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AnnyKZ [126]
3 years ago
15

Dichloroethane, a compound that is often used for dry cleaning, contains carbon, hydrogen, and chlorine. It has a molar mass of

99 g/mol. Analysis of a sample shows that it contains 24.3% carbon and 4.1% hydrogen. What is its molecular formula?
Chemistry
1 answer:
OverLord2011 [107]3 years ago
3 0

Answer: The molecular formula for the given compound is C_2H_4Cl_2

Explanation : Given,

Percentage of C = 24.3 %

Percentage of H = 4.1 %

Percentage of Cl = 100 - (24.3 + 4.1) = 71.6 %

Let the mass of compound be 100 g. So, percentages given are taken as mass.

Mass of C = 24.3 g

Mass of H = 4.1 g

Mass of Cl = 71.6 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon =\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{24.3g}{12g/mole}=2.025moles

Moles of Hydrogen = \frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{4.1g}{1g/mole}=4.1moles

Moles of Chlorine = \frac{\text{Given mass of chlorine}}{\text{Molar mass of chlorine}}=\frac{71.6g}{35.5g/mole}=2.017moles

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 2.017 moles.

For Carbon = \frac{2.025}{2.017}=1.00\approx 1

For Hydrogen  = \frac{4.1}{2.017}=2.03\approx 2

For Chlorine = \frac{2.017}{2.017}=1

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : Cl = 1 : 2 : 1

The empirical formula for the given compound is C_1H_2Cl_1=CH_2Cl

Mass of empirical formula = CH_2Cl  = 1(12) + 2(1) + 35.5 = 49.5 g/eq.

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is :

n=\frac{\text{molecular mass}}{\text{empirical mass}}

We are given:

Mass of molecular formula = 99 g/mol

Mass of empirical formula = 49.5 g/mol

Putting values in above equation, we get:

n=\frac{99g/mol}{49.5g/mol}=2

Multiplying this valency by the subscript of every element of empirical formula, we get:

CH_2Cl=(CH_2Cl)_n=(CH_2Cl)_2=C_2H_4Cl_2

Thus, the molecular formula for the given compound is C_2H_4Cl_2

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melomori [17]

Explanation:

As it is given that solubility of water in diethyl ether is 1.468 %. This means that in 100 ml saturated solution water present is 1.468 ml.

Hence, amount of diethyl ether present will be calculated as follows.

                          (100ml - 1.468 ml)

                        = 98.532 ml

So, it means that 98.532 ml of diethyl ether can dissolve 1.468 ml of water.

Hence, 23 ml of diethyl ether can dissolve the amount of water will be calculated as follows.

          Amount of water = \frac{1.468 ml \times 23 ml}{98.532 ml}

                                       = 0.3427 ml

Now, when magnesium dissolves in water then the reaction will be as follows.

                Mg + H_{2}O \rightarrow Mg(OH)_{2}

Molar mass of Mg = 24.305 g

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6 0
3 years ago
The enthalpy change for converting 1.00 mol of ice at -50.0 ∘c to water at 60.0∘c is ________ kj. the specific heats of ice, wat
guajiro [1.7K]
First, we have to get:

1- The heat required to increase T of ice from -50 to 0 °C:

according to q formula:

q1 = m*C*ΔT

when m is the mass of ice = mol * molar mass

                                             =  1 mol * 18 mol/g

                                            = 18 g

and C is the specific heat capacity of ice = 2.09 J/g-K

and ΔT change in temperature = 0- (-50) = 50°C

by substitution:

∴q1 = 18 g * 2.09 J/g-K *50°C

       = 1881 J = 1.881 KJ

2- the heat required to melt this mass of ice is :

q2 = n*ΔHfus 

when n is the number of moles of ice = 1 mol

and ΔHfus = 6.01 KJ/mol

by substitution:

q2 = 1 mol * 6.01 KJ/mol

     = 6.01 KJ

3- the heat required to increase the water temperature from 0°C to 60 °C is:

q3 = m*C*ΔT

when m is the mass of water = 18 g 

C is the specific heat capacity of water = 4.18 J/g-K

ΔT is the change of Temperature of water = 60°C - 0°C = 60°C

by substitution:

∴q3 = 18 g * 4.18 J/g-K * 60°C

      = 4514 J = 4.514 KJ

∴the total change of enthalpy = q1+q2+q3

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The correct answer is D. chemical reaction.

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23) What is the volume of 2.454 x 1024 atoms of nitrogen gas at STP?
earnstyle [38]

Answer:

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Explanation:

Given data:

Volume of nitrogen = ?

Temperature = standard = 273.15 K

Pressure = standard = 1 atm

Number of atoms of nitrogen = 2.454×10²⁴ atoms

Solution:

First of all we will calculate the number of moles of nitrogen by using Avogadro number.

1 mole = 6.022×10²³ atoms

2.454×10²⁴ atoms × 1 mol / 6.022×10²³ atoms

0.407×10¹ mol

4.07 mol

Volume of nitrogen:

PV = nRT

1 atm × V = 4.07 mol ×0.0821 atm.L /mol.K ×273.15 K

V =  91.3 atm.L /1 atm

V =  91.3 L

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