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    Decomposition of NaHCO3

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    At 125°C, Kp = 0.25 for the following reaction.
    2 NaHCO3(s)<---> Na2CO3(s) + CO2(g) + H2O(g)

    A 1.00 L flask containing 11.1 g NaHCO3 is evacuated and heated to 125°C.
    (a) Calculate the partial pressures of CO2 and H2O after equilibrium is established.
    PCO2
    atm
    PH2O
    atm

    (b) Calculate the masses of NaHCO3 and Na2CO3 present at equilibrium.
    Na2CO3
    g
    NaHCO3 reacted.
    g
    NaHCO3 remaining.
    g

    (c) Calculate the minimum container volume necessary for all the NaHCO3 to decompose.
    L

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    Solution Preview

    Chemical Equilibrium and partial pressure
    At 125°C, Kp = 0.25 for the following reaction.
    2 NaHCO3(s)<---> Na2CO3(s) + CO2(g) + H2O(g)

    A 1.00 L flask containing 11.1 g NaHCO3 is evacuated and heated to 125°C.
    (a) Calculate the partial pressures of CO2 and H2O after equilibrium is established.

    First you can write an equilibrium expression with the products on top and reactants on bottom. You can ...

    Solution Summary

    This solution explains how to calculate the equilibrium pressures of CO2 and H2O during the decomposition of NaHCO3.

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