All categories

3 years ago

Based on the following chemical equation how many hydrogen atoms are present in the products side?

Chemistry

1 answer:

OleMash [197]3 years ago

7 0

The number of Hydrogen atoms = 6 atoms

<h3>Further explanation</h3>

Given

Reaction

N₂ + 3H₂ ⇒ 2NH₃

Required

The number of Hydrogen atoms

Solution

The reaction coefficient of a chemical equation shows the mole ratio of the reacting compound.

On a compound the reaction coefficient indicates the number of molecules

Whereas the subscript after the atom shows the number of atoms in that compound

Product from the reaction : 2NH₃

Number of H-atoms :

= 2 x 3

= 6 atoms

You might be interested in

Why are relative atomic masses on the periodic tables not whole numbers?

Kobotan [32]

Answer:

They are averages.

Explanation:

atomic numbers on periodic tables are derived from the average value of all the isotopes of the element. So being averages they are sometimes not integers.

6 0

3 years ago

Read 2 more answers

A student carries out a chemical reaction that produces a brown powder. How should the student measure the amount of product for

adoni [48]

The mass of the solid product of the reaction is determined by weighing.

6 0

4 years ago

Read 2 more answers

How many moles of methane (CH4) could be made from 4.6 moles of hydrogen?

DENIUS [597]

Answer:

Number of moles of methane form = 2.3 mol

Explanation:

Given data:

Number of moles of Hydrogen = 4.6 mol

Number of moles of methane form = ?

Solution:

Chemical equation:

C + 2H₂ → CH₄

Now we will compare the moles of methane with hydrogen from balance chemical equation.

H₂ : CH₄

2 : 1

4.6 : 1/2×4.6 = 2.3 mol

Form 3.6 moles of hydrogen 2.3 moles of methane can be formed.

6 0

3 years ago

The number of electrons in the outermost principal energy level of a chlorine atom is

Hitman42 [59]

Answer:

seven electrons

Explanation:

Chlorine is present in group seventeen of periodic table. It is halogen element. All halogens have seven electrons in outer most valance shell.

The require only one electron to gain the stable electronic configuration or to complete the octet.

Electronic configuration of chlorine:

Cl₁₇ = 1s² 2s² 2p⁶ 3s² 3p⁵

Abbreviated electronic configuration:

Cl₁₇ = [Ne] 3s² 3p⁵

Properties of chlorine:

1. it is greenish-yellow irritating gas.

2. its melting point is 172.2 K

3. its boiling point is 238.6 K

4. it is disinfectant and can kill the bacteria.

5. it is also used in manufacturing of paper, paints and textile industries.

5 0

3 years ago

When 125 grams of FeO react with 25.0 grams of Al, how many grams of Fe can be produced? FeO + Al → Fe + Al2O3 25.9 g Fe 38.7 g

Serga [27]

<u>Answer:</u> The mass of iron produced will be 77.6 grams

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

<u>For FeO:</u>

Given mass of FeO = 125 g

Molar mass of FeO = 71.8 g/mol

Putting values in equation 1, we get:

$\text{Moles of FeO}=\frac{125g}{71.8g/mol}=1.74mol$

<u>For aluminium:</u>

Given mass of aluminium = 25.0 g

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

$\text{Moles of aluminium}=\frac{25.0g}{27g/mol}=0.93mol$

The given chemical reaction follows:

$3FeO+2Al\rightarrow 3Fe+Al_2O_3$

By Stoichiometry of the reaction:

2 moles of aluminium metal reacts with 3 mole of FeO

So, 0.93 moles of aluminium metal will react with = $\frac{3}{2}\times 0.93=1.395mol$ of FeO

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

Thus, aluminium metal is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of aluminium metal produces 3 mole of iron metal

So, 0.93 moles of aluminium metal will produce = $\frac{3}{2}\times 0.93=1.395moles$ of iron metal

Now, calculating the mass of iron metal from equation 1, we get:

Molar mass of iron = 55.85 g/mol

Moles of iron = 1.395 moles

Putting values in equation 1, we get:

$1.395mol=\frac{\text{Mass of iron}}{55.85g/mol}\\\\\text{Mass of iron}=(1.395mol\times 55.85g/mol)=77.6g$

Hence, the mass of iron produced will be 77.6 grams

4 0

4 years ago