Consider the following reactions,
`CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(g)`
How many moles of methane are required to produce 22g of `CO_(2)`(g) after combustion?

Explanation

According to the chemical equation,
` CH_(4) (g) +2O_(2) (g) to CO_(2) (g) +2 h_(2)O(g) `
44 g `CO_(2) ` (g) is obtained from 1 mol of `CH_(4)(g) ` ]
Number of moles of `CO_(2)(g) `
`=22 g CO_(2)(g) xx (1 mol CO_(2) (g))/(44 g CO_(2) (g) )`
`=0.5 ml CO_(2)` (g)
Hence , 0.5 ` CO_(2) (g) ` would be obtained from 0.5 mol `CH_(4) (g) ` or 0.5 mol of `CH_(4) (g) ` would be required to produce 22 g ` CO_(2) (g) `