IBSL Chemistry Multiple Choice Topic 1 Quantitative Chemistry

21 Questions | Total Attempts: 264

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IBSL Chemistry Quizzes & Trivia

Questions and Answers
  • 1. 
    Which sample has the greatest mass?
    • A. 

      1.0 mol of N2H4

    • B. 

      2.0 mol of N2

    • C. 

      3.0 mol of NH3

    • D. 

      25.0 mol of H2

  • 2. 
    What is the mass in grams of one molecule of propanol, C3H7OH? (Avogadro's constant 6.0 x 1023 /mol)
    • A. 

      60

    • B. 

      1.0 x 10^-22

    • C. 

      1.0 x 10^-23

    • D. 

      3.6 x 10^25

  • 3. 
    Chloroethene, C2H3Cl reacts with oxygen according to the equation below:   2C2H3Cl + 5O2 --> 4CO2 + 2H2O +2HCl   How many moles of CO2 are produced when 3.0 mol of C2H3Cl and 3.0 mol of O2 are reacted?
    • A. 

      2.4

    • B. 

      3.0

    • C. 

      4.0

    • D. 

      6.0

  • 4. 
    How many molecules are there in 180 g of H2O?
    • A. 

      6.0 x 10^22

    • B. 

      6.0 x 10^23

    • C. 

      6.0x 10^24

    • D. 

      6.0 x 10^21

  • 5. 
    How many moles of CH4 are needed to obtain 6.0 x 1023 hydrogen atoms?
    • A. 

      1/4

    • B. 

      1

    • C. 

      2

    • D. 

      4

  • 6. 
    What is the minimum number of grams of O2 (MR= 32) required to burn 1.6g of CH4 (MR= 16) according to the equation below?   CH4 +2O2 -> CO2 +2H20
    • A. 

      1.6

    • B. 

      3.2

    • C. 

      6.4

    • D. 

      32

  • 7. 
    The number of moles in 500 g of water is approximately:
    • A. 

      28

    • B. 

      9000

    • C. 

      1 x10^25

    • D. 

      3x 10^26

  • 8. 
    Hydrogen sulfide, H2S, reacts with oxygen to form sulfur dioxide and water as shown below: 2H2S + _O2 --> _SO2 + _H20 What is the whole number coefficient for oxygen when this equation is balanced?
    • A. 

      1

    • B. 

      2

    • C. 

      3

    • D. 

      6

  • 9. 
    vC2H3Cl(g) + w02 (g) à xCO2 (g) + yH20(g) + zHCI(g) Chloroethene can be burned in oxygen as shown above. What is the value of w when v = 2 ?
    • A. 

      2

    • B. 

      3

    • C. 

      4

    • D. 

      5

  • 10. 
    Arsenic, As4, reacts with oxygen to produce the oxide As4010. What is the sum of the coefficients for the reactants in the balanced equation? __As4  +  __O2 à __As4010
    • A. 

      5

    • B. 

      6

    • C. 

      7

    • D. 

      8

  • 11. 
    One stage in the manufacture of nitric acid is the oxidation of ammonia as shown below: 4NH3 +__O2 →__ NO +__H2O   What is the coefficient for O2 when the equation is balanced?
    • A. 

      3

    • B. 

      4

    • C. 

      5

    • D. 

      6

  • 12. 
    PbS(s) + O2 (g) → PbO(s) + SO2 (g)   The reaction of lead(II) sulfide with oxygen is represented by the unbalanced equation above.  What is the sum of the coefficients in the balanced equation?
    • A. 

      4

    • B. 

      5

    • C. 

      8

    • D. 

      9

  • 13. 
    8.0 g of a pure compound contains 3.2 g of sulfur and 4.8 g of oxygen. What is its empirical formula?
    • A. 

      SO

    • B. 

      SO2

    • C. 

      SO3

    • D. 

      S2O3

  • 14. 
    How many carbon atoms are present in 0.10 mol of ethanoic acid, CH 3COOH ?
    • A. 

      6.0 ×10^22

    • B. 

      1.2 ×10^23

    • C. 

      6.0 ×10^23

    • D. 

      1.2 ×10^24

  • 15. 
     Zn(s) + Cu2+ (aq) → Zn2+(aq) + Cu(s) Powdered zinc reacts with Cu2+ ions according to the equation above.  What will be the result of adding 3.25 g of Zn to 100 cm3 of 0.25 mol dm−3 CuSO4 solution
    • A. 

      All the Cu2+ ions react and some solid zinc remains.

    • B. 

      All the Cu2+ ions react and no solid zinc remains.

    • C. 

      All the solid zinc reacts and Cu2+ ions remain.

    • D. 

      Neither solid zinc nor Cu2+ ions remain.

  • 16. 
    Which sample contains the greatest number of ions?
    • A. 

      25 cm3 of 0.40 mol dm−3 NaCl

    • B. 

      50 cm3 of 0.20 mol dm−3 MgCl2

    • C. 

      100 cm3 of 0.10 mol dm−3 KNO3

    • D. 

      200 cm3 of 0.05 mol dm-3 CuSO4

  • 17. 
    Which sample has the greatest mass?
    • A. 

      1.0 mol of H2S

    • B. 

      2.0 mol of OH−

    • C. 

      1.0 mol of H2O2

    • D. 

      2.0 mol of NH4+

  • 18. 
    A hydrocarbon contains 80 % by mass of carbon.  What is its empirical formula?
    • A. 

      CH

    • B. 

      CH2

    • C. 

      CH3

    • D. 

      CH4

  • 19. 
    Methanol can undergo complete combustion in air as shown below: 2CH 3OH + ____O2 → ____CO2 + ____H2O               What is the coefficient for O2 when the equation is balanced?
    • A. 

      1

    • B. 

      2

    • C. 

      3

    • D. 

      4

  • 20. 
    How many hydrogen atoms are contained in one mole of ethanol, C2 H5OH?
    • A. 

      5

    • B. 

      6

    • C. 

      1.0x10^23

    • D. 

      3.6×10^24

  • 21. 
    The percentage by mass of the elements in a compound is C=72%, H=12%, O=16%. What is the mole ratio of C : H in the empirical formula of this compound?
    • A. 

      1 : 1

    • B. 

      1 : 2

    • C. 

      1 : 6

    • D. 

      6 : 1

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