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28 May, 18:36

Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the equation: 4NH3 + 5O2 → 4NO + 6H2O What mass of O2 would be required to react completely with 6.87 g of NH3?

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  1. 28 May, 20:54
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    16.16g of O2.

    Explanation:

    We'll begin by writing the balanced equation for the reaction. This is illustrated below:

    4NH3 + 5O2 → 4NO + 6H2O

    Next, we shall determine the mass of NH3 and O2 that reacted from the balanced equation. This is illustrated below:

    Molar mass of NH3 = 14 + (3x1) = 17g/mol

    Mass of NH3 from the balanced equation = 4 x 17 = 68g

    Molar Mass of O2 = 16x2 = 32g/mol

    Mass of O2 from the balanced equation = 5 x 32 = 160g.

    From the balanced equation above,

    68g of NH3 reacted with 160g of O2.

    Now, we can calculate the mass of O2 that will be required to react completely with 6.87 g of NH3. This is illustrated below:

    From the balanced equation above,

    68g of NH3 reacted with 160g of O2

    Therefore, 6.87g of NH3 will react with = (6.87 x 160) / 68 = 16.16g of O2.

    Therefore, 16.16g of O2 is needed for the reaction.
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