Question

Given that you have 14.5 moles of n2, how many moles of h2 are theoretically needed to produce 30.0 moles of nh3 according to reaction below?

Answer 1

45 moles of H₂ are theoretically needed to produce 30.0 moles of NH₃

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).

The concentration of a substance can be expressed in several quantities such as moles, percent (%) weight/volume,), molarity, molality, parts per million (ppm) or mole fraction. The concentration shows the amount of solute in a unit of the amount of solvent.

• Mole

The mole itself is the number of particles contained in a substance amounting to 6.02.10²³

Mole can also be sought if the amount of substance mass and its molar mass is known

$\large{\boxed{\boxed{\bold{mol=\frac{mass}{molar\:mass}}}}$

 

Reaction that happens :

N₂ +3H₂ ⇒ 2NH₃

mole N₂ : H₂ : NH₃ = 1 : 3 : 2

To produce 30.0 moles of NH₃,

• H₂ needed :

$mole~H_2~=~\frac{3}{2}\times~30~mole$

mole H₂ = 45 mole

• N₂ needed :

$mole~N_2~=~\frac{1}{2}~\times~30$

mole N₂ = 15 mole

So the minimum N₂ needed is: 15 mole

14.5 moles of N₂ can only produce NH₃ :

$mole~NH_3~=~\frac{2}{1}~\times~14.5$

mole NH₃ = 29 mole

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Keywords: mole,  NH₃, N₂, H₂

Answer 2

$\boxed{45 \text{mol}}$ of $\text{H}_2$ are theoretically needed to produce 30.0 moles of  .

Further Explanation:

Stoichiometry is used to describe quantitative relationship between reactants and products. In stoichiometric problems, amount of one of the species involved in the reaction can be calculated with the help of known amounts of other species in the same reaction.

Consider a reaction of the general form as follows:

$\text{X}+2\text{Y}\rightarrow3\text{Z}$

Where,

X and Y are reactants of reaction.

Z is the product of reaction.

The stoichiometry of this reaction indicates that one mole of X can react with two moles of Y and three moles of Z are produced.

The balanced chemical reaction for the formation of   is as follows:

$\text{N}_2+3\text{H}_2\rightarrow2\text{NH}_3$

According to balanced chemical reaction, one mole of $\text{N}_2$ reacts with three moles of  $\text{H}_2$ to form two moles of  $\text{NH}_3$. So stoichiometric ratio between  $\text{H}_2$ and $\text{NH}_3$  is 3:2.

Since three moles of hydrogen produce two moles of $\text{NH}_3$, moles of $\text{H}_2$ that are required to form 30.0 moles of $\text{NH}_3$ can be calculated as follows:

$\begin{aligned}\text{Moles of H}_2=&\left ({\dfrac{\text{3 Mol of H}_2}{\text{2 Mol of NH}_3} \right )\left(30\text{mol of NH}_3\right)\\=& 45.0\text{ mol of H}_2\end{aligned}$

Hence 45.0 moles of $\text{H}_2$ are required to produce 30.0 moles of $\text{NH}_3$ .

Learn more:

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Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Mole concept

Keywords: NH3, 45 mol, H2, N2, stoichiometry, balanced chemical reaction, one mole, two moles, three moles, X, Y, Z, 2Y, 3Z, 3H2, 2NH3, quantitative relationship.