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3 years ago

A compound is found to contain 11.21 % hydrogen and 88.79 % oxygen by mass. What is the empirical formula for this compound?

Chemistry

2 answers:

Artemon [7]3 years ago

7 0

Answer:

H₂O

Explanation:

The empirical formular of the compound is obtained using the following steps;

Step 1: Divide the percentage composition by the atomic mass

Hydrogen = 11.21 / 1 = 11.21

Oxygen = 88.79 / 16 = 5.55

Step 2: Divide by the lowest number

Hydrogen = 11.21 / 5.55 = 2.02 ≈ 2

Oxygen = 5.55 / 5.55 = 1

This means the ratio of the elements is 2 : 1

The empirical formular (simplest formular of a compound) of the compound is;

H₂O

stiv31 [10]3 years ago

3 0

Answer:Empirical formula ======== H₂O

Explanation:The empirical formula of a compound shows the whole number ratio for each atom in a compound.

To find empirical formula. we follow the below steps

The total mass of the compound here is 100 grams, that is (11.21% of hydrogen + 88.79% of oxygen) we can then assume 11.21 grams of hydrogen and 88.79grams of oxygen

Hydrogen Oxygen

1.composition by mass 11.21 88.79

molecular weight 1.007g/mol 15.990g/mol

2.Divide composition by mass 11.21/1.007 88.79/15.99

by each molecular weight to get 11.13 5.553

no of moles

3 Divide by the least number of moles

to get atomic ratio 11.13/5.553 5.553/5.553

2.004 1.00

4.Convert to whole numbers 2 1

Empirical formula ======== H₂O

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How much water (H2O ) would form if 4.04 g of hydrogen (H2) reacted with 31.98 g of oxygen (O2 )?

Norma-Jean [14]

Answer:

Mass = 36 g

Explanation:

Given data:

Mass of water formed = ?

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Mass of oxygen = 31.98 g

Solution:

Chemical equation:

2H₂ + O₂ → 2H₂O

Number of moles of hydrogen:

Number of moles = mass/molar mass

Number of moles = 4.04 g/ 2 g/mol

Number of moles = 2.02 mol

Number of moles of oxygen:

Number of moles = mass/molar mass

Number of moles = 31.98 g/ 32 g/mol

Number of moles = 1.0 mol

Now we will compare the moles of water with hydrogen and oxygen.

O₂ : H₂O

1 : 2

H₂ : H₂O

2 : 2

2.02 : 2.02

Number of moles of water formed by oxygen are less thus oxygen will limiting reactant.

Mass of water:

Mass = number of moles × molar mass

Mass = 2 mol × 18 g/mol

Mass = 36 g

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In order to solve this problem, a good knowledge of the periodic table and shell notation is required.

For example;

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We know the number is made of both the atomic number of the element and the highest quantum number.

It is easier for us to know the highest quantum number from the shell notation:

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We are left with atomic number 5-2, which is 3

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s-orbital brainly.com/question/9288609

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3 years ago

How many moles are there in 3.612 x 1024 formula units of Na2SO4?

vitfil [10]

Answer:

<h3>Theanswer is 6 moles</h3>

Explanation:

To find the number of moles in a substance given it's number of entities we use the formula

$n = \frac{N}{L} \\$

where n is the number of moles

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L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

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We have the final answer as

<h3>6 moles</h3>

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3 years ago

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Explanation:

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