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Grade 12 Chemistry national exam, 2010 E.C. (2018 G.C.)

71 questions · 120 minutes. The first 5 answers are shown with explanations; sit the whole paper timed in the app to get your score and the textbook page behind every question.

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  1. 1.Fats and oils are:
    • A. Acids
    • B. Alcohols
    • C. Alkenes
    • D. Esters
    Answer: D. Fats and oils belong to a group of compounds called esters. Their molecules form when glycerol joins with fatty acids. A is wrong because fats and oils are not acids. B is wrong because they are not alcohols, although glycerol is an alcohol used to make them. C is wrong because they do not have the carbon-carbon double bonds that define alkenes. Textbook: Grade 11, unit 6 · section 6.6.4.
  2. 2.The reaction between alcohols and acyl chlorides produces
    • A. Ethers
    • B. Esters
    • C. Carboxylic acids
    • D. Aromatic salts
    Answer: B. The key idea is that alcohols react with acyl chlorides to form esters. B is correct because this reaction makes an ester. A ethers, C carboxylic acids, and D aromatic salts are not the main products of this reaction. Textbook: Grade 11, unit 6 · section 6.5.3.
  3. 3.When a student draws a plausible Lewis structure for hydrazine molecule ( ), how many lone pair of electrons are available?
    • A. 1
    • B. 4
    • C. 3
    • D. 2
    Answer: D. The question tests how to count lone pairs in a Lewis structure. In $N_2H_4$, each nitrogen forms three single bonds and has one lone pair, giving two lone pairs in total. Option A counts only one nitrogen atom's lone pair. Option B counts too many lone pairs. Option C also counts too many lone pairs. Textbook: Grade 11, unit 2 · section 2.3.
  4. 4.Who used the cathode Ray tube to discover the electron and determine its charge to mass ratio?
    • A. Robert A. Millikan
    • B. James Chadwick
    • C. J.J Thomson
    • D. Ernest Rutherford
    Answer: C. The question tests who used a cathode-ray tube to study electrons. J.J. Thomson used it to discover the electron and measure its charge-to-mass ratio. A is wrong because Millikan measured the electron's charge. B is wrong because Chadwick discovered the neutron. D is wrong because Rutherford is known for work on the atomic nucleus. Textbook: Grade 9, unit 3 · section 3.5.
  5. 5.Compounds that contain the carboxyl (carbonyl and hydroxyl) group are said to be:
    • A. Organic acids
    • B. Ketones
    • C. Aldehydes
    • D. Esters
    Answer: A. The question tests which compounds contain the carboxyl group, written as $\mathrm{-COOH}$. Organic acids contain this group, which has a carbonyl part and a hydroxyl part. Ketones have a carbonyl group between two carbon atoms, not a carboxyl group. Aldehydes have a carbonyl group at the end of a carbon chain, not a carboxyl group. Esters contain an $\mathrm{-COO-}$ ester linkage, not a carboxyl group. Textbook: Grade 11, unit 6 · section 6.3.2.
  6. 6.The main ore of lead is called:
    • A. Zinc blend
    • B. Galena
    • C. Cinnabar
    • D. Chromite
    Answer, explanation and textbook page: open in the app.
  7. 7.During nitrification, bacterial convert into
    • A. $\mathrm{N_2}$, $\mathrm{N_2O}$ in to nitrous oxide
    • B. $\mathrm{NO_3^-}$, $\mathrm{NH_4^+}$ or nitrates into ammonium
    • C. $\mathrm{N_2}$ into nitrates
    • D. $\mathrm{N_2}$, nitrous oxide into nitrogen
    Answer, explanation and textbook page: open in the app.
  8. 8.Which one of the following metals exists in a free state?
    • A. Na
    • B. Mg
    • C. Pt
    • D. Zn
    Answer, explanation and textbook page: open in the app.
  9. 9.A ___ corresponds to an ___ process.
    • A. Negative, endothermic
    • B. Positive, exothermic
    • C. Zero, exothermic
    • D. Positive, endothermic
    Answer, explanation and textbook page: open in the app.
  10. 10.Which of the following is NOT both a Bronsted-Lowry acid and a Bronsted-Lowry base?
    • A. $\mathrm{HS^-}$
    • B. $\mathrm{OH^-}$
    • C. $\mathrm{HCO_3^-}$
    • D. $\mathrm{HSO_4^-}$
    Answer, explanation and textbook page: open in the app.
