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Dima020 [189]
3 years ago
7

What is one bad thing that can happen when humans build more and more streets and buildings?

Chemistry
1 answer:
Irina18 [472]3 years ago
4 0

Answer:

there will be less and less space

Explanation:

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Using the mmoles of (35)-2,2,-dibromo-3,4-dimethylpentane calculated earlier and the molecular weight of the product (962 g/mol)
Sedbober [7]

Answer:

The yield of the product in gram is \mathsf{{w_P}=0.26 \ gram}

Explanation:

Given that:

the molecular mass weight of the product = 96.2 g/mol

the molecular mass of the reagent (3S)-2,2,-dibromo-3,4-dimethylpentane is 257.997 g

given that the millimoles of the reagent = 2,7 millimoles = 2.7 \times 10^{-3} \ moles

We know that:

Number of moles = mass/molar mass

Then:

2.7 \times 10^{-3} = \dfrac{ mass}{257.997}

mass = 2.7 \times 10^{-3} \times 257.997

mass = 0.697

Theoretical yield = (number of moles of the product/ number of moles of reactant) × 100

i.e

Theoretical yield = \dfrac{n_P}{n_R}\times 100\%

where;

n_P = \dfrac{w_P}{m_P}    and n_R = \dfrac{w_R}{m_R}

Theoretical yield = \dfrac{(\dfrac{w_P}{m_P})}{(\dfrac{w_R}{m_R})} \times 100\%

Given that the theoretical yield = 100%

Then:

100\% =\dfrac{(\dfrac{w_P}{m_P})}{(\dfrac{w_R}{m_R})} \times 100\%

\dfrac{w_P}{m_P}=\dfrac{w_R}{m_R}

{w_P}=\dfrac{w_R \times m_P}{m_R}

where,

w_P = derived weight of the product

m_P =the molecular mass of the derived product

m_R = the molecular mass of the reagent

w_R = weight in a gram of the reagent

{w_P}=\dfrac{w_R \times m_P}{m_R}

{w_P}=\dfrac{0.697 \times 96.2}{257.997}

\mathsf{{w_P}=0.26 \ gram}

8 0
3 years ago
Why Ammonia is nut dried by passing through concentrated H2SO4.​
STALIN [3.7K]

Answer:

Because it is absorbed by conc . H . SO , to form ammonium sulphate.

6 0
3 years ago
171 g of sucrose ( MW of 342, melting point 186 oC, boiling point very high, and vapor pressure is negligible) is dissolved in o
Fantom [35]

The complete question is as follows: 171 g of sucrose ( MW of 342, melting point 186 oC, boiling point very high, and vapor pressure is negligible) is dissolved in one liter of water at 25 oC. At 25 oC the vapor pressure of water is 24 mmHg. Which value is closest to the vapor pressure (VP) of this solution at 25 oC?

a. 16mm Hg

b. 24mm Hg  

c. 20mm Hg  

d. 12mm Hg

Answer: The vapor pressure (VP) of this solution at 25^{o}C is closest to the value 24 mm Hg.

Explanation:

Given: Mass of sucrose = 171 g

Mass of water = 1 L = 1000 g

Vapor pressure of water = 24 mm Hg

As moles is the mass of substance divided by its molar mass. Hence, moles of water (molar mass = 18.02 g) is calculated as follows.

Moles = \frac{mass}{molar mass}\\= \frac{1000 g}{18.02 g/mol}\\= 55.49 mol

Similarly, moles of sucrose (molar mass = 342 g/mol) is as follows.

Moles = \frac{mass}{molar mass}\\= \frac{171 g}{342 g/mol}\\= 0.5 mol

Total moles = 55.49 + 0.5 mol = 55.99 mol

Mole fraction of water is as follows.

Mole fraction = \frac{moles of water}{total moles}\\= \frac{55.49}{55.99}\\= 0.99

Formula used to calculate vapor pressure of the solution is as follows.

P_{i} = P^{o}_{i} \times \chi_{i}

where,

P_{i} = vapor pressure of component i over the solution

P^{o}_{i} = vapor pressure of pure component i

\chi_{i} = mole fraction of i

Substitute the values into above formula to calculate vapor pressure of water as follows.

P_{i} = P^{o}_{i} \times \chi_{i}\\= 24 mm Hg \times 0.99\\= 23.76 \\or 24 mm Hg\\

Thus, we can conclude that the vapor pressure (VP) of this solution at 25^{o}C is closest to the value 24 mm Hg.

4 0
3 years ago
In terms of electrons, what is the difference between a covalent and ionic bond
kramer

Answer:

An ionic bond essentially donates an electron to the other atom participating in the bond, while electrons in a covalent bond are shared equally between the atoms. Ionic bonds form between a metal and a nonmetal. Covalent bonds form between two nonmetals

7 0
3 years ago
3. What is the molar mass of O2? Round to nearest whole number.<br> 8<br> O<br> 16<br> 32<br> 64
SVETLANKA909090 [29]

Answer:

Molar mass of O is = 16

Molar mass of O2 = 32

5 0
3 years ago
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