How many grams of methane are needed to form 33.6 L of carbon dioxide

Answers

Answer 1

Answer: If you suppose standard temperature and pressure, 1 mol = 22.4 liters.

33.6 liters* 1mol/22.4liters = 1.5 mols.

Molar mass of carbon dioxide: 12 g/mol + 2x16 g/mol = 44 g/mol

Mass of 1.5 mols = 1.5mol * 44 g/mol = 66 g.

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Which substance represents a compound?(1) C(s) (3) CO(g)(2) Co(s) (4) O2(g)

Answers

The substance that represents a compound among the given options is CO. The correct answer is (3) CO(g)

From the question,

We are to determine which of the given substances is a compound.

First, we will define a compound

A compound is a chemical species that is formed when two or more atoms join together chemically, with covalent or ionic bonds.

A compound is a substance that contains atoms of two or more different elements, and these atoms are chemically joined together

NOTE: A molecule consisting of atoms of only one element is NOT a compound.

Among the given options, only CO satisfies the definition of a compound, because it contains two different elements, Carbon (C) and Oxygen (O).

Hence, the substance that represents a compound among the given options is CO. The correct answer is (3) CO(g)

Learn more here: brainly.com/question/12862037

C = Carbon
CO = Carbon Monoxide
Co = Cobalt
O2 = Oxygen

So the answer is (3) CO

Nitrogen gas consists of _____. two separate nitrogen atoms a diatomic nitrogen atom a molecule of two nitrogen atoms a compound of nitrogen atoms

Answers

Nitrogen gas consists of a molecule of 2 nitrogen atoms.

Final answer:

Nitrogen gas consists of a molecule of two nitrogen atoms, known as a nitrogen-nitrogen triple bond, making it stable and unreactive. Diatomic nitrogen atoms or compounds of nitrogen atoms are not correct representations of nitrogen gas due to the bonding and structure of nitrogen gas.

Explanation:

Nitrogen gas consists of a molecule of two nitrogen atoms. In this molecule, the two nitrogen atoms are bound together in what is known as anitrogen-nitrogen triple bond, which is very strong. This is why nitrogen gas is very stable and unreactive under normal conditions.

Therefore, a diatomic nitrogen atom or a compound of nitrogen atoms is not a correct representation of nitrogen gas because these expressions do not accurately reflect the bonding and molecular structure of nitrogen gas.

Learn more about Nitrogen gas here:

brainly.com/question/34332615

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A sulfur atom has 16 protons and 16 electrons. If you add a proton to a sulfur atom, what have you done? Created an isotope of sulfur. Created a positively charged ion of sulfur. Created a negatively charged ion of sulfur. Converted the atom into a different element.

Answers

The addition of a proton to the sulfur atom has resulted in the formation of an isotope. Thus, option A is correct.

The addition of a proton to the nucleus has been resulted in the change in the atomic mass of the element without changing the atomic number.

The atomic mass has been the number of protons and neutrons present in the nucleus. The ions have been resulted when there has been a change in the number of electrons in the atom.

The isotopes have been the element that has been considered of the same atomic number with different atomic masses. The addition of a proton to the sulfur atom changes its atomic mass and thereby forms the isotope of sulfur. Thus, option A is correct.

For more information about the protons and electrons, refer to the link:

brainly.com/question/803445

Answer:

Created a positively charged ion of Sulfur

Explanation:

As the number of protons in Sulfur is more than the electrons in Sulfur, thus it'll be a positively charged ion of Sulfur

How many grams of sodium oxide can be produced when 55.3 g Na react with 64.3 g O2? Unbalanced equation: Na + O2 → Na2O

Show, or explain, all of your work along with the final answer.

Answers

Answer : The amount of sodium oxide produced is, 74.40 grams

Solution : Given,

Mass of sodium = 55.3 g

Mass of $O_2$ = 64.3 g

Molar mass of sodium = 23 g/mole

Molar mass of $O_2$ = 32 g/mole

Molar mass of $Na_2O$ = 61.9 g/mole

First we have to calculate the moles of sodium and oxygen.

Moles of Na = $\frac{\text{ given mass of Na}}{\text{ molar mass of Na}}= (55.3g)/(23g/mole)=2.404moles$

Moles of $O_2$ = $\frac{\text{ given mass of }O_2}{\text{ molar mass of }O_2}= (64.3g)/(32g/mole)=2.009moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction will be,

$4Na+O_2\rightarrow 2Na_2O$

From the balanced reaction we conclude that

4 moles of sodium react with 1 mole of oxygen

2.404 moles of sodium react with $(2.404)/(4)=0.601$ moles of oxygen

Excess moles of oxygen = 2.009 - 0.601 = 1.408 moles

That means sodium is a limiting reagent and oxygen is an excess reagent.

Now we have to calculate the moles of sodium oxide.

From the reaction we conclude that,

4 moles of sodium react to give 2 moles of sodium oxide

2.404 moles of sodium react to give $(2)/(4)* 2.404=1.202$ moles of sodium oxide

Now we have to calculate the mass of sodium oxide.

$\text{Mass of }Na_2O=\text{Moles of }Na_2O* \text{Molar mass of }Na_2O$

$\text{Mass of }Na_2O=(1.202moles)* (61.9g/mole)=74.40g$

Therefore, the amount of sodium oxide produced is, 74.40 grams

Given the two amounts of reactants, we get the limiting reactant between the two. We convert each to mole and divide them to their corresponding stoichiometric coefficient. we balance first above, that is 4Na+O2=2Na2O. hence, for Na that is 0.60 mole and oxygen is 2.00 mole. We follow the smaller amount, Na, hence the amount of sodium oxide in grams is 74.53 grams.

What is the percent by mass of water in Na2SOa 10H20?total mass of element in compoundUse%Elementx 100molar mass of compoundO 5.59%O 11.26%44.08%O 55.92%

Answers

Molar mass Na₂SO₄. 10H₂O = 322.19 g/mol

Molar mass H₂O = 18.0

% Element = molar mass / total mass x 100

% Element = 18 / 322,19 x 100

% Element = 5.59 %

Answer A

hope this helps!

Answer:

The answer is D.55.92%

Explanation:

The concentration of hydrogen peroxide (H2O2) can be determined by titrating it with an acidified MnO4− solution. The following is an unbalanced equation. MnO4− (aq) + H2O2 (aq) → O2 (g) + Mn2+ (aq)

(a) Balance the above redox reaction.
(b) Determine the concentration of H2O2 solution in molarity if 10.00 mL of this solution requires 20.00 mL of 1.5 M MnO4− for a complete reaction.