Grab a calculator and a copy of the periodic table

(This test has only 10 questions, but may take 15 - 20 mins).
1. Calculate the relative formula mass (Mr) of calcium hydroxide, Ca(OH)2.
  • A.   38
  • B.   58
  • C.   74
  • D.   114
2. Which of the following contains the greatest number of moles?
  • A.   2.4 g of carbon, C
  • B.   2.3 g of sodium, Na
  • C.   2.4 g of Magnesium, Mg
  • D.   3.9 g of potassium, K
3. A student required 0.15 moles of magnesium oxide, MgO, for a reaction. What mass of MgO should she weigh out? [Mr of MgO is 40]
  • A.   0.00375 g
  • B.   0.0060 g
  • C    6.0 g
  • D.   267 g
4. A student produced a sample of copper(II)sulfate crystals from copper(II)oxide and sulfuric acid. She calculated that she should obtain 18.6g of dry crystals but she only actually obtained 12.4g.

 

 copper sulfate crystals
Crystal Titan | CC 4.0

What was her percentage yield?

  • A.   1.5%
  • B.   150%
  • C.   0.67%
  • D.   67%
5. 60.0g of calcium carbonate decomposed on heating to form calcium oxide and carbon dioxide.   The equation for the reaction is:

                                            CaCO3 → CaO + CO2

What is the maximum mass of calcium oxide which could be formed in this reaction?
[Mr values: CaCO3 = 100; CaO = 56; CO2 = 44]

  • A.   26.4 g
  • B.   30.0 g
  • C.   33.6 g
  • D.   56.0 g
6. An oxide of iron, on reduction, was found to contain 1.12 g of iron and 0.32 g of oxygen.

Calculate the empirical formula of this iron oxide.  
[Relative atomic masses: Fe = 56; O=16]

  • A: FeO
  • B: Fe2O2
  • C: Fe2O
  • D: Fe2O3

7. A carbohydrate was found to have an empirical formula CH2O and a relative molecular mass of 120. The molecular formula of the carbohydrate is …

  • A.   CH2O
  • B.   C2H4O2
  • C.   C4H8O4
  • D.   C6H12O6
8. 1.38 g of sodium was burned in oxygen. An oxide of mass 2.34 g was formed.

Calculate the moles of sodium and oxygen atoms in the final product.
[Ar of Na = 23; Ar of O = 16]

  Moles of sodium atoms Moles of oxygen atoms
A 0.06 0.146
B 0.06 0.06
C 0.102 0.06
D 0.102 0.146

Q9-10: 34.0 kg of ammonia, NH3 is reacted with excess nitric acid, HNO3, to produce ammonium nitrate fertilizer. The equation for the reaction is:

NH3  + HNO3 → NH4NO3

 

fertilizer

Muibu88 | CC4.0 licence
9. Calculate the number of moles of ammonia, NH3, used in this reaction.

[Relative atomic masses H = 1; N = 14, O = 16]

  • A.   2.27
  • B.   2.00
  • C.   2267
  • D.   2000
10. Calculate the maximum mass, in kg, of ammonium nitrate formed [Mr of NH4NO3 is 80]
  • A.   181.6 kg
  • B.   160 kg
  • C.   181,600 kg
  • D.   160,000 kg