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The decomposition of dinitrogen pentoxide is described by the reaction: 2N2O5(g)→4NO2(g)+O2(g). If O2 is being formed at a rate of 2.40 mol/min, what is the rate at which N2O5 is being used up?

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rspill6

Answer:

4.80 mol N2O5/min

Explanation:

The balanced equation tells us that 2 moles of N2O5 are required for every 1 mole of O2.  Therefore:

(2.40 mol O2/min)*(2 mol N2O5/mol O2) = 4.80 mol N2O5/min

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