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26 May, 08:13

How many grams of NaCl was used by the electrolysis method to obtain 74L of chlorine gas at a temperature of 27 degrees C at 1 atm?

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  1. 26 May, 10:56
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    351g

    Explanation:

    The following were obtained from the question:

    Volume (V) of Cl2 = 74L

    Temperature (T) = 27°C = 27°C + 273 = 300K

    Pressure (P) = 1 atm

    To obtain the mass of NaCl used in the reaction, we need to determine the number of mole Cl2 produced from the reaction. This is illustrated below:

    Using the ideal gas equation, the number of mole of Cl2 can be obtained as follow:

    Volume (V) of Cl2 = 74L

    Temperature (T) = 300K

    Pressure (P) = 1 atm

    Gas constant (R) = 0.082atm. L/Kmol

    Number of mole (n) of Cl2 = ?

    PV = nRT

    n = PV / RT

    n = (1 x 74) / (0.082 x 300)

    n = 3 moles

    Therefore, the reaction produced 3 moles of Cl2.

    Next, the balanced equation for the reaction. This is given below:

    2NaCl - > 2Na + Cl2

    From the balanced equation above,

    2 moles of NaCl produced 1 mole of Cl2.

    Therefore, Xmol of NaCl will produce 3 moles of Cl2 i. e

    Xmol of NaCl = 2 x 3

    Xmol of NaCl = 6 moles

    Therefore, 6 moles of NaCl was used in the reaction.

    Next, we shall convert 6 mole of NaCl to grams. This is illustrated below:

    Number of mole NaCl = 6 moles

    Molar Mass of navl = 23 + 35.5 = 58.5g/mol

    Mass of NaCl = ?

    Mass = number of mole x molar Mass

    Mass of NaCl = 6 x 58.5

    Mass of NaCl = 351g

    From the calculations made above, 351g of NaCl was used in the electrolysis.
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