Question

For the reaction shown, calculate how many moles of NO2 form when each amount of reactant completely reacts.
2N2O5(g)→4NO2(g)+O2(g)

1.2 molN2O5

Answer 1

Answer:-  2.4 mol $NO_2$ .

Solution:- It asks to calculate the moles of $NO_2$ formed when 1.2 moles of $N_2O_5$ are reacted.

There is 2:4 mol ratio between $N_2O_5$ and $NO_2$ . So, the moles of reactant are multiplied by the mol ratio to get the moles of $NO_2$ . The calculations are shown below:

$1.2mol N_2O_5(\frac{4mol NO_2}{2mol N_2O_5})$

= 2.4 mol $NO_2$

So, 2.4 moles of $NO_2$ are formed when 1.2 moles of  $N_2O_5$ were reacted.

Answer 2

Moles of NO₂ : 2.4

Further explanation

Stoichiometry in Chemistry learn about chemicals mainly emphasizes quantitative, such as the calculation of volume, mass, number, which is related to numbers, molecules, elements, etc.

A reaction coefficient is a number in the chemical formula of a substance involved in the reaction equation. The reaction coefficient is useful for equalizing reagents and products.

In the reaction there are also manifestations of reagent substances namely gas (g), liquid (liquid / l), solid (solid / s) and solution (aqueous / aq).

Reactions that occur:

2N₂O₅(g)→4NO₂(g)+O₂(g)

From the reaction equation above, the reaction coefficient shows the mole ratio of reagents and products

mol N₂O₅: mol NO₂ = 2: 4

So if there is 1.2 mol N₂O₅  , then

$\rm mol\:NO_2=\dfrac{4}{2}\times 1.2\\\\mol\:NO_2=2.4\:mol$

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