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Galina-37 [17]
3 years ago
12

Look at the image please. I need the help as soon as possible.

Chemistry
1 answer:
boyakko [2]3 years ago
5 0

Answer:

It's the first option

Explanation:

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PLS HELP! WILL MARK BRAINLIEST!!! 50 PTS
AveGali [126]

Answer:

from the pic:

empirical \: formular :  \:  \: C  _{2}H _{3}O _{2}

since molar mass is 118.084 g/mol;

(C  _{2}H _{3}O _{2}) _{n} = 118.084 \\ C  _{2n}H _{3n}O _{2n} = 118.084 \\(12 \times 2)  _{n} + (1 \times 3) _{n} + (16 \times2 ) _{n} = 118.084 \\ 24_{n} + 3_{n} + 32_{n} = 118.084 \\ 59_{n} = 118.084 \\ n = 2

{ \boxed{ \bf{molecular \: formular :  \: C  _{4}H _{6}O _{4}}}}

It is an aldehyde with structure ( second pic )

3 0
3 years ago
10. A small gold nugget has volume of 0.87 cm3. What is its mass if the density of gold is 19.3 g/cm3?
bulgar [2K]

Answer:

16.791 grams

Explanation:

The density formula is:

d=\frac{m}{v}

Rearrange the formula for m, the mass. Multiply both sides of the equation by v.

d*v=\frac{m}{v}*v

d*v=m

The mass of the gold nugget can be found by multiplying the density and volume. The density is 19.3 grams per cubic centimeter and the volume is 0.87 cubic centimeters.

d= 19.3 g/cm^3\\v-0.87 cm^3

Substitute the values into the formula.

m=d*v

m= 19.3 g/cm^3*0.87 cm^3

Multiply. Note that the cubic centimeters, or cm³ will cancel each other out.

m=19.3 g*0.87

m=16.791 g

The mass of the gold nugget is 16.791 grams.

8 0
3 years ago
"what is the mole fraction of solute in a 3.87 m aqueous solution?"
sattari [20]

The mole fraction of solute in a 3.87 m aqueous solution is 0.0697

<h3> calculation</h3>

molality = moles of the solute/Kg of the solvent

3.87 m dissolve in 1 Kg of water= 1000g

find the moles of water= mass/molar mass

that is 1000 g/ 18 g/mol= 55.56 moles

mole of solute = 3.87 moles

mole fraction is = moles of solute/moles of solvent

that is 3.87/ 55.56 = 0.0697

5 0
3 years ago
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By there pH . a pH below 7 is acidic . Above 7 is basic. If it’s right at 7 it’s neutral.
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