Question

How many moles of methane are required to produce 11g Co2 after combustion
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Answer 1

Answer:

CH4 + 2O2 -> CO2 + 2H2O

GRAM MOLECULAR MASS OF CO2 = 12 +2(16) = 44g

From the reaction it is clear that 1 mole of methane on complete combustion produces 44g (1 mole) of carbon dioxide.

therefore moles of CH4 required to produce 22g of CO2 are:

(22) * (1/44) = 1/2 moles

Answer 2

Answer:

0.25 moles of methane is required to produce 11g of $CO_2$ after combustion.

Explanation:

When methane is burn in the presence of oxygen then the carbon dioxide gas releases.

$CH_4+O_2 \rightarrow CO_2 + 2H_2O$

Now,

The gram molecular mass of $CO_2$ is,

= 12 + 2(16)

= 12 + 32

= 44 g/mol

From the reaction,

On the complete combustion, 1 mole of methane produce 44 grams of carbon dioxide, i.e.,

44 grams of $CO_2$ produce = 1 mole of methane.

1 gram of $CO_2$ produce = 1/44 moles of methane.

Then,

11 grams of $CO_2$ produce = $\frac{1}{44}\times 11$

                                          = 0.25 moles of methane

Therefore, 0.25 moles of methane is required to produce 11g of $CO_2$ after combustion.

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