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Find out the amount of [tex]$CO_2$[/tex] produced in moles by the combustion of 3.29 g of [tex]$CH_4$[/tex].

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To determine the amount of [tex]\( CO_2 \)[/tex] produced from the combustion of 3.29 moles of [tex]\( CH_4 \)[/tex] (methane), follow these steps:

1. Understand the chemical reaction:
The combustion of methane can be represented by the balanced chemical equation:
[tex]\[ CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O \][/tex]
This equation tells us that one mole of methane ([tex]\( CH_4 \)[/tex]) reacts with two moles of oxygen ([tex]\( O_2 \)[/tex]) to produce one mole of carbon dioxide ([tex]\( CO_2 \)[/tex]) and two moles of water ([tex]\( H_2O \)[/tex]).

2. Determine the mole ratio:
From the balanced equation, we see that 1 mole of [tex]\( CH_4 \)[/tex] produces 1 mole of [tex]\( CO_2 \)[/tex]. This is a straightforward 1:1 ratio.

3. Apply the mole ratio to find moles of [tex]\( CO_2 \)[/tex] produced:
Given that we have 3.29 moles of [tex]\( CH_4 \)[/tex], we use the 1:1 mole ratio to find the moles of [tex]\( CO_2 \)[/tex] produced.
Since 1 mole of [tex]\( CH_4 \)[/tex] produces 1 mole of [tex]\( CO_2 \)[/tex], 3.29 moles of [tex]\( CH_4 \)[/tex] will produce 3.29 moles of [tex]\( CO_2 \)[/tex].

Thus, the amount of [tex]\( CO_2 \)[/tex] produced from the combustion of 3.29 moles of [tex]\( CH_4 \)[/tex] is 3.29 moles of [tex]\( CO_2 \)[/tex].
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