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10 March, 13:03

For the reaction: N2O5 (g) / longrightarrow& longrightarrow; 2NO2 (g) + 1/2O2 (g)

If N2O5 is decomposing with an instantaneous rate of 7.81 mol/L·s, what is the instantaneous rate of formation of NO2?

I don't know where to begin

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  1. 10 March, 16:31
    0
    The given equation from the problem above is already balance,

    N2O5 - - - > 2NO2 + 0.5O2

    Since, in every mole of N2O5 consumed, 2 moles of NO2 are formed, we can answer the problem by multiplying the given rate, 7.81 mol/L. s with the ratio.

    (7.81 mol/L. s) x (2 moles NO2 formed / 1 mole of N2O5 consumed)

    = 15.62 mol/L. s

    The answer is the rate of formation of NO2 is approximately 15.62 mol/L. s.
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