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strojnjashka [21]
3 years ago
8

Balance the following chemical equation by providing the correct coefficients.

Chemistry
1 answer:
sukhopar [10]3 years ago
7 0

Answer:

2Na+2H2O→2NaOH+H2

Explanation:

I think this is it

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All of the halogens, group 17, have seven valence electrons. which of these would represent the oxidation number of the halogens
fomenos
It depends if it occurs naturally it has oxidation number of 0
but when it react with other element it has an oxidation number of -1
6 0
3 years ago
PLEASE HELP I DONT WANT TO FAIL!! ):
Fudgin [204]
Hope this helps :) I didn’t know how to write subscripts so I wrote it down on some paper.

3 0
3 years ago
Given the following equation, what is the correct form of the conversion factor needed to convert the number of moles of O₂ to t
djverab [1.8K]

Answer : The correct option is (c) \frac{2\text{ mole of }Fe_2O_3}{3\text{ mole of }O_2}

Explanation :

The given balanced chemical reaction is,

4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)

From the balanced chemical reaction, we conclude that

As, 3 moles of O_2 react to give 2 mole of Fe_2O_3

So, 1 mole of O_2 react to give \frac{2\text{ mole of }Fe_2O_3}{3\text{ mole of }O_2} moles of Fe_2O_3

Thus, the conversion factor needed to convert the number of moles of O_2 to the number of moles of Fe_2O_3 produced is \frac{2\text{ mole of }Fe_2O_3}{3\text{ mole of }O_2}

Hence, the correct option is (c) \frac{2\text{ mole of }Fe_2O_3}{3\text{ mole of }O_2}

7 0
3 years ago
Read 2 more answers
In an atom, the number of neutrons determines most specifically the ________.
lord [1]

In an atom, the number of neutrons determines most specifically the isotopes of an element.

<h2>Further Explanation</h2><h3>An atom  </h3>
  • An atom is defined as the smallest particle of an element that can take part in a chemical reaction.
  • Atoms are made of energy shells and the inner nucleus.
  • It is also made up of subatomic particles, protons and neutrons.
<h3>Neutrons  </h3>
  • They are sub-atomic particles in an atom that are found in the nucleus of an atom. They have a zero charge or no charge.
  • Neutrons are slightly heavier than protons.
  • The number of protons and neutrons in a nucleus of an atom results to the atomic mass number of an atom. Like protons they only take part in nuclear reactions.
<h3>Protons</h3>
  • Protons are subatomic particles that are found in the nucleus of an atom. They are positively charged. with a charge of +1.
  • The number of protons differ from one element to another and thus used as the atomic number of an individual element.
  • The nucleus of an atom is positively charged due to the positive charge of the protons.  
  • Additionally, protons do not take part in chemical reactions but in nuclear reactions.
<h3>Electrons  </h3>
  • They are found orbiting the nucleus on energy shells based on Clouds’ theory. Electrons are negatively charged each with a charge of -1.
  • The number of electrons and protons in a neutral atom are equal. Additionally they have the least mass of the three sub-atomic particles.
  • Electrons are the only sub-atomic particles that take part in chemical reactions.
<h3>Isotopes </h3>
  • Isotopes are atoms of the same element that have the same mass number but different atomic number.
<h3>Mass number;</h3>
  • Mass number is the sum of the number of protons and neutrons in the nucleus of an atom of an element.

Keywords: Atom, sub-atomic particles, electrons, protons, neutrons, isotopes  

<h3>Learn more about:</h3>
  • Sub-atomic particles: brainly.com/question/12762384
  • Electrons: brainly.com/question/1264222
  • Protons: brainly.com/question/1264222
  • Neutrons: brainly.com/question/1264222
  • Mass number: brainly.com/question/2152789
  • Atomic number: brainly.com/question/8100107

Level: High school

Subject: Chemistry  

Topic: Atomic structure

4 0
3 years ago
Read 2 more answers
Combustion of 9.511 grams of c4h10 will yield ____ grams of CO2
Flauer [41]

Answer:

\boxed{28.81}

Explanation:

We know we will need an equation with masses and molar masses, so let’s gather all the information in one place.  

M_r:      58.12                   44.01

           2C₄H₁₀ + 13O₂ ⟶ 8CO₂ + 10H₂O

m/g:     9.511

1. Moles of C₄H₁₀

\text{Moles of C$_{4}$H$_{10} $} = \text{ 9.511 g C$_{4}$H$_{10} $} \times \dfrac{\text{1 mol C$_{4}$H$_{10} $}}{\text{ 58.12 g C$_{4}$H$_{10} $}} = \text{0.1636 mol C$_{4}$H$_{10}$}

2. Moles of CO₂

The molar ratio is 8 mol CO₂:2 mol C₄H₁₀

\text{Moles of CO}_{2} =\text{0.1636 mol C$_{4}$H$_{10} $} \times \dfrac{\text{8 mol CO}_{2}}{\text{2 mol C$_{4}$H$_{10}$}} = \text{0.6546 mol CO}_{2}

3. Mass of CO₂

\text{Mass of CO}_{2} = \text{0.6546 mol CO}_{2} \times \dfrac{\text{44.01 g CO}_{2}}{\text{1 mol CO}_{2}} = \textbf{28.81 g CO}_{2}\\\\\text{The combustion will form $\boxed{\textbf{28.81 g CO}_{2}}$}

8 0
3 years ago
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