19 Gold reacts with the elements in Group 7 of the periodic table. 0.175 g of gold reacts with chlorine. The equation for

Question

19
Gold reacts with the elements in Group 7 of the periodic table.
0.175 g of gold reacts with chlorine.
The equation for the reaction is:
2 Au + 3 Cl2 – 2 AuCla
Calculate the mass of chlorine needed to react with 0.175 g of gold.
Give your answer in mg
Relative atomic masses (Ar): Cl = 35.5 Au = 197

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Thu Hương 3 years 2021-07-16T01:59:27+00:00 1 Answers 1145 views -1

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  1. Verity
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    2021-07-16T02:00:37+00:00
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    Answer: The mass of chlorine gas required is 94.6 mg

    Explanation:

    The number of moles is defined as the ratio of the mass of a substance to its molar mass.

    The equation used is:

    \text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}} ……(1)

    Given mass of gold = 0.175 g

    Molar mass of gold = 197 g/mol

    Plugging values in equation 1:

    \text{Moles of gold}=\frac{0.175g}{197g/mol}=0.000888 mol

    The given chemical equation follows:

    2Au+3Cl_2\rightarrow 2AuCl_3

    By the stoichiometry of the reaction:

    If 2 moles of gold reacts with 3 moles of chlorine gas

    So, 0.000888 moles of gold will react with = of chlorine gas

    Molar mass of chlorine gas = 71 g/mol

    Plugging values in equation 1:

    \text{Mass of chlorine gas}=(0.001332mol\times 71g/mol)=0.0946g=94.6mg       (Conversion factor: 1 g = 1000 mg)

    Hence, the mass of chlorine gas required is 94.6 mg

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