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3 years ago

The empirical formula of styrene is ch; its molar mass is 104.1 g/mol. what is the molecular formula of styrene? select one:

2 answers:

6 0

The empirical formula is a formula of a compound showing the proportion of each element involved in the compounds but it does not represent the total number of atoms in the compound. It is the lowest number of ratio between the elements in the compound. In order, to determine the actual number of the atoms or the molecular formula of the compounds, we make use of the molar mass of the compound.

<span>To determine the molecular formula, we multiply a value to the empirical formula. Then, calculate the molar mass and see whether it is equal to the one given (104.1 g/ mol). From the choices, the only valid options are b, d and e.
</span> molar mass
1 CH 13.02
8 C8H8 104.16
6 C6H6 78.12

Therefore the correct answer is option B.

geniusboy [140]3 years ago

3 0

Answer:

b. C₈H₈

Explanation:

The empirical formula of styrene is CH. To calculate the molecular formula, we have to calculate "n", where n:

$n=\frac{molar\ mass\ molecular\ formula }{molar\ mass\ empirical\ formula}$

The molar mass of the empirical formula is C + H = 12.01 + 1.00 = 13.01 g/mol

The molar mass of the molecular formula is 104.1 g/mol

n = (104.1 g/mol) / (13.01 g/mol) ≈ 8

The molecular formula is:

Molecular formula = n × Empirical formula = 8 × CH = C₈H₈

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dlinn [17]

Answer:

Molarity of sodium acetate you will need to add is 0.0324M

Explanation:

<em>Assuming volume of the buffer is 1L.</em>

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The pH of a buffer can be determined using Henderson-Hasselbalch equation:

pH = pKa + log [A⁻] / [HA]

<em>Where pKa is pKa of the weak acid, [A⁻] molar concentration of conjugate base and [HA] molar concentration of weak acid</em>

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Replacing for the acetic buffer (pKa = 4.76):

pH = 4.76 + log [Sodium Acetate] / [Acetic Acid]

As you have 0.010 moles of acetic acid in 1L:

[Acetic Acid] = 0.010mol / 1L = 0.010M

And you require a pH of 5.27:

5.27 = 4.76 + log [Sodium Acetate] / [0.010M]

0.51 = log [Sodium Acetate] / [0.010M]

10^0.51 = [Sodium Acetate] / [0.010M]

3.236 = [Sodium Acetate] / [0.010M]

3.236 [0.010M] = [Sodium Acetate]

0.0324M = [Sodium Acetate]

<h3>Molarity of sodium acetate you will need to add is 0.0324M</h3>

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2 years ago

Plz help for brainlieast answer

Debora [2.8K]

Answer:

Na+

Explanation:

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2 years ago

Write a balanced chemical equation for the standard formation reaction of gaseous formaldehyde CH2O

Free_Kalibri [48]

From the combustion of octane, the formaldehyde will be formed as this equation:

C8H18 + O2 → CH2O + H2O this is the original equation but it is not a balanced equation, so let's start to balance it:

the equation to be balanced so the number of atoms on the right side of the equation sholud be equal with the number of atoms on the lef side.

-we have 8 C atoms on left side and 1 atom on the right side so we will try putting 8 CH2O on the right side instead of CH2O

C8H18 + O2 → 8 CH2O + H2O

we have 2 O atoms on the left side and 9 atoms on the right side so we will try first to put 9 O2 instead of O2 on the left side and put 2H2O on the right side and put 16 CH2O instead of 8 CH2O to make the atoms of O are equal on both sides = 18 atoms

C8H18 + 9 O2 → 16 CH2O + 2H2O

put now we have 8 atom C on the left side and 16 atom on the right side so, we will put 2 C8H18 instead of C8H18 now we get this equation:

2C8H18 + 9O2 →16 CH2O + 2H2O

-now we have 36 of H atoms on both sides.

- and 16 of C atoms on both sides.

- and 18 of O atoms on both sides.

now all the number of atoms of O & C & H are equal on both sides

∴ 2C8H18 + 9O2 → 16 CH2O + 2 H2O

is the final balanced equation for the formation of formaldehayde

5 0

3 years ago

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LUCKY_DIMON [66]

Answer: Directly through the phospholipid membrane

Explanation:

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3 years ago

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zvonat [6]

Answer:

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Explanation:

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3 years ago