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Archy [21]
2 years ago
6

Please help ASAP! What mass of hydrogen is needed to produce 10 moles of ammonia (NH3)?

Chemistry
1 answer:
stiks02 [169]2 years ago
7 0

Answer:

Mass = 30 g

Explanation:

Given data:

Mass of hydrogen needed = ?

Number of moles of ammonia produced = 10 mol

Solution:

Chemical equation:

N₂ + 3H₂        →      2NH₃

Now we will compare the moles of ammonia and hydrogen.

                  NH₃            :                H₂

                    2               :                3

                   10               :               3/2×10 = 15 mol

Mass of hydrogen needed:

Mass = number of moles × molar mass

Mass = 15 mol × 2 g/mol

Mass = 30 g

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According to the law of conservation of mass, what is the same on both sides of a balanced chemical equation?
Firlakuza [10]

According to the law of conservation of mass, what is the same on both sides of a balanced chemical equation?

A. the volume of the substances

B. the subscripts

C. the total mass of atoms

D. the coefficients

Answer:

A balanced equation demonstrates the conservation of mass by having the same number of each type of atom on both sides of the arrow.

Explanation:

Every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. ... Use coefficients of products and reactants to balance the number of atoms of an element on both sides of a chemical equation.

Consider the balanced equation for the combustion of methane.

CH

4

+

2O

2

→

CO

2

+

2H

2

O


All balanced chemical equations must have the same number of each type of atom on both sides of the arrow.


In this equation, we have 1

C

atom, 4

H

atoms, and 4

O

atoms on each side of the arrow.


The number of atoms does not change, so the total mass of all the atoms is the same before and after the reaction. Mass is conserved.


Here is a video that discusses the importance of balancing a chemical equation.

8 0
2 years ago
In which of these diatomic molecules would you NOT find an octet of electrons
Semmy [17]

Answer:

The hydrogen molecule is the only one in which can not find an octet of electrons around each atom.

Explanation:

Let's evaluate each case.  

1. Nitrogen (N₂):

With Z = 7, nitrogen has the following electronic configuration

1s²

2s² 2p³  → valence electrons

Since its valence electrons are 5, in the molecule one nitrogen atom shares 3 electrons with the other one, and each remains with an electron pair, so <u>each atom has an octet of electrons.</u>

2. Hydrogen (H₂):

With Z = 1, its electronic configuration is:

1s¹  → valence electron

In the molecule, the hydrogen atoms share the only electron they have, so they will have only 2 electrons around. In this diatomic molecule, <em><u>we can not find an octet.</u></em>

3. Oxygen (O₂):

Z = 8. Electronic configuration:

1s²

2s² 2p⁴  → valence electrons

In the diatomic molecule, each oxygen atom shares 2 electrons with the other one and remains with 2 pairs of electrons, therefore, <u>each oxygen atom has an octet</u>.      

4. Fluorine (F₂)

Z = 9. Electronic configuration:

1s²

2s² 2p⁵  → valence electrons

In this molecule, each fluorine atom shares 1 electron with the other and remains with 3 pairs of electrons, hence, <u>each fluorine atom has an octet of electrons around</u>.

Finally, we can say that the hydrogen molecule is the only one in which can not find an octet of electrons around each atom.

I hope it helps you!  

8 0
2 years ago
Atoms of which two elements have combined total of 23 protons​
vichka [17]

Answer:

sodium and magnesium

Explanation:

4 0
3 years ago
Read 2 more answers
For the following reaction, 38.3 grams of sulfuric acid are allowed to react with 33.5 grams of calcium hydroxide sulfuric acid(
Likurg_2 [28]

Answer:

What is the maximum amount of calcium sulfate that can be formed? 53.1 grams CaSO4

What is the FORMULA for the limiting reagent? H2SO4

What amount of the excess reagent remains after the reaction is complete? 4.59 grams of Ca(OH)2

Explanation:

Step 1: Data given

Mass of sulfuric acid = 38.3 grams

Molar mass of H2SO4 = 98.08 g/mol

Mass of calcium hydroxide = 33.5 grams

Molar mass of Ca(OH)2 = 74.09 g/mol

Step 2: The balanced equation

H2SO4 + Ca(OH)2 → CaSO4 + 2H2O

Step 3: Calculate moles of H2SO4

moles H2SO4 = mass H2SO4 / molar mass H2SO4

moles H2SO4 = 38.3 grams / 98.08 g/mol

moles H2SO4 = 0.390 moles

Step 4: Calculate moles of Ca(OH)2

moles Ca(OH)2 = 33.5 grams / 74.09 g/mol

moles Ca(OH)2 =0.452 moles

Step 5: Calculate limiting reactant

For 1 mol H2SO4, we need 1 mol of Ca(OH)2 to produce, 1 mol of CaSO4 and 2 mol of H2O

H2SO4 is the limiting reactant. It will completely be consumed (0.390 moles).

Ca(OH)2 is in excess. There will be consumed 0.390 moles

There will remain 0.452 - 0.390 = 0.062 moles

This is 0.062 * 74.09 g/mol = 4.59 grams

Step 6: Calculate moles of calcium sulfate

For 1 mol H2SO4, we need 1 mol of Ca(OH)2 to produce, 1 mol of CaSO4 and 2 mol of H2O

For 0.390 moles of H2SO4, there will be produced 0.390 moles of CaSO4

Step 7: Calculate mass of CaSO4

Mass CaSO4 = moles CaSO4 * molar mass CaSO4

Mass CaSO4 = 0.390 moles * 136.14 g/mol

Mass of CaSO4 = 53.1 grams

7 0
2 years ago
Martin slowly pours an unknown liquid into a container that originally had some water in it. He is measuring the temperature in
Evgen [1.6K]
B. a chemical change
8 0
2 years ago
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