10.00 g of O2 reacts with 20.00 g NO Determine the amount of NO2, limiting reactant, and the excess reactant.

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10.00 g of O2 reacts with 20.00 g NO Determine the amount of NO2, limiting reactant, and the excess reactant.

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Tryphena 2 months 2021-09-01T07:49:29+00:00 1 Answers 0 views 0

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    2021-09-01T07:50:34+00:00

    Answer:

    Limiting reactant: O₂

    Excess reactant: NO

    Amount of NO₂ produced: 28.75 g

    Explanation:

    The balanced equation for the reaction between O₂ and NO to produce NO₂ is the following:

    O₂(g) + 2NO(g) → 2NO₂(g)

    According to the equation, 1 mol of O₂ reacts with 2 moles of NO to produce 2 moles of NO₂.

    We first convert the moles of each compound to mass by using the molecular weight (MW):

    MW(O₂) = 16 g/mol x 2 = 32 g/mol

    ⇒ mass O₂ = 1 mol O₂ x 32 g/mol O₂ = 32 g

    MW(NO) = 14 g/mol + 16 g/mol = 30 g/mol

    ⇒ mass NO = 2 mol NO x 30 g/mol NO = 60 g

    MW(NO₂) = 14 g/mol + (2x 16 g/mol) = 46 g/mol

    ⇒ mass NO = 2 mol NO₂ x 46 g/mol NO₂ = 92 g

    For the reactants, the stoichiometric ratio is 32 g O₂/60 g NO. Thus, the mass of O₂ required to completely react with 20.00 g of NO is:

    mass of O₂ required = 20.00 g NO x 32 g O₂/60 g NO = 10.67 g O₂

    We need 10.67 g of O₂ and we have only 10.00 g, so the limiting reactant is O₂. Thus, the excess reactant is NO.

    With the limiting reactant, we calculate the amount of product produced (NO₂). For this, we consider the stoichiometric ratio 92 g NO₂/32 g O₂:

    mass of NO₂ produced = 10.00 g O₂ x 92 g NO₂/32 g O₂ = 28.75 g NO₂

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