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17 June, 21:36

What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N2 gas when the ammonium nitrite in 1.00 L of 0.500 M NH4NO2 decomposes at 25.0°C?

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  1. 17 June, 21:57
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    First, let's find the number of moles of ammonium nitrite.

    0.5 mol/L * 1.10 L = 0.6 mol

    The decomposition reaction is

    NH₄NO₂ → N₂ + 2 H₂O

    Let's calculate the amount of N₂ gas produced.

    0.6 mol * 1 mol N₂/1 mol NH₄NO₂ = 0.6 mol N₂

    Then, let's compute P through the ideal gas equation:

    P = nRT/V

    P = (0.6) (0.0821 L-atm/mol-K) (25+273 K) / 10 L

    P = 1.47 atm
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