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# Calculations based on reactions - Test

1.

What mass of magnesium will produce 0.1g of hydrogen? The balanced equation is: Mg(s) + H2SO4(aq) → MgSO4 (aq) + H2(g)

2.

What mass of carbon dioxide is produced when 30.9g of copper carbonate is reacted with excess hydrochloric acid? The balanced equation is:

CuCO3 + 2HCl(aq) → CuCl2(aq) + CO2(g) + H2O(l)

3.

What mass of water is produced when 18.4g of ethanol (C2H5OH) is burned in excess oxygen? The balanced equation is:

C2H5OH(l) + 3O2(g) → 3H2O(l) + 2CO2(g)

4.

What mass of hydrogen was used to produce 3.4g of ammonia when hydrogen and nitrogen react together? The balanced equation is:

N2(g) + 3H2(g) → 2NH3(g)

5.

30cm3 of 1.5 mol/l hydrochloric acid was required to neutralise 30cm3 of potassium hydroxide. What is the concentration of the potassium hydroxide?HCl(aq) + KOH(aq) ? KCl(aq) + H2O(l)

6.

What volume of 1 mol/l sulphuric acid is required to neutralise 25 cm3 of 2 mol/l barium hydroxide? H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)

7.

7cm3 of 2.2 mol/l sulphuric acid was neutralised by sodium hydroxide (concentration 2 mol/l). What is the volume of sodium hydroxide used? H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l)

8.

A 2 mol/l nitric acid solution is titrated against 50cm3 of 1 mol/l lithium hydroxide. What volume of nitric acid was used? HNO3(aq) + LiOH(aq) ? LiNO3(aq) + H2O(l)

9.

4cm3 of phosphoric acid exactly neutralises 30cm3 of 0.1 mol/l calcium hydroxide. What is the concentration of the phosphoric acid? 2H3PO4(aq) + 3Ca(OH)2(aq) → Ca3(PO4)2 (s) + 6H2O(l)