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7 November, 06:09

What mass of hydrogen sulfide, H2S1, will completely react with 2.00 moles of silver nitrate, AgNO3?

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  1. 7 November, 08:57
    0
    34g

    Explanation:

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

    H2S + 2AgNO3 - > 2HNO3 + Ag2S

    Next, we shall determine the number of mole of H2S required to react with 2 moles of AgNO3.

    This is illustrated below:

    From the balanced equation above,

    We can see that 1 mole of H2S is required to react completely with 2 moles of AgNO3.

    Finally, we shall convert 1 mole of H2S to grams. This is shown below:

    Number of mole H2S = 1 mole

    Molar mass of H2S = (2x1) + 32 = 34g/mol

    Mass = number of mole x molar Mass

    Mass of H2S = 1 x 34

    Mass of H2S = 34g

    Therefore, 34g of H2S is needed to react with 2 moles of AgNO3.
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