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22 November, 05:45

Ammonium nitrite undergoes decomposition to produce only gases as shown below. nh4no2 (s) → n2 (g) + 2h2o (g) how many liters of gas will be produced by the decomposition of 32.0 g of nh4no2 at 525°c and 1.5 atm?

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  1. 22 November, 09:35
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    From the given balanced reaction equation:

    we can see that every 1 mole of NH4NO2 will produce 1 mole of N2 and when the water also on the gas phase so, every 1 mole of NH4NO2 will produce 3 moles of gas

    now we need to get number of moles of NH4NO2 = mass/molar mass

    when the mass = 32 g and the molar mass of NH4NO2 = 64 mol/g

    ∴moles of NH4NO2 = 32 g / 64 mol/g = 0.5 mole

    so, the moles that produced of gas will be = 3 * 0.5 = 1.5 moles

    now, we can use the ideal gas formula to get V:

    PV = nRT

    when P is the pressure = 1.5 atm

    n is the number of moles = 1.5 moles

    R is the ideal gas constant = 0.0821 L*atm/mol*K

    and T is the temperature in Kelvin = 525 °C + 273 = 798 K

    so by substitution:

    1.5 atm * V = 1.5 moles * 0.0821 * 798 K

    ∴ V = 65.5 L
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