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Alla [95]
3 years ago
14

Chlorofluorocarbons (CFCs) are no longer used as refrigerants because they destroy the ozone layer. Trichlorofluoromethane (CCl₃

F) boils at 296.95 K, and its molar heat of vaporization is 24.8 kJ/mol.
Calculate the molar entropy of the evaporation of CC₃F (l).
Chemistry
1 answer:
Daniel [21]3 years ago
8 0

Answer:

The molar entropy of the evaporation of Trichlorofluoromethan is 83.516 J/molK.

Explanation:

Entropy :It is defined as amount of energy which is unable to do work or the measurement of randomness or disorderedness in a system.

S=\frac{Q}{T(Kelvins)}

Molar heat of molar vaporization of Trichlorofluoromethane = 24.8 kJ/mol

Temperature at which Trichlorofluoromethan boils , T= 296.95 K

The molar entropy of the evaporation of Trichlorofluoromethan :

=\frac{24.8 kJ/mol}{296.95 K}=0.083516 kJ/mol K = 83.516 J/molK

The molar entropy of the evaporation of Trichlorofluoromethan is 83.516 J/molK.

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guajiro [1.7K]

Answer:

the ph of an aqueous solution of sulphuric acid which is 5*10^5 mol in concentration is basic in nature

6 0
3 years ago
Which of the following involves a chemical reaction?
Andrews [41]
A combustion involves a chemical reaction.
6 0
3 years ago
The rotten smell of a decaying animal carcass is partially due to a nitrogen-containing compound called putrescine. Elemental an
balu736 [363]

The empirical formula is C_2H_6N.

<u>Explanation:</u>

Putrescine has the elements like Carbon, Nitrogen and Hydrogen present in them. So in order to determine the empirical formula, we first have to find the number of moles present in the putrescine. As the percentage of C, H and N present in the chemical is given as 54.50%, 13.73% and 31.77%, we assume that 100 g of Putrescine is taken as sample.

Then the mass of C, H and N present in Putrescine will be 54.50 g, 13.73 g and 31.77 g.  We know that the molar mass of C is 12 g/mol, H is 1 g/mol and N is 14 g/mol.  So divide the mass with the molar mass of the respective elements to determine the number of moles of these elements present in the sample.

<u></u>No.\ of\ moles\ of\ C=\frac{\text { Mass of } C}{\text { Molar mass of } C}=\frac{54.50 \mathrm{g}}{12 \mathrm{g} / \mathrm{mol}}=4.54\ moles<u></u>

Similarly, the number of moles of H and N present is determined.

\text { No. of moles of } H=\frac{\text { Mass of } H}{\text { Molar mass of } H}=\frac{13.73 \mathrm{g}}{1 \mathrm{g} / \mathrm{mol}}=13.73 \text { moles }

No.\ of\ moles\ of\ N=\frac{\text { Mass of } N}{\text { Molar mass of } N}=\frac{31.77 \mathrm{g}}{14 \mathrm{g} / \mathrm{mol}}=2.27\ moles

Then the empirical formula can be determined by dividing the number of moles of all elements with the least number of moles that is 2.27.

    \begin{aligned}&\text { No. of atoms of } C=\frac{4.54}{2.27}=2\\&\text { No. of atoms of } H=\frac{13.73}{2.27}=6\\&\text { No. of atoms of } N=\frac{2.27}{2.27}=1\end{aligned}

So, the empirical formula is C_2H_6N.

3 0
3 years ago
I need help with this question
Maru [420]

Aluminum sulfide : Al₂S₃

ratio cation : anion = 2 : 3

<h3>Further explanation</h3>

Given

Compound of Aluminium

Required

cations anions ratio

Solution

Salt can be formed from cations and anions which have their respective charges.

In the chemical compound formula these charges are crossed with each other

For aluminum it has a +3 charge

1. Aluminum carbide : Al₄C₃

ratio cation : anion = 4 : 3

2. Aluminum chloride : AlCl₃

ratio cation : anion = 1 : 3

3. Aluminum sulfide : Al₂S₃

ratio cation : anion = 2 : 3

4. Aluminum nitride : AlN

ratio cation : anion = 1 : 1

3 0
3 years ago
The coefficients in a balanced chemical equation represent
jolli1 [7]
(l ) the mass ratios of the substances in the reaction
<u>(2) the mole ratios of the substances in the reaction</u>
(3) the total number of electrons in the reaction
<span>(4) the total number of elements in the reaction</span>
6 0
3 years ago
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