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3 years ago

A 23.0g sample of a compound contains 12.0g of C, 3.0g of H, and 8.0g of O.What the empirical formula of the compound

Chemistry

1 answer:

Kryger [21]3 years ago

5 0

Answer:

The empirical formula of compound is C₂H₆O.

Explanation:

Given data:

Mass of carbon = 12 g

Mass of hydrogen = 3 g

Mass of oxygen = 8 g

Empirical formula of compound = ?

Solution:

First of all we will calculate the gram atom of each elements.

no of gram atom of carbon = 12 g / 12 g/mol = 1 g atoms

no of gram atom of hydrogen = 3 g / 1 g/mol = 3 g atoms

no of gram atom of oxygen = 8 g / 16 g/mol = 0.5 g atoms

Now we will calculate the atomic ratio by dividing the gram atoms with the 0.5 because it is the smallest number among these three.

C:H:O = 1/0.5 : 3/0.5 : 0.5/0.5

C:H:O = 2 : 6 : 1

The empirical formula of compound will be C₂H₆O

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Answer:

In order to prepare 200.0 mL of an aqueous solution of iron (III) chloride, at a concentration of 1.25 x 10⁻² M, you need to weight 0.4055 g of FeCl₃ and add to 200.0 mL of water.

Explanation:

Concentration: 1.25 x 10⁻² M

1,25 x 10⁻² mol FeCl₃ ___ 1000 mL

x ___ 200.0 mL

x = 2.5 x 10⁻³ mol FeCl₃

Mass of FeCl₃:

1 mol FeCl₃ _____________ 162.2 g

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8 0

4 years ago

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dlinn [17]

Answer:

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8 0

3 years ago

If the vapor pressure of pure benzene is 96.1 mm Hg, what must the vapor pressure of pure toluene be in order for the 50/50 % mi

mylen [45]

Answer:

$P_{tol}=30.34mmHg$

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to calculate the vapor pressure of pure toluene by using the Raoult's law as shown below:

$y_{tol}P_{mix}=x_{tol}P_{tol}\\\\y_{ben}P_{mix}=x_{ben}P_{ben}$

Thus, we solve for the mole fraction of benzene in the vapor phase first:

$y_{ben}=\frac{x_{ben}P_{ben}}{P_{mix}} =\frac{0.5*96.1mmHg}{63.2mmHg}=0.76$

Which means that the mole fraction of toluene in the vapor phase is 0.24, and therefore, the vapor pressure of pure toluene turns out to be:

$P_{tol}=\frac{y_{tol}P_{mix}}{x_{tol}} =\frac{0.24*63.2mmHg}{0.5}=30.34mmHg$

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7 0

3 years ago

How many moles of water are produced when 3.45 moles of KMnO4 react? Give your answer to the nearest 0.1 moles. moles H2O

andrew11 [14]

Answer:

13.8 moles of water produced.

Explanation:

Given data:

Moles of KMnO₄ = 3.45 mol

Moles of water = ?

Solution:

Chemical equation:

16HCl + 2KMnO₄ → 2KCl + 2MnCl₂ + 5Cl₂ + 8H₂O

Moler ratio of water and KMnO₄:

KMnO₄ : H₂O

2 : 8

3.45 : 8/2×3.45 = 13.8 mol

Hence, 3.45 moles of KMnO₄ will produced 13.8 mol of water.

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3 years ago

How many formula units are in 4.52 moles of H3SO3?<br> Type your answer

lakkis [162]

Answer:

The answer is 98.07848. We assume you are converting between grams H2SO4 and mole. You can view more details on each measurement unit: This compound is also known as Sulfuric Acid. The SI base unit for amount of substance is the mole. 1 grams H2SO4 is equal to 0.010195916576195 mole.

<u>Quick conversion chart of moles H2SO3 to grams</u>

1 moles H2SO3 to grams = 82.07908 grams

2 moles H2SO3 to grams = 164.15816 grams

3 moles H2SO3 to grams = 246.23724 grams

4 moles H2SO3 to grams = 328.31632 grams

5 moles H2SO3 to grams = 410.3954 grams

6 moles H2SO3 to grams = 492.47448 grams

7 moles H2SO3 to grams = 574.55356 grams

8 moles H2SO3 to grams = 656.63264 grams

9 moles H2SO3 to grams = 738.71172 grams

10 moles H2SO3 to grams = 820.7908 grams

7 0

3 years ago