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leonid [27]
3 years ago
10

How benzene is formed?

Chemistry
2 answers:
Sergio039 [100]3 years ago
5 0
From natural processes
horsena [70]3 years ago
3 0
It is formed from natural causes
-volcanoes
-Forest Fires
You might be interested in
how many kilograms of water must evaporate from 8kg of a 25% salt solution to produce 40% salt solution?
Lena [83]

Answer: The kilograms of water must evaporate from 8kg of a 25% salt solution to produce 40% salt solution is 3 kg.

Explanation:

According to the ratio and proportion:

C_1m_1=C_2m_2

where,

C_1 = concentration of ist solution = 25%

m_1 = mass of ist solution = 8 kg

C_2 = concentration of second solution = 40%

m_2 = mass of second solution = ? kg

25\times 8=40\times m_2

m_2=5kg

Thus the final solution must have a mass of 5 kg , i.e (8-5)= 3 kg of mass must be evaporated.

Therefore, the mass that must be evaporated from 8kg of a 25% salt solution to produce 40% salt solution is 3 kg.

6 0
3 years ago
Which symbol is associated with structure C?<br> A. _<br> B.+<br> C.X<br> D.<br> none
IgorLugansk [536]
B I’m guessing not sure
6 0
2 years ago
The formula of nitrobenzene is c6h5no2. the molecular weight of this compound is __________ amu.
mafiozo [28]

The molecular weight of a given compound would simply the sum of the molar weights of each component.

 

The molar masses of the elements are:

C = 12 amu

H = 1 amu

N = 14 amu

O = 16 amu

where 1 amu = 1 g / mol

 

Since there are 6 C, 5 H, 1 N and 2 O, therefore the total molecular weight is:

molecular weight = 6 (12 amu) + 5 (1 amu) + 1 (14 amu) + 2 (16 amu)

molecular weight = 123 amu

 

Therefore the molecular weight of nitrobenzene is 123 amu or which is exactly equivalent to 123 g / mol.

4 0
3 years ago
Hank's Garage has an air compressor with a holding tank that contains 200L of compressed air at 5200 torr. One day a hose ruptur
Scrat [10]

Hank's Garage has an air compressor with a holding tank that contains 200L of compressed air at 5200 torr. One day a hose ruptured and all the compressed air was released to a volume of 1370 L at atmospheric pressure.

Hank's Garage has an air compressor with a holding tank that contains a volume of 200L (V₁) of compressed air at a pressure of 5200 torr (P₁).

One day a hose ruptured and all the compressed air was released. The final pressure was the atmospheric pressure (1 atm = 760 torr) (P₂).

We can calculate the new volume (V₂) in these conditions using Boyle's law, which states there is an inverse relationship between the volume and the pressure of an ideal gas.

P_1 \times V_1 = P_2 \times V_2\\\\V_2 = \frac{P_1 \times V_1}{P_2} = \frac{5200 torr \times 200L}{760torr} = 1370 L

Hank's Garage has an air compressor with a holding tank that contains 200L of compressed air at 5200 torr. One day a hose ruptured and all the compressed air was released to a volume of 1370 L at atmospheric pressure.

Learn more: brainly.com/question/1437490

4 0
3 years ago
A sample of hydrogen gas, has a volume of 8.56 L at a temperature 0oC and pressure of 1.5 atm. Calculate the number of moles of
erica [24]
P = 1.5atm ≈ 1519.88hPa
V = 8.56L
R = 83.1 [hPa*L] / [mol*K]
T = 0°C =273K

pV = nRT   |:RT

n = pV / RT

n = [1519.88hPa*8.56L] / [83.1 [hPa*L] / <span>[mol*K] * 273K]
n </span>≈ <u>0.57mol</u><span><u> </u></span>
3 0
3 years ago
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