Question

Read the given chemical reaction.

C2H6 + O2 CO2 + H2O

How many moles of CO2 are produced during the complete combustion of 3. 6 moles of C2H6?

O 1. 8 moles

O 4. 4 molele

O 7. 2 moles

O 9. 2 moles

Answer 1

So the correct answer is option (C) 7.2 moles.

Step-by-step explanation:

According to the balanced chemical equation for the combustion of C2H6:

C2H6 + O2 → CO2 + H2O

The stoichiometric coefficients tell us that 1 mole of C2H6 reacts with 3 moles of O2 to produce 2 moles of CO2.

To determine how many moles of CO2 are produced from 3.6 moles of C2H6, we need to use stoichiometry. We can set up a proportion using the stoichiometric coefficients from the balanced equation:

3.6 mol C2H6 / 1 x 2 mol CO2 / 1 mol C2H6 = 7.2 mol CO2

Therefore, 7.2 moles of CO2 are produced during the complete combustion of 3.6 moles of C2H6.

So the correct answer is option (C) 7.2 moles.

Answer 2

During the complete combustion of 3.6 moles of
`\(C_2H_6\)`, 7.2 moles of
`\(CO_2\)` are produced. The correct answer is 7.2 moles.

The balanced chemical equation for the complete combustion of
`\(C_2H_6\)` is:

`\[2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O.\]`

This equation indicates that 2 moles of
`\(C_2H_6\)` react to produce 4 moles of
`\(CO_2\)`. Therefore, the mole ratio between
`\(C_2H_6\) and \(CO_2\)` is 2:4 (or simplified, 1:2).

If 3.6 moles of
`\(C_2H_6\)` are completely combusted, we can use the mole ratio to determine the moles of
`\(CO_2\)` produced.

`\[ \text{Moles of } CO_2 = \frac{\text{Moles of } C_2H_6 * (\text{Moles of } CO_2/\text{Moles of } C_2H_6)}{1} \]`

`\[ \text{Moles of } CO_2 = (3.6 * 2)/(1) = 7.2 \text{ moles.} \]`

Therefore, during the complete combustion of 3.6 moles of
`\(C_2H_6\)`, 7.2 moles of
`\(CO_2\)` are produced. The correct answer is 7.2 moles.