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3 years ago

Write a balanced chemical equation for the standard formation reaction of gaseous dinitrogen tetroxide n2o4 .

Chemistry

2 answers:

mixer [17]3 years ago

7 0

Answer and explanation;

-Dinitrogen tetroxide is a dimer and a colorless toxic gas which results from the reaction between two nitrogen dioxide molecules (NO2) a process called dimerization.

-The Dimerization process occurs readily when there is high concentration of mixtures of NO2 or when NO2 condenses on surfaces or at very low temperatures.

The reaction is;

2 NO2(g) → N2O4 (g)

eduard3 years ago

3 0

Answer: 3 N2H4 (l) = 4 NH3 (g)+ N2 (g) 2 N2H4 (l) + N2O4 (g) =3 N2 (g)+ 4 H2O (g)

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2 years ago

Be sure to answer all parts. Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark brown gas: 2NO(g) +

notka56 [123]

Answer: NO is the limiting reagent in the given reaction and 0.857 moles of $NO_2$ will be produced.

Explanation:

Limiting reagent is defined as the reagent which is present in less amount and it limits the formation of products.

Excess reagent is defined as the reagent which is present in large amount.

For the given chemical reaction:

$2NO(g)+O_2(g)\rightarrow 2NO_2(g)$

We are given:

Moles of NO = 0.857 mol

Moles of oxygen = 0.498 mol

By stoichiometry of the reaction:

If 2 moles of NO reacts with 1 mole of oxygen gas.

So, 0.857 moles of NO will react with = $\frac{1}{2}\times 0.857=0.4285mol$ of $O_2$

As, the given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, NO is considered as the limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

If 2 moles of NO produces 2 moles of nitrogen dioxide gas.

So, 0.857 moles of NO will produce = $\frac{2}{2}\times 0.857=0.857mol$ of $NO_2$

Hence, NO is the limiting reagent in the given reaction and 0.857 moles of $NO_2$ will be produced.

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3 years ago

What are diatomic molecules and are they compounds? PLEASE ANSWER ASAP!!

Fantom [35]

Answer:

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hope this helps :)

Explanation:

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2 years ago