Question #01ad7

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Question #01ad7

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Answer 1 · 2017-08-24T14:46:48

$N_{2} + O_{2} \to 2 N O$ $N_2 + O_2 -> 2NO$

Explanation:

$N_{2} O$ $N_2O$ can only be made from $2 N_{2} + O_{2} \to 2 N_{2} O$ $2N_2 + O_2 -> 2N_2O$ . Nitrogen and Oxygen can form many compounds but with specific(and slightly confusing) requirements!

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Answer 2 · 2017-08-24T17:42:57

$N_{2} + O_{2} \to N_{2} O$ $N_2+O_2→N_2O$ unbalanced

We count the number of same atoms on each side. If there are different numbers of same atoms, we put coefficients in front to make them equal on both sides.
In the equation given,

Reactant(left)
$N = 2$ $N= 2$
$O = 2$ $O=2$

Product(right)
$N = 2$ $N= 2$
$O = 1$ $O=1$
we have same number of nitrogens, but not oxygens. Therefore, we put $\frac{1}{2}$ $1/2$ in front of oxygen on the reactant side
$N_{2} + \frac{1}{2} O_{2} \to N_{2} O$ $N_2+1/2O_2 →N_2O$ balanced

count the number of atoms now

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Question #01ad7

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