  11. 11.Chlorine has an oxidation number of +5 in:
    • A. $\mathrm{NaClO_3}$
    • B. $\mathrm{NaClO_2}$
    • C. $\mathrm{NaClO}$
    • D. $\mathrm{NaClO_4}$
    Answer, explanation and textbook page: open in the app.
  12. 12.What is a measure of the closeness of a measurement to its true value?
    • A. Accuracy
    • B. Precision
    • C. Reproducibility
    • D. Usefulness
    Answer, explanation and textbook page: open in the app.
  13. 13.The monomer of neoprene is:
    • A. Butadiene
    • B. Isoprene
    • C. Chloroprene
    • D. 2-methyl-1,3-butadiene
    Answer, explanation and textbook page: open in the app.
  14. 14.What is the sum of $3.72\times10^8$ and $4.62\times10^7$ to the correct significant figure?
    • A. $4.991\times10^7$
    • B. $4.17\times10^8$
    • C. $4.172\times10^8$
    • D. $4.99\times10^7$
    Answer, explanation and textbook page: open in the app.
  15. 15.Which of the following is a natural polymer?
    • A. PVC
    • B. Rubber
    • C. Perspex
    • D. Teflon
    Answer, explanation and textbook page: open in the app.
  16. 16.When a sodium chromate $\mathrm{Na_2CrO_4}$ solution is acidified, it is converted to:
    • A. $\mathrm{Cr_2O_7^{-2}}$
    • B. $\mathrm{Cr_2O_3}$
    • C. $\mathrm{CrO_3}$
    • D. $\mathrm{Cr(s)}$
    Answer, explanation and textbook page: open in the app.
  17. 17.Nylons are:-
    • A. Amides
    • B. Peptides
    • C. Polyesters
    • D. Polyamides
    Answer, explanation and textbook page: open in the app.
  18. 18.Which quantum number is used to be determine sub shells?
    • A. Principal quantum number
    • B. Magnetic quantum number
    • C. Spin quantum number
    • D. Azimuthal quantum number
    Answer, explanation and textbook page: open in the app.
  19. 19.The maximum kinetic energy of a photoelectron emitted from a metal is $1.03\times10^{-19}\,\text{J}$ when light that has a $656\,\text{nm}$ wavelength shines on the surface. What is the threshold frequency for this metal?
    • A. $4.57\times10^{14}\,\text{s}^{-1}$
    • B. $3.02\times10^{14}\,\text{s}^{-1}$
    • C. $3.02\times10^{-14}\,\text{s}^{-1}$
    • D. $4.57\times10^{-14}\,\text{s}^{-1}$
    Answer, explanation and textbook page: open in the app.
  20. 20.What is the maximum number of electrons in an atom that can have the principal quantum number n = 4?
    • A. 34
    • B. 8
    • C. 32
    • D. 18
    Answer, explanation and textbook page: open in the app.
  21. 21.Which of the following questions expresses de Broglie's hypothesis?
    • A. $\lambda = h/(mv)$
    • B. $\blacklozenge\Delta E = hc/\lambda$
    • C. $v = c/\lambda$
    • D. $\blacklozenge\Delta E = c/\lambda$
    Answer, explanation and textbook page: open in the app.
  22. 22.What skill is a scientist using when he/she listens to the sounds that animals make?
    • A. Drawing conclusions
    • B. Making a hypothesis
    • C. Interpreting data
    • D. Making observations
    Answer, explanation and textbook page: open in the app.
  23. 23.Which of the following is fundamentally different from the others?
    • A. Light waves
    • B. Radio waves
    • C. Sound waves
    • D. Microwaves
    Answer, explanation and textbook page: open in the app.
  24. 24.What is (are) the bond angle (s) in $\mathrm{SF_6}$?
    • A. $109.5^\circ$
    • B. $90^\circ$
    • C. $90^\circ$ and $109.5^\circ$
    • D. $180^\circ$
    Answer, explanation and textbook page: open in the app.
  25. 25.The number of resonance structures for are:
    • A. 9
    • B. 2
    • C. 3
    • D. 6
    Answer, explanation and textbook page: open in the app.
  26. 26.In the following equation, what type of hybridization change, if any occurs at the Xe atom? sp d 3 sp d 3 2 dsp2 sp3
    • A. to
    • B. to sp3 sp d 3 sp d 3 sp3
    • C. to
    • D. to
    Answer, explanation and textbook page: open in the app.
