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5 February, 17:25

Q1.

In an experiment, ammonia gas is made by heating a mixture of ammonium chloride and calcium

hydroxide.

2NH4Cl (s) + Ca (OH) 2 (s) =

CaCl2 (s) + 2NH3 (g) + 2H2O (l)

10.0 g of ammonium chloride is added to an excess of calcium hydroxide.

Calculate the maximum volume of ammonia gas that could be formed.

(relative atomic mass H = 1.00, N = 14.0, 0 = 16.0 and Ca = 40.0; one mole of any gas occupies 24 dm

at room temperature and pressure)

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Answers (1)
  1. 5 February, 20:46
    0
    4.49dm3

    Explanation:

    2NH4Cl + Ca (OH) 2 - > CaCl2 + 2NH3 + 2H2O

    First, we need to convert 10g of ammonium chloride to mole. This is illustrated below:

    Molar Mass of NH4Cl = 14 + (4x1) + 35.5 = 53.5g/mol

    Mass of NH4Cl = 10g

    Number of mole = Mass / Molar Mass

    Number of mole of NH4Cl = 10/53.5 = 0.187mol

    From the equation,

    2moles of NH4Cl produced 2 moles of NH3.

    Therefore, 0.187mol of NH4Cl will also produce 0.187mol of NH3

    Now we can obtain the volume of NH3 produced by doing the following:

    1mole of any gas occupy 24dm3

    Therefore, 0.187mol of NH3 will occupy = 0.187 x 24 = 4.49dm3
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