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S_A_V [24]
3 years ago
5

_P4 + ____O2 → __P2O3 How do I balance this equation?

Chemistry
2 answers:
enot [183]3 years ago
7 0

Explanation:

<em>hope</em><em> it's</em><em> helpful</em><em> for</em><em> you</em>

<em>pls</em><em> mark</em><em> above</em><em> guy</em><em> ans</em><em> as</em><em> brainliest</em>

Murljashka [212]3 years ago
5 0

Explanation:

please mark me as brainlest

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A buret was improperly read to 1 decimal place giving a reading of 27.2 mL. If the actual volume is 27.26 mL, what is the percen
Nezavi [6.7K]
Percent error can be calculated by the difference of the theoretical value and the measured value divided by the theoretical value multiplied by 100 percent. 

% error = 27.26 - 27.2 / 27.26 x100
% error = 0.22%

A value close to zero would mean that the measured value is more or less near the actual value.
5 0
3 years ago
Read 2 more answers
A factor that keeps a population size from growing too large is called a ______ _______.
Liula [17]

Answer:

limiting factor i think

7 0
3 years ago
Read 2 more answers
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xenn [34]

Answer:

Its C hope it helped

Explanation:

3 0
3 years ago
what is the molar mass of a gaseous flouride of sulfur containing 70.4% F and having a density of approximately 4.5g/L at 20 deg
zlopas [31]

Answer:

The molar mass is 180.2 g/mol

Explanation:

<u>Step 1:</u> Data given

% of F = 70.4 %

Density = 4.5 g/L

Temperature = 20 °C

Pressure = 1 atm

<u>Step 2:</u> Calculate the number of moles

PV = nRT

 ⇒ with P = the pressure = 1.00 atm

⇒ with V = the volume = Assume this is 1L

⇒ with n = the number of moles = TO BE DETERMINED

⇒ R = the gas constant = 0.08206 L*atm/K*mol

⇒ T = the temperature : 20°C = 293 Kelvin

1 atm*1L= n(0.08206 L-atm/mol-K)*(293 K)

n = 0.04159 moles

<u>Step 3</u>: Calculate molar mass

Molar mass = Mass / moles

4.5 grams / 0.04159 moles = 108.2 g/mol

<u>Step 4:</u> Calculate moles of F

Moles = Mass / molar mass

Moles F = 70.4 g / 19 g/mol

Moles F =  3.70 moles

Moles S = 29.6g / 32.07 g/mol

Moles S = 0.923 moles S

<u>Step 5:</u> Divide by the smallest amount of moles

F = 3.70 / 0.923 = 4

S = 0.923 / 0.923 = 1

The empirical formula is SF4

The molar mass of SF4 = 32.07 + 4*19 = 108.07 g/mol

This means the empirical formula is the same as the molecular formula SF4

The molar mass is 180.2 g/mol

4 0
3 years ago
A mixture of compounds containing diethylamine, phenol, ammonia, and acetic acid is separated using liquid-liquid extraction as
umka2103 [35]

Answer:

I would expect to extract the acetic acid.

Explanation:

In the first step, since we are adding a concentrated acid,<u> it will react with the bases present in the mixture (diethylamine and ammonia) </u><u>forming salts</u><u>, </u><u>which are soluble in water</u>. Therefore, after draining the aqueous layer, we will have phenol and acetic acid left in the organic layer.

In the second step, we are adding a diluted base, so it will react with a strong acid. This compound is acetic acid, and its salt will be present in the aqueous layer. Phenol will be left on the organic layer.

7 0
3 years ago
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