  27. 27.Which of the following compounds does NOT contain an ionic bond?
    • A. $\mathrm{NaOH}$
    • B. $\mathrm{HCl}$
    • C. $\mathrm{K_2S}$
    • D. $\mathrm{LiH}$
    Answer, explanation and textbook page: open in the app.
  28. 28.Which of the following statements about oxygen and fluorine is NOT correct?
    • A. O has a smaller atomic radius than F.
    • B. O has a smaller electron affinity than F. O2− F−
    • C. has a larger ionic radius than .
    • D. O and F have the same number of core electrons.
    Answer, explanation and textbook page: open in the app.
  29. 29.What will be the charges on the ions formed when silicon reacts with nitrogen?
    • A. $\mathrm{Si^{2+}},\ \mathrm{N^{2-}}$
    • B. $\mathrm{Si^{3+}},\ \mathrm{N^{3-}}$
    • C. $\mathrm{Si^{4+}},\ \mathrm{N^{2-}}$
    • D. $\mathrm{Si^{4+}},\ \mathrm{N^{3-}}$
    Answer, explanation and textbook page: open in the app.
  30. 30.The equilibrium constant for the ionization of HCN is Which of the following statements is true regarding this equilibrium? (I) The reaction is product favoured. (II) The reaction is reactant favoured. (III) Equilibrium lies far to the right. (IV) Equilibrium lies far to the left.
    • A. II and III
    • B. I and IV
    • C. I and III
    • D. II and IV
    Answer, explanation and textbook page: open in the app.
  31. 31.The rate equation for the decomposition of nitramide, is rate = which of the following mechanisms is consistent with this rate equation? H NNO ⇌ 2 2 H + + HNNO 2 HNNO → 2 − N O + 2 OH− H + + OH → − H O 2 H NNO + → 2 2 H+ ⇌H NNO 3 2 + H NNO → 3 2 + N O + 2 H O 3 + H O ⇌ 3 + H + + H O 2
    • A. fast equilibrium; slow; fast
    • B. fast; slow; fast equilibrium H NN → 3 2 + N O + 2 H O 2 H NNO → 2 2 OH + − NH 4 + NH ⇌ 4 + NH + 3 H+ H O ⇌ 2 H + + OH−
    • C. slow
    • D. slow; fast equilibrium; fast equilibrium
    Answer, explanation and textbook page: open in the app.
  32. 32.Given the equilibrium constant values: What is the value of for + 2 3O (g) ⇌ 2 2N (g) 2 4 O the following reaction? 1.2 ? × 10−6 2.4 × 10−6
    • B. 1.2 × 106 4.8 × 106
    Answer, explanation and textbook page: open in the app.
  33. 33.Which of the following factors does NOT affect the rate of a chemical reaction?
    • A. Concentration
    • B. Nature of reactants
    • C. Temperature
    • D. Humidity
    Answer, explanation and textbook page: open in the app.
  34. 34.Which of the following orbital diagrams is correct for the carbide ion( )? σ σ σ σ π 1s 2 1s ∗2 2s 2 2s ∗2 2p 4 σ σ σ σ π σ π 1s 2 1s ∗2 2s 2 2s ∗2 2p 4 2p 2 2p ∗2
    • B. σ σ σ σ π σ 1s 2 1s ∗2 2s 2 2s ∗2 2p 4 2p 2 σ σ σ σ π σ π 1s 2 1s ∗2 2s 2 2s ∗2 2p 4 2p 2 2p ∗4
    Answer, explanation and textbook page: open in the app.
  35. 35.If a reaction is zero order in A, tripling the concentration of A will cause the reaction rate to:
    • A. Increase by a factor of 3
    • B. Remain constant
    • C. Increase by a factor of 27
    • D. Increase by a factor of 9
    Answer, explanation and textbook page: open in the app.
  36. 36.The phrase "like dissolves like" refers to the fact that:
    • A. Polar solvents dissolve non polar solutes and vice versa
    • B. Solvents can only dissolve solutes of similar molar mass
    • C. Polar solvents dissolve polar solutes and non-polar solvents dissolve non polar solutes
    • D. Gases can only dissolve other gases
    Answer, explanation and textbook page: open in the app.
38 An ester has the structural formula shown below. On hydrolysis, the ester would produce: [Figure: A printed skeletal/condensed structural formula of an ester. On the left, written on one line, is the chain CH3CH2CH2C. From that terminal carbon two bonds branch to the right: an upward-sloping double bond (two parallel lines) to an O written above and to the right, and a downward-sloping single bond to OCH2CH3 written below and to the right.
