Grab a calculator and a copy of the periodic table

(This test has only 10 questions, but may take 15 - 20 mins).

Q1-2:  A student used the following reaction to try to produce 20.0 g of copper(II)chloride.

CuCO3 + 2HCl → CuCl2  + H2O  + CO2

[Relative atomic masses Cl = 35.5; Cu = 63.5]

  

1. The formula mass of copper(II)chloride and the number of moles of copper(II)chloride produced is …

  Formula Mass Moles produced
A 99 4.95
B 99 0.202
C 134.5 6.73
D 134.5 0.149
2. What mass of copper(II)carbonate does the student need to react with excess hydrochloric acid to make the 20.0 g of copper(II)chloride? [Mr of CuCO3 = 123.5]
  • A.   18.4 g
  • B.   20.0 g
  • C.   24.9 g
  • D.   36.8 g
3. 2.54g of copper reacts with 0.32g of oxygen gas to produce copper oxide.

A possible balanced equation for this reaction is …… 
[Relative atomic masses: Cu = 63.5; O=16]

  • A. Cu   +   O  → CuO
  • B. 2Cu   +  O2  → 2CuO
  • C. 4Cu   +  O2  → 2Cu2O
  • D. 8Cu   +  O2  → 2Cu4O

4. In the thermite reaction aluminium powder reacts very exothermically with iron(III)oxide displacing molten iron. The equation for the reaction is: 

2Al + Fe2O3  → Al2O3 + 2Fe

What mass of molten iron is formed from 0.1moles of iron(III)oxide?
[Mr of Fe2O3 is 160; Ar of Fe is 56]

 thermite reaction
Author:Caesium Fluoride | CC 3.0
  • A.   2.8 g
  • B.   5.6 g
  • C.   11.2 g
  • D.   22.4 g
5. 100cm3 of a sodium hydroxide solution was prepared by dissolving 20g of sodium hydroxide, NaOH, in water.

What is the concentration of this solution in g/dm3?

  • A.   0.2 g/dm3
  • B.   5 g/dm3
  • C.   20 g/dm3
  • D.   200 g/dm3
6. How many CaCO3 particles are there in 2 moles of CaCO3?
  • A.   1.20 x 1023
  • B.   3.01 x 1023
  • C.   1.02 x 1024
  • D.   6.02 x 1024
7. What amount, in moles, is 3.0g of carbon and how many carbon atoms does it contain?

[Ar of carbon = 12]

  Number of moles of carbon Number of carbon atoms
A 0.25 1.51 x 1023
B 0.25 2.41 x 1024
C 4.0 1.51 x 1023
D 4.0 2.41 x 1024

 

8. A mass of 3.00 g of magnesium was reacted with 0.200 moles of ethanoic acid in the following reaction:

Mg + 2CH3COOH → (CH3COO)2Mg + H2

Calculate the number of moles of magnesium used and determine the reagent in excess.
  Number of moles of magnesium Reagent in excess
A 0.125 Ethanoic acid
B 0.125 magnesium
C 0.100 Ethanoic acid
D 0.100 magnesium
9. What is a limiting reactant?
  • A.   The reactant with the lowest molecular mass
  • B.   The reactant that is used in the smallest mass in the reaction
  • C.   The reactant that is all used up in the reaction
  • D.   The reactant that is left over at the end of a reaction
10. Iron(III)hydroxide is a brown precipitate formed during the test for iron(III) ions.

FeCl3 (aq)  + 3NaOH (aq)  → Fe(OH)3 (s)   +   3NaCl (aq)

What amount, in moles, of each reactant would be needed to produce 0.6 moles of iron(III)hydroxide?

  
  Moles of FeCl3 (aq) Moles of NaOH (aq)
A 0.2 0.6
B 0.3 0.3
C 0.6 0.6
D 0.6 1.8