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ASHA 777 [7]
3 years ago
11

1. Balance the equation, then answer the following based on the equation

Chemistry
1 answer:
Artemon [7]3 years ago
4 0

Answer:

Q1. a) 4Al + 3O₂ ➟ 2Al₂O₃

b) 7.4 moles

c) 11.1 moles

Explanation:

To balance an equation, ensure that the total number of atoms of each element on both sides are equal.

Al + O₂ ➟ Al₂O₃

On the left side of the arrow, you would find the reactants while the product(s) is found on the left hand side.

<u>Reactants</u>

Al atoms: 1

O atoms: 2

<u>Product</u>

Al atoms: 2

O atoms: 3

After balancing,

4Al + 3O₂ ➟ 2Al₂O₃

We have 4 Al atoms and 6 O atoms on both sides.

b) The balanced equation tells us the mole ratio of Al to Al₂O₃.

Al: Al₂O₃

= 4: 2 (÷2 throughout)

= 2: 1

This means that for every 1 mole of Al₂O₃, 2 moles of Al is needed.

Since we need 3.7 moles of Al₂O₃,

number of moles of Al needed

= 2×3.7

= 7.4

c) 4Al + 3O₂ ➟ 2Al₂O₃

For every 4 moles of Al, 3 moles of O are needed.

For each mole of Al,

number of moles of O needed

= 3÷4

= 0.75

For 14.8 moles of Al,

number of moles of O required

= 0.75 ×14.8

= 11.1

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Liquid hexane
maks197457 [2]

<u>Answer:</u> The mass of H_2O produced is 2.52 g

<u>Explanation:</u>

The number of moles is defined as the ratio of the mass of a substance to its molar mass.  The equation used is:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}} ......(1)

  • <u>For hexane:</u>

Given mass of hexane = 1.72 g

Molar mass of hexane = 86.18 g/mol

Putting values in equation 1, we get:

\text{Moles of hexane}=\frac{1.72g}{86.18g/mol}=0.020mol

  • <u>For oxygen gas:</u>

Given mass of oxygen gas = 8.0 g

Molar mass of oxygen gas= 32 g/mol

Putting values in equation 1, we get:

\text{Moles of water}=\frac{8.0g}{32g/mol}=0.25mol

The chemical equation for the combustion of hexane follows:

2C_6H_{14}+19O_2\rightarrow 12CO_2+14H_2O

By stoichiometry of the reaction:

If 2 moles of hexane reacts with 19 moles of oxygen gas

So, 0.020 moles of hexane will react with = \frac{19}{2}\times 0.020=0.19mol of oxygen gas

As the given amount of oxygen gas is more than the required amount. Thus, it is present in excess and is considered as an excess reagent.

Thus, hexane is considered a limiting reagent because it limits the formation of the product.

By the stoichiometry of the reaction:

If 2 moles of hexane produces 14 moles of H_2O

So, 0.020 moles of hexane will produce = \frac{14}{2}\times 0.020=0.14mol of H_2O

We know, molar mass of H_2O = 18 g/mol

Putting values in above equation, we get:

\text{Mass of }H_2O=(0.14mol\times 18g/mol)=2.52g

Hence, the mass of H_2O produced is 2.52 g

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Answer:

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Explanation:

11.340+2.268= 13.608

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