper next to a sample. It reads “3 mol, 102.27g”, but unfortunately you cannot find the compound that they were referring to. However, you do know that it is one of the four samples listed above. Please draw out the compound that best fits the above description and name the intermolecular bonds that form.

B. How much energy would it take for the compound you identified in part A to be warmed from −70℃ to −10℃? Assume that the specific heat is 1.015Jg −1 K −1, q = mc∆T, and that all 102.27g is to be warmed.

2. Using your knowledge about oxidation numbers, identify the reduction and oxidation half reactions then balance the following equation in acidic solution. Zn + NO3 − → NH4 + + Zn2+

3. In a sealed steel vessel, 0.250mol of Propane (C3 H8 ) burned in 1.75mol of oxygen gas to give carbon dioxide gas and water vapour. A. Write a balanced equation for this reaction.

B. Find the limiting reactant, if any.

C. Calculate the yield CO2 in grams.

D. In moles, how much of the reactant in excess remained?

4. Given the following reaction: S(g) + 3F2(g) ⇌ SF6(g) + 93.5kJ

A. The Keq value for this reaction is 200. Is this reaction product favoured or reactant favoured? B. Given the Keq value is 200 and the concentrations of SF6(g) and F2(g) are 14.3M and 0.84M, what is the concentration of S (g) at equilibrium? 5. Fill in the table with the appropriate acid-base definitions Theory

Arrhenius

Brønsted-Lowry

Lewis

Acid

Base

B. Balance the following equation below, and use Le Chatelier’s Principle to fill in the following table. Stressor

Direction of reaction

Change to C3H8

Change to CO2

Remove CO2

Add C3H8 Increase temperature

Decrease volume of the vessel Add Catalyst

6. The following results were obtained for the titration of 25.0mL of 0.0500M sodium carbonate solution, Na2CO3, against hydrochloric acid

A. Calculate the mean titre in mL (remember 1cm3 = 1mL)

B. Calculate the amount (moles) of sodium carbonate, Na2CO 3, in 25.0mL of the 0.0500M solution

C. Hence calculate the amount (moles) of hydrogen chloride, HCl, used

D. Calculate the concentration of the hydrochloric acid solution to three significant figures

E. A 2nd time the experiment is performed, sodium carbonate is neutralised by sulfuric acid. Assume that 25.0mL of 0.0500M sodium carbonate solution is neutralised this time in reaction with sulfuric acid (H2SO4) assuming mean titre is kept constant (i.e. the same volume of HCl used in the table now becomes the H2SO4 volume used). What is the concentration of this solution of H2SO4? Leave answer in 3 significant figures.

7. If a compound has percent composition by mass 42.86% Carbon, 4.80% Hydrogen, 19.03% Oxygen and 33.3% Nitrogen. What is the empirical formula for this compound?...