Question

26. How many moles of methane are required to produce 22 g CO, for combustion? Hint : CH, + 202 → CO, + 2H20​

Answer 1

Answer:

0.5 moles of Methane are required.

Explanation:

First, we must make this a balanced reaction. The balanced reaction will be:

$CH_{4} + 2O_{2} -----> CO_{2} \ + 2H_{2}O$, as given in the question.

This provides us with the following information:

One mole of Methane must be combined with two moles of Oxygen gas to form one mole of Carbon Dioxide and two moles of Water.

So, we know that one mole of Methane forms one mole of Carbon Dioxide.

We shall now find how many moles of Carbon Dioxide is 22g.

Molecular mass of Carbon Dioxide = 12 + (2 × 16) = 44u

Gram molecular mass = 44g

Number of moles = $\frac{Given\ mass}{Gram\ molecular\ mass}$ = $\frac{22}{44}$ = 0.5 moles of Carbon Dioxide.

Thus, 0.5 moles of Methane will be required to form 22g of Carbon Dioxide.

I hope this helps!!

Regards,

Lilac584