Question

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

How many grams of CO₂ will be produced from 12.0 g of CH₄ and 133