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Given:
[tex]\[
CH_4 + 2 O_2 \rightarrow CO_2 + 2 H_2O
\][/tex]

In the chemical reaction, if 10 moles of [tex]\(H_2O\)[/tex] are produced, [tex]\(\square\)[/tex] moles of [tex]\(CO_2\)[/tex] are also produced.

Sagot :

GinnyAnswer
To solve this problem, we need to analyze the stoichiometric relationship in the chemical reaction:

[tex]\[ \text{CH}_4 + 2 \text{O}_2 \rightarrow \text{CO}_2 + 2 \text{H}_2\text{O} \][/tex]

According to the balanced equation:

- 1 mole of [tex]\( \text{CH}_4 \)[/tex] reacts with 2 moles of [tex]\( \text{O}_2 \)[/tex] to produce 1 mole of [tex]\( \text{CO}_2 \)[/tex] and 2 moles of [tex]\( \text{H}_2\text{O} \)[/tex].

The stoichiometric ratio between [tex]\( \text{CO}_2 \)[/tex] and [tex]\( \text{H}_2\text{O} \)[/tex] is 1:2. This means that for every 2 moles of [tex]\( \text{H}_2\text{O} \)[/tex] produced, 1 mole of [tex]\( \text{CO}_2 \)[/tex] is produced.

Given that 10 moles of [tex]\( \text{H}_2\text{O} \)[/tex] are produced, we can use this ratio to determine the moles of [tex]\( \text{CO}_2 \)[/tex] produced:

[tex]\[ \frac{\text{moles of H}_2\text{O}}{2} = \frac{10}{2} = 5 \text{ moles of CO}_2 \][/tex]

Therefore, 5 moles of [tex]\( \text{CO}_2 \)[/tex] are produced.

So, the correct answer is:
[tex]\[ \boxed{5} \][/tex]
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