How many moles of nitrogen dioxide are produced from 4.754 mol NO? Given the equation: NO(g) + O2(g) --> NO2(g).

Answer 1

#NO(g) + 1/2O_2(g) rarr NO_2(g)#

Since masses are conserved in all chemical reactions, the reaction described above is stoichiometric, which means that there is a corresponding reactant particle for each product particle.

Now of course I cannot have 1/2 an oxygen molecule, but I can certainly have 16 g of oxygen, which represents 1/2 a mole (i.e. Avogadro's number) of oxygen, #O_2#, molecules.

Given the stoichiometry, 1 mole of nitrous oxide, #NO#, combines with stoichiometic oxygen, to give stoichiometric nitric oxide, #NO_2#. So there is a 1:1 equivalence between nitrous oxide and its oxidation product.

I believe the answer is fairly obvious: given the 1:1 stoichiometry and 4.754 moles of nitrous oxide at the beginning, how many moles of nitric oxide will you finish with given adequate oxygen gas?

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Answer 2

Olivia Anton

The balanced equation indicates that one mole of NO reacts with one mole of O2 to produce two moles of NO2. Therefore, if 4.754 moles of NO are reacted, the moles of NO2 produced would be twice that amount, which is 9.508 moles.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

How many moles of nitrogen dioxide are produced from 4.754 mol NO? Given the equation: NO(g) + O2(g) --&gt; NO2(g).

How many moles of nitrogen dioxide are produced from 4.754 mol NO? Given the equation: NO(g) + O2(g) --> NO2(g).