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kvv77 [185]
3 years ago
6

A 143.1 g sample of a compound contains 53.4 g of carbon, 16.9 g of hydrogen, 43 g of nitrogen, and some amount of oxygen. what

is the mass percent of oxygen in the compound? 11.20% 11.81% 20.82% 30.05% 37.34%
Chemistry
2 answers:
nika2105 [10]3 years ago
6 0
I'm fairly sure this is it 20.82%
dalvyx [7]3 years ago
6 0

Answer:

20.82% is the mass percent of oxygen in the compound.

Explanation:

Total mass of the compound = 143.1 g

Mass of carbon = 53.4 g

Mass of hydrogen = 16.9 g

Mass of nitrogen= 43 g

Mass of oxygen= x

143.1 g = x + 53.4 g + 16.9 g + 43 g

x = 143.1 g - 53.4 g - 16.9 g - 43 g = 29.8 g

Percentage of oxygen in the compound:

\%=\frac{\text{Mass of oxygen}}{\text{Mass of compound}}\times 100

\%=\frac{29.8 g}{143.1 g}\times 100=20.82\%

20.82% is the mass percent of oxygen in the compound.

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MrMuchimi

Visual representation of covalent bonding indicating the valence shell electrons in the molecule, lines represents the shared pair of electron and pair of electrons that are not involved in bonding are represented as dots(lone pairs) are known as Lewis structures.

Compound formation takes place in order to complete the octet of each element that is according to octet rule, each atom forms bond with other atom in order to complete their octet that is to get eight electrons in its valence shell and attain stability.

An organic compound of the form R^{'}R^{''}C=C=O is known as ketene.

The given ketene is C_2H_2O.

The number of valence electron of:

C = 4

H = 1

O = 6

The number of valence electrons in C_2H_2O = 2\times 4+2\times 1+1\times 6 =16

2 electrons are involved in each single bond between carbon and hydrogen and 4 electrons are involved in each double bond formed between carbon-carbon and carbon-oxygen. Hence, the total number of electrons involved in bond formation are 12 and rest 2 pair of electrons are present on oxygen as lone pair of electrons.

Therefore, the attached image is the Lewis structure of C_2H_2O .

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In the laboratory, a general chemistry student measured the pH of a 0.529 M aqueous solution of phenol (a weak acid), C6H5OH to
Artyom0805 [142]

Answer:

The dissociation constant of phenol from given information is 9.34\times 10^{-11}.

Explanation:

The measured pH of the solution = 5.153

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Initially      c

At eq'm   c-x       x  x

The expression of dissociation constant is given as:

K_a=\frac{[C_6H_5O^-][H^+]}{[C_6H_5OOH]}

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3 years ago
In an electrically heated boiler, water is boiled at 140°C by a 90 cm long, 8 mm diameter horizontal heating element immersed in
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Explanation:

The given data is as follows.

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Density of water = 1000 kg/m^{3}

Therefore,  mass of water = Density × Volume

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                       = 250 kg  

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As 25% of water got evaporated at its boiling point (140^{o}C) in 60 min.

Therefore, amount of water evaporated = 0.25 × 250 (kg) = 62.5 kg

Heat required to evaporate = Amount of water evapotaed × Heat of vaporization

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