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    Kc for the equilibrium below is 0.0036 at 2680K. If 1 mole of N2 and 1 mole of 02 are allowed to reach equilibrium at 2680K, what mass of NO will be present in the mixture? (you will need to solve a quadratic equation to answer this)

    N2 + O2 --> 2NO its a reversible reaction btw


    I'm trying to figure out what the quadratic could be but I just dont understand how to solve this at all. Please help?
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    (Original post by _s_ox)
    Kc for the equilibrium below is 0.0036 at 2680K. If 1 mole of N2 and 1 mole of 02 are allowed to reach equilibrium at 2680K, what mass of NO will be present in the mixture? (you will need to solve a quadratic equation to answer this)

    N2 + O2 --> 2NO its a reversible reaction btw


    I'm trying to figure out what the quadratic could be but I just dont understand how to solve this at all. Please help?
    Let the moles of nitrogen (for example) reacted at equilibrium be 'x'.
    Moles of nitrogen at equilibrium will be (1-x).
    Get all of the other components in terms of 'x' and substitute into the equilibrium law expression.
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    (Original post by charco)
    Let the moles of nitrogen (for example) reacted at equilibrium be 'x'.
    Moles of nitrogen at equilibrium will be (1-x).
    Get all of the other components in terms of 'x' and substitute into the equilibrium law expression.
    thank you so much! your reply was really helpful
 
 
 
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