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3 years ago

What would be the balanced chemical equation for the complete combustion of butane ( C4H10 .)

Chemistry

1 answer:

Vilka [71]3 years ago

4 0

The balanced chemical equation b. 2 C₄H₁₀ + 13 O₂ ⇒ 8 CO₂ + 10 H₂O

<h3>Further explanation</h3>

Given

Butane (C₄H₁₀)

Required

Balanced equation

Solution

Formula

Hydrocarbon combustion reactions (specifically alkanes)

$\large {\box {\bold {C_nH _ (_2_n _ + _ 2_) + \dfrac {3n + 1} {2} O_2 \rightarrow nCO_2 + (n + 1) H_2O}}}$

In the combustion process, the compound in the reactants is Oxygen (O₂)

If the oxygen needed for combustion is sufficient (or excess) then the combustion results are in the form of CO₂ and H₂O, but if not enough, CO and H₂O will be obtained.

The only answer that contains O₂ in the reactants is option B

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A molecule is broken down into its constituent atoms. Do these atoms have the same properties as the molecule?

belka [17]

When a molecule is broken down into its constituent atoms, these atoms do not have the same properties as the molecule.

We can use an everyday molecule, such as water, H20, to show this property. Water is a liquid with unique properties that stem from its hydrogen bonding. On the other hand, its constituent atoms, hydrogen and oxygen, are not liquids, and have very different properties. Oxygen and hydrogen are both gases; hydrogen is dangerous and very flammable, while we breathe in oxygen throughout our lives. This example illustrates how the atoms that make up a molecule usually have different properties than the completed molecule.

Hope this helps!

4 0

4 years ago

Pls help<br> 25 points, thank you

denis23 [38]

Answer:

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7 0

3 years ago

Formulate a hypothesis about the stoichiometry of the reaction between NaCl and AgNO3.

MAXImum [283]

Answer:

AgCl + NaNO3 would be the products of the reaction between sodium chloride and silver nitrate.

The stoichiometry of this reaction is written below, and it is because for this reaction to be fulfilled the products have to be in equilibrium with the reactants, since the mass in the reaction is conserved and must be balanced in the amount of molecules that they react to each other.

Explanation:

NaCl + AgNO3 -------------- AgCl + NaNO3

3 0

4 years ago

What would happen if I removed a resistor from a parallel circuit? What would

barxatty [35]

Answer:

In a parallel circuit, current divides through resistors and current might be different depending upon the resistor and all resistors have the same potential difference. Therefore, if a parallel resistor was removed then the total resistance of the circuit will increase.

7 0

3 years ago

how many grams of calcium oxide will be produced in a closed vessel containing 20.0 kg of calcium and 20.0 kg of oxygen gas if t

sergejj [24]

Answer:

27984.1311 g

Explanation:

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

<u>For calcium :- </u>

Mass of calcium = 20.0 kg = 20000 g ( 1 kg = 1000 g )

Molar mass of calcium = 40.078 g/mol

Thus,

$Moles= \frac{20000\ g}{40.078\ g/mol}$

$Moles\ of\ calcium= 499.0269\ mol$

<u>For oxygen gas :- </u>

Mass of oxygen gas = 20.0 kg = 20000 g ( 1 kg = 1000 g )

Molar mass of oxygen gas = 31.999 g/mol

Thus,

$Moles= \frac{20000\ g}{31.999\ g/mol}$

$Moles\ of\ oxygen\ gas= 625.0195\ mol$

According to the given reaction:

$2Ca+O_2\rightarrow 2CaO$

2 moles of calcium reacts with 1 moles of oxygen gas

Also,

1 mole of calcium react with 1/2 mole of oxygen gas

So,

499.0269 mole of calcium react with $\frac{1}{2}\times 499.0269$ mole of oxygen gas

Moles of oxygen gas = 249.5135 moles

Available moles of oxygen gas = 625.0195 moles

Limiting reagent is the one which is present in small amount. Thus, calcium is limiting reagent.

The formation of the product is governed by the limiting reagent. So,

2 moles of calcium produces 2 moles of calcium oxide

So,

1 mole of calcium produces 1 mole of calcium oxide

Also,

499.0269 mole of calcium produces 499.0269 mole of calcium oxide

Moles of calcium oxide = 499.0269 moles

Molar mass of calcium oxide = 56.0774 g/mol

Mass of calcium oxide = Moles × Molar mass = 499.0269 × 56.0774 g = 27984.1311 g

<u>27984.1311 g of calcium oxide will be produced.</u>

8 0

4 years ago