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Lemur [1.5K]
3 years ago
12

How many elements of unsaturation are implied by the molecular formula c6h12?

Chemistry
2 answers:
Dmitriy789 [7]3 years ago
6 0
(2C+2-H-X+N)/2
(2*6+2-12-0+0)/2
1 UNSATURATION

Temka [501]3 years ago
4 0

There is \boxed{{\text{one}}} element of unsaturation that is implied by the molecular formula {{\text{C}}_{\text{6}}}{{\text{H}}_{{\text{12}}}}.

Further Explanation:

Hydrocarbons are organic compounds that are composed of hydrogen and carbon only. Aromatic hydrocarbons, alkanes, cycloalkanes are different types of hydrocarbons.

Types of hydrocarbons:

1. Saturated hydrocarbons

These are the simplest type of hydrocarbons. These are composed of only single bonds and therefore called saturated hydrocarbons. The general formula of saturated hydrocarbons is {{\text{C}}_n}{{\text{H}}_{2n + 2}}, where <em>n</em> is the number of carbon atoms. Methane, butane, hexane, and propane are some examples of saturated hydrocarbons.

2. Unsaturated hydrocarbons

These have one or more multiple bonds in them. Hydrocarbons consisting of double bonds are called alkenes while those comprising of triple bonds are called alkynes. The general formula for alkenes is {{\text{C}}_n}{{\text{H}}_{2n}}, while that of alkynes is {{\text{C}}_n}{{\text{H}}_{2n - 2}}, where<em> n</em> is the number of carbon atoms.

The formula to calculate the element of unsaturation is as follows:

{\text{Element of unsaturation}}=\dfrac{{\left( {2{\text{C}} + {\text{2}} - {\text{H}} - {\text{X}} + {\text{N}}} \right)}}{2}                                        …… (1)

Here,

C is the number of carbons.

H is the number of hydrogens.

X is the number of halogens.

N is the number of nitrogens.

The molecular formula of the given compound is {{\text{C}}_6}{{\text{H}}_{12}}. So it has 6 carbon atoms and 12 hydrogen atoms in it.

Substitute 6 for C, 12 for H, 0 for X and 0 for N in equation (1).

\begin{aligned}{\text{Element of unsaturation}}&=\frac{{\left( {2\left( {\text{6}} \right) + {\text{2}} - {\text{12}} - {\text{0}} + {\text{0}}} \right)}}{2}\\&={1}\end{aligned}

Therefore there is only one element of unsaturation in {{\text{C}}_6}{{\text{H}}_{12}}. This indicates either the presence of a double bond or a ring in the given compound.

Learn more:

1. What is the empirical formula of the compound? brainly.com/question/6126420

2. Write the name of the hydrocarbon: brainly.com/question/3551546

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Hydrocarbons

Keywords: hydrocarbon, saturated, unsaturated, alkene, alkyne, CnH2n+2, CnH2n, CnH2n-2, element of unsaturation, 1, .ring, double bond.

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How many grams of zinc would be required to produce 9.65g of zinc hydroxide
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The question is incomplete, here is the complete question:

How many grams of zinc would be required to produce 9.65g of zinc hydroxide

Zn+2MnO₂+H₂O→Zn(OH)₂+Mn₂O₃

<u>Answer:</u> The mass of zinc required is 6.35 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)

Given mass of zinc hydroxide = 9.65 g

Molar mass of zinc hydroxide = 99.4 g/mol

Putting values in equation 1, we get:

\text{Moles of zinc hydroxide}=\frac{9.65g}{99.4g/mol}=0.0971mol

The given chemical equation follows:

Zn+2MnO_2+H_2O\rightarrow Zn(OH)_2+Mn_2O_3

By Stoichiometry of the reaction:

1 mole of zinc hydroxide is produced from 1 mole of zinc

So, 0.0971 moles of zinc hydroxide will be produced from = \frac{1}{1}\times 0.0971=0.0971mol of zinc

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

Molar mass of zinc = 65.4 g/mol

Moles of zinc = 0.0971 moles

Putting values in equation 1, we get:

0.0971mol=\frac{\text{Mass of zinc}}{65.4g/mol}\\\\\text{Mass of zinc}=(0.0971mol\times 65.4g/mol)=6.35g

Hence, the mass of zinc required is 6.35 grams

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Bezzdna [24]
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Read 2 more answers
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