Question

Consider the reaction ch4 + 2 o2 → co2 + 2 h2o exactly 14.5 moles of co2 are produced upon reaction of 34.6 moles of o2 and how many moles of ch4?

Answer 1

14.5 moles  
The balanced reaction indicates that for every molecule of CH4 consumed, one molecule of CO2 is produced. So in order to produce 14.5 moles of CO2, you need exactly 14.5 moles of CH4. As a side note, only 2 molecules of O2 is needed per molecule of CO2 produced. So you need 14.5*2 = 29 moles of O2. So in this question, we were provided with an excess of O2.

Answer 2

Answer:

14.5 moles of methane had produced 14.5 moles of carbon dioxide.

Explanation:

$CH_4 + 2O_2\rightarrow CO_2 + 2H_2O$

Moles of oxygen gas = 34.6 moles

According to reaction 1 mole of methane reacts with 2 moles of oxygen.

The 34.6 moles of oxygen gas will react with :

$\frac{1}{2}\times 34.6 moles=17.3 mol$ of methane

According to reaction 1 mole of methane gives 1 moles of carbon dioxide .

The 14.5 moles of carbon dioxide gas will be obtained from:

$\frac{1}{1}\times 14.5 moles=14.5 mol$ of methane

As we can see that oxygen is present in an excess , which means that formation of carbon dioxide would have depend upon moles of methane.

So, the moles of methane used to form 14.5 moles of carbon dioxide will be:

$\frac{1}{1}\times 14.5 moles=14.5 mol$ of methane