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2 years ago

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$\mathcal\blue{what \: is \: organic \: chemistry}$
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Chemistry

2 answers:

nignag [31]2 years ago

6 0

Organic chemistry as the the study of general properties and compositions of organic compounds.

<h3 />

<h3>What is organic chemistry?</h3>

Organic chemistry can be simply defined as the study of organic compounds.

Organic chemistry studies the structure, properties, composition, reactions, and preparation of carbon-containing compounds also known as organic compounds.

Thus, we can defined organic chemistry as the the study of general properties and compositions of organic compounds.

Learn more about organic chemistry here: brainly.com/question/704297

svlad2 [7]2 years ago

6 0

Organic chemistry is the study of the structure, properties, composition, reactions, and preparation of carbon-containing compounds

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The directional term that refers to an area or structure off to the side and away from the midline is __________.

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3 years ago

Ammonium phosphate NH43PO4 is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid H3PO4 with

VladimirAG [237]

Answer:

7.3 g (NH₄)₃PO₄

Explanation:

The balanced equation for the reaction is:

H₃PO₄ + 3 NH₃ ----> (NH₄)₃PO₄

To find the mass of ammonium phosphate ((NH₄)₃PO₄) produced, you need to (1) convert grams NH₃ to moles NH₃ (via the molar mass from the periodic table), then (2) convert moles NH₃ to moles (NH₄)₃PO₄ (via mole-to-mole ratio from balanced equation), and then (3) convert moles (NH₄)₃PO₄ to grams (NH₄)₃PO₄ (via molar mass from periodic table). Make sure to arrange the ratios/conversions in a way that allows for the cancellation of units. The final answer should have 2 sig figs because the given value (2.5 grams) has 2 sig figs.

Molar Mass (NH₃): 14.01 g/mol + 3(1.008 g/mol)

Molar Mass (NH₃): 17.034 g/mol

Molar Mass ((NH₄)₃PO₄):

3(14.01 g/mol) + 12(1.008 g/mol) + 30.97 g/mol + 4(16.00 g/mol)

Molar Mass ((NH₄)₃PO₄): 149.096 g/mol

2.5 g NH₃ 1 mole NH₃ 1 mole (NH₄)₃PO₄ 149.096 g
--------------- x -------------------- x --------------------------- x --------------------------
17.034 g 3 moles NH₃ 1 mole (NH₄)₃PO₄

= 7.3 g (NH₄)₃PO₄

8 0

2 years ago

A mixture of CO2 and Kr weighs 41.0 g and exerts a pressure of 0.729 atm in its container. Since Kr is expensive, you wish to re

Elena-2011 [213]

Answer:

a) 24.31 g

b) 16.69 g

Explanation:

A mixture of CO2 and Kr weighs 41.0 g and exerts a pressure of 0.729 atm in its container.

After the CO2 is completely removed by absorption with NaOH(s), the pressure in the container is 0.193 atm.

Therefore, Pressure of Kr = 0.193 atm

Pressure of CO2 = 0.729 - 0.193 = 0.536 atm

Their mole fraction can be also determined as follows:

CO2 = $\frac{Presssure due to CO_2}{Total pressure}$

CO2 = $\frac{0.536}{0.729}$

= 0.735

Also; for Kr ; we have

Kr = $\frac{0.193}{0.729}$

Kr = 0.265

Molar mass of CO2 = 44 g/mol

Molar mass of Kr = 83.78 g/mol

Mass of CO2 = mole fraction * molar mass = 0.735 * 44 = 32.34

Mass of Kr = 0.265 * 83.78 = 22.20

Total mass = 32.34 +22.20 = 54.54

The Percentage of gas in mixture is as follows:

% CO2 = $\frac{32.34}{54.54}$ * 100 %

= 0.5930

= 59.30%

(a) Mass of CO2 in mixture = 0.5930* 41 g = 24.31 g

% Kr = $\frac{22.20}{ 54.54}$ * 100 %

= 0.407

= 40.70 %

(b) Mass of Kr in mixture = 0.407 * 41 = 16.69 g

4 0

3 years ago