  1. 37.The overall structure is ethyl butanoate, CH3CH2CH2C(=O)OCH2CH3.]
    • A. Propanoic acid and propan -1 ol
    • B. Bunanoic acid and ethanol
    • C. Ethanoic acid and butan -1 -ol
    • D. Propanoic acid and ethanol
    Answer, explanation and textbook page: open in the app.
  2. 38.You are given a bottle of solid x and three aqueous solutions of Y, the first saturated the second unsaturated and the third supersaturated. Which of the following is correct, if you add a small amount of the solid solute to each solution?
    • A. The solution n which the added solid solute dissolves is the saturated solution.
    • B. The solution is which the added solid solute remains undissolved is the unsaturated solution.
    • C. In all the three solution, saturated. Unsaturated and supersaturated the added solid solute will dissolve.
    • D. The supersaturated solution is unstable and addition of additional solute causes the excess solute to crystallize.
    Answer, explanation and textbook page: open in the app.
  3. 39.Consider the following equilibrium: $2\mathrm{CO(g)} + \mathrm{O_2(g)} \rightleftharpoons 2\mathrm{CO_2(g)}$ $K_{\mathrm{eq}} = 4.0 \times 10^{-10}$ What is the value of $K_{\mathrm{eq}}$ for $2\mathrm{CO_2(g)} \rightleftharpoons 2\mathrm{CO(g)} + \mathrm{O_2(g)}$?
    • A. $2.5 \times 10^9$
    • B. $2.0 \times 10^{-5}$
    • C. $5.0 \times 10^4$
    • D. $4.0 \times 10^{-10}$
    Answer, explanation and textbook page: open in the app.
  4. 40.For a certain gas phase reaction Which of the 25 C 0 200 C 0 following would be true if the temperature was increased from to ? I. The value of k would be smaller. II. The concentration of A(g) would be increased III. The concentration of B(g) would increase
    • A. I
    • B. II
    • C. I and II
    • D. III
    Answer, explanation and textbook page: open in the app.
  5. 41.Which of the following compounds would be the most soluble in ?
    • A. Ethane
    • B. Pentane
    • C. Ethanoic acid
    • D. Octanoic acid
    Answer, explanation and textbook page: open in the app.
  6. 42.A 0.2M solution of a weak acid HA is 1% ionized at $25^\circ\mathrm{C}$ $K_a$ for the acid is equal to:
    • A. $\frac{0.01\times0.01}{0.19}$
    • B. $\frac{0.02\times0.02}{0.18}$
    • C. $\frac{0.002\times0.002}{0.198}$
    • D. $\frac{0.19}{0.01\times0.01}$
    Answer, explanation and textbook page: open in the app.
  7. 43.What species of ions are present in a 0.1M solution of HCl and what will be their equilibrium concentrations? [H O] = 3 + 0.1M [OH] = − 10 M −13 [Cl] = − [H O] = 3 + 0.1M [OH] = − 0.1M [Cl] = − 0.1M
    • A. ; ,
    • B. ; , 0.1M [H O] = 3 + 0.1M [OH] = − 0.01M [Cl] = − 0.1M [H O] = 3 + 10−13 [OH] = − 0.1M [Cl] = − 0.1M
    • C. ; ,
    • D. ; ,
    Answer, explanation and textbook page: open in the app.
  8. 44.Commercial concentrated sulphuric acid (density = $1.831\,\text{g cm}^{-3}$) is 94.0% $\mathrm{H_2SO_4}$ by mass. What is the normality of $\mathrm{H_2}$)
    • A. 16.8M
    • B. 35.0N
    • C. 28.2
    • D. 40.4M
    Answer, explanation and textbook page: open in the app.
  9. 45.2.3g of ethanol ( ) is added to 500g of water. What is the molality of the resulting solution?
    • A. 0.1m
    • B. 0.01m
    • C. 1.0m
    • D. 10.0m
    Answer, explanation and textbook page: open in the app.
  10. 46.A 0.5L and 0.1 solution is to be prepared by dilution process form a 13M nitric acid. How many ml conc. and how many ml of water are required to prepare the dilute solution?
    • A. 2ml and 498 ml water
    • B. 10ml and 490ml water HNO 3 HNO 3 HNO 3 HNO 3
    • C. 20ml and 490ml water
    • D. 3.85ml and 496.15ml water
    Answer, explanation and textbook page: open in the app.
