Question

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5.6 liters of methane gas is ignited in oxygen oxygen gas. Calculate the mass of CO2 formed.​

Answer 1

Explanation:

Combustion of methane is represented by:

CH_4(g)+2O_2(g)arrow CO_2(g)+2H_2O(g)CH

4

(g)+2O

2

(g)arrowCO

2

(g)+2H

2

O(g)

According to Avogadro's law, 1 mole of every gas occupies 22.4 Litres at STP.

Thus from the balanced chemical equation:

22.4 L of methane produces= 1 mole of carbon dioxide.

5.6 L of methane will produce=\frac{1}{22.4}\times 5.6=0.25 moles

22.4

1

×5.6=0.25moles of carbon dioxide.

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Answer 2

Answer:

The equation for the reaction:

CH 4 + 2O2 → CO2 + 2H2O

At S.T.P., 1 mol of gas = 22.4 L

So, 22.4 L of CH4 will give 22.4L of CO2

⇒ 1L of CH4 will give 1L of CO2

⇒ 5.6L of CH4 gives 5.6L of CO2

At S.T.P.

22.4L = 1 mol

⇒ 5.6 L = 5.6/22.4= 0.25 mol

Thus, 5.6L of methane will give 0.25 mol of carbon dioxide