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12 April, 02:02

Magnesium nitride is formed in the reaction of magnesium metal and nitrogen gas. 4.0 mol of nitrogen is reacted with 6.0 mol of magnesium. The result is ...

a. 2.0 mol of magnesium nitride and 2.0 mol excess nitrogen

b. 4.0 mol of magnesium nitride and 2.0 mol excess magnesium

c. 6.0 mol of magnesium nitride and 3.0 mol excess nitrogen

d. No product because the reactants are not in the correct mole ratio

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  1. 12 April, 02:22
    0
    The correct answer is A

    We'll have 2.0 moles of magnesium nitride produced and and excess of 2.0 moles nitrogen gas

    Explanation:

    Step 1: Data given

    Number of moles nitrogen gas (N2) = 4.0 moles

    Number of moles magnesium = 6.0 moles

    Step 2: The balanced equation

    3Mg + N2 → Mg3N2

    Step 3: Calculate the limiting reactant

    For 3 molesmagnesium (Mg) we need 1 mol nitrogen gas (N2) to react, to produce 1 mol magnesium nitride (Mg3N2)

    Magnesium is the limiting reactant. It will completely be consumed 6.0 moles. Nitrogen is in excess. There will react 6.0 / 3 = 2.0 moles

    There will remain 4.0 - 2.0 = 2.0 moles N2

    Step4: Calculate moles Mg3N2

    For 3 molesmagnesium (Mg) we need 1 mol nitrogen gas (N2) to react, to produce 1 mol magnesium nitride (Mg3N2)

    For 6.0 moles Mg we'll have 6.0 / 3 = 2.0 moles Mg3N2

    The correct answer is A

    We'll have 2.0 moles of magnesium nitride produced and and excess of 2.0 moles nitrogen gas
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