  11. 47.During the electrolysis of a concentrated aqueous solution of NaCl, what substance is formed at the cathode?
    • A. Chlorine
    • B. Hydrogen
    • C. Oxygen
    • D. Sodium
    Answer, explanation and textbook page: open in the app.
  12. 48.In a voltaic cell, electrons flow from the___________ to the __________
    • A. Anode, cathode
    • B. Salt bridge, anode
    • C. Anode, salt bridge
    • D. Salt bridge, cathode
    Answer, explanation and textbook page: open in the app.
  13. 49.What is the PH of a mixture of 15.0ml of 0.126M NaOH and 21.0M ?
    • A. 1.7
    • B. 11.81
    • C. 2.15
    • D. 13.6
    Answer, explanation and textbook page: open in the app.
  14. 50.Which of the following correctly lists electromagnetic waves in order from shortest to longest wavelength?
    • A. Microwaves, ultraviolet, visible light, gamma rays
    • B. Gamma rays, ultraviolet, infrared, microwaves
    • C. Radio waves, infrared, gamma rays, ultraviolet
    • D. Gamma rays, infrared, ultraviolet, microwaves
    Answer, explanation and textbook page: open in the app.
  15. 51.The relationship between Pico meter (pm) and nanometre (nm) is:
    • A. 1nm = 1000pm
    • B. 1nm = 10pm
    • C. 1pm = 100nm
    • D. 1pm = 10nm
    Answer, explanation and textbook page: open in the app.
  16. 52.What would be the wavelength of a radio wave having a frequency of 3 MHz?
    • A. 100nm
    • B. 300m
    • C. 100m
    • D. 300nm
    Answer, explanation and textbook page: open in the app.
  17. 53.The process of vulcanization of rubber makes it
    • A. More soluble in solvents
    • B. Soft
    • C. Less elastic
    • D. Hard
    Answer, explanation and textbook page: open in the app.
  18. 54.Which of the following is NOT the decomposition product of $\mathrm{HNO_3}$?
    • A. $\mathrm{NO_2}$
    • B. $\mathrm{O_2}$
    • C. $\mathrm{N_2O_4}$
    • D. $\mathrm{H_2O}$
    Answer, explanation and textbook page: open in the app.
  19. 55.The determine the volume of an irregularly shaped glass vessel, the vessel is weighed empty ($121.3\text{g}$) and when filled with $\mathrm{CCl_4}$ ($283.2\text{g}$). What is the volume capacity of the vessel, given that the density of $\mathrm{CCl_4}$ is $1.59\text{g}/\text{cm}^3$?
    • A. $76.29\text{cm}^3$
    • B. $178.11\text{cm}^3$
    • C. $101.82\text{cm}^3$
    • D. $257.42\text{cm}^3$
    Answer, explanation and textbook page: open in the app.
  20. 56.For the reaction , was found to be atm/s, where Δp(H ) 2 Δp(H H )/Δt 6 14 is change in the pressure of hydrogen. Determine in units of atm/s for this reaction at the same time. 6.2 × 10−2 1.6 × 10−3
    • B. −6.2 × 10−3 2.5 × 10−2
    Answer, explanation and textbook page: open in the app.
  21. 57.The decomposition of a compound at is first order with a half - life of 1570 seconds what fraction of an initial amount of the compound remains after 4710 seconds?
    • A. 1/8
    • B. 1/12
    • C. 1/6
    • D. 1/3
    Answer, explanation and textbook page: open in the app.
  22. 58.Given the following species, , , , , . What is the correct order of F - A - F bond angles? 2 < 2 BeF < 2 NF < 3 BF < 3 CF4 BeF < 2 OF < 2 NF < 3 BF < 3 CF
    • B. OF 4 CF 4 < 4 NF < 3 BeF < 2 OF 2 OF < 2 NF < 3 CF < 4 BF < 3 BeF 2
    Answer, explanation and textbook page: open in the app.
  23. 59.How many electrons are present in the $\sigma_{2p}$ molecular orbital of $\mathrm{N_2^+}$?
    • A. 2
    • B. 1
    • C. 3
    • D. 4
    Answer, explanation and textbook page: open in the app.
  24. 60.A solution of $\mathrm{NH_4Cl}$ made by dissolving $3.16\mathrm{g}$ $\mathrm{NH_4Cl}$ in $30.14\mathrm{g}$ $\mathrm{H_2O}$ has a density of $1.0272\mathrm{g\,cm^{-3}}$. What is the mole fraction of $\mathrm{NH_4Cl}$?
    • A. 0.9659
    • B. 0.21
    • C. 0.65
    • D. 0.0341
    Answer, explanation and textbook page: open in the app.
  25. 61.Which of the following is true regarding the solution formation process?
    • A. New coulombic attraction between the solute and solvent form in which the enthalpy change is ΔH < 0 exothermic ( )
    • B. Intermolecular forces between the solvent molecules must weaken in which the enthalpy change is exothermic ( ΔH < 0 )
    • C. Intermolecular forces between the solute particles must weaken in which the enthalpy change is exothermic ( ΔH < 0 )
    • D. Covalent bonds within the solute and solvent molecules must be broken
    Answer, explanation and textbook page: open in the app.
  26. 62.What volume of 1.40M solution is needed to react exactly with 10.0g of aluminium according of the following reaction?
    • A. 2.643ml
    • B. 264.3ml
    • C. 26.43ml
    • D. 2643ml
    Answer, explanation and textbook page: open in the app.
  27. 63.Which of the following statements is NOT true in relation to the triple point on a single component phase diagram?
    • A. The point at which the solid. Liquid and gaseous phases for a substance co-exist.
    • B. The triple point exists at a single temperature and is independent of pressure.
    • C. The system must be enclosed so that no Vapour can escape
    • D. The triple point exists for a substance occurs at a specific temperature and pressure.
    Answer, explanation and textbook page: open in the app.
  28. 64.Consider the following equilibrium: $\mathrm{Cl_2(g)} + 2\mathrm{NO(g)} \rightleftharpoons 2\mathrm{NOCl(g)}$ $K_{\mathrm{eq}} = 5.0$ At equilibrium, $[\mathrm{Cl_2}] = 1.0\mathrm{M}$ and $[\mathrm{NO}] = 2.0\mathrm{M}$. What is the $[\mathrm{NOCl}]$ at equilibrium?
    • A. 0.80M
    • B. 0.89
    • C. 10M
    • D. 4.5M
    Answer, explanation and textbook page: open in the app.
  29. 65.Which acid is produced when toluene is subjected to oxidation?
    • A. Phenyl acetic acid
    • B. Toluic acid
    • C. Benzoic acid
    • D. Phthalic acid
    Answer, explanation and textbook page: open in the app.
  30. 66.Calculate for the following reaction using the bond energies given below H - H(g) + I - I(g) 2H - I (g) bond energies: H - H = 436KJ/mol, I - I = 151KJ/mol, H - I = 297KJ/mol
    • A. -7KJ
    • B. -290KJ
    • C. +7KJ
    • D. +290KJ
    Answer, explanation and textbook page: open in the app.
  31. 67.How long has a current of 3 ampere to be applied through a solution of silver nitrate to coat a metal surface of 80cm2 10.5gcm−3 with 0.005cm thick layer? Density of silver =
    • A. 476s
    • B. 1252s
    • C. 683s
    • D. 1028s
    Answer, explanation and textbook page: open in the app.
  32. 68.Which of the following is an organic acid?
    • A. $\mathrm{CH_3CH_2OH}$
    • B. $\mathrm{CH_3CH_3}$
    • C. $\mathrm{CH_2 = CH_2}$
    • D. $\mathrm{CH_3CO_2H}$
    Answer, explanation and textbook page: open in the app.
  33. 69.During a titration what volume of 0.500M $\mathrm{KOH}$ is necessary to completely neutralize 10.0ml of 2.00M $\mathrm{CH_3COOH}$?
    • A. 10.0ml
    • B. 40.0ml
    • C. 25.0ml
    • D. 20.0ml
    Answer, explanation and textbook page: open in the app.
  34. 70.What is the standard cell potential of the oxidation of ammonia, given below?
    • A. 7.02V
    • B. 3.51V
    • C. 1.17V
    • D. 14.04V
    Answer, explanation and textbook page: open in the app.
  35. 71.Two electrolytic cells were placed in series, one of $\mathrm{AgNO_3}$ and the other of $\mathrm{CuSO_4}$. If 1.273g Ag is deposited, how much Cu was deposited, how much Cu was deposited at the same time?
    • A. 0.374
    • B. 0.0118
    • C. 0.748
    • D. 0.954
    Answer, explanation and textbook page: open in the app.
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