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3 October, 12:51

Calculate the actual yield for the production of ammonia gas (nh3) from hydrogen and nitrogen gases if the percent yield is 68.2% and you begin with 2.00 kg of nitrogen gas

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  1. 3 October, 13:15
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    Percentage yield = (actual yield / theoretical yield) x 100%

    Hence,

    actual yield = percentage yield x theoretical yield / 100

    The balanced reaction equation for the production of ammonia is

    N₂ (g) + 3H₂ (g) → 2NH₃ (g)

    The mass of N₂ (g) used = 2.00 kg = 2 x 10³ g

    Molar mass of N₂ (g) = 28 g mol⁻¹

    moles (mol) = mass (g) / molar mass (g/mol)

    Hence, moles of N₂ (g) = 2 x 10³ g / 28 g mol⁻¹

    = 71.428 mol

    Stoichiometric ratio between N₂ (g) and NH₃ (g) is 1 : 2

    Hence, produced NH₃ (g) moles = 71.428 mol x 2

    = 142.856 mol

    Molar mass of NH₃ (g) = 17 g mol⁻¹

    mass of NH₃ (g) = 142.856 mol x 17 g mol⁻¹ = 2428.552 g

    Hence, the theoretical yield = 2428.552 g

    Then the actual yield of NH₃ (g) produced = (68.2 x 2428.552 g) / 100

    = 1656.27 g
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