Nitric oxide (NO) reacts with oxygen gas to produce nitrogen dioxide. A gaseous mixture contains 0.66 g of nitric oxide and 0.58 g of oxygen

Question

Nitric oxide (NO) reacts with oxygen gas to produce nitrogen dioxide. A gaseous mixture contains 0.66 g of nitric oxide and 0.58 g of oxygen gas. After the reaction is complete, what mass of nitrogen dioxide is formed? Which reactant is in excess? How do you know? Suppose you actually recovered 0.91 g of nitrogen dioxide. What is your percent yield?

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Ngọc Khuê 4 years 2021-09-05T03:04:22+00:00 1 Answers 36 views 0

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  1. ThanhThu
    0
    2021-09-05T03:06:00+00:00
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    Answer:

    NO is the limiting reagent.  

    In this reaction 0.886 mole of NO2 is produced

    Explanation:

    The chemical equation for this reaction is  

    2NO(g) + O2(g) → 2NO2(g)

    In this limiting reagent reaction, 2 moles of NO reacts with one mole of O2  to produce 2 mole of 2NO2

    0.886 mole of NO * (2 mole of NO2/2 mole of NO) = 0.886 mole of NO2

    0.503 mole of O2 * (1 mole of NO2/1 mole of O2) = 1.01 mole of NO2

    Hence, NO is the limiting reagent.  

    In this reaction 0.886 mole of NO2 is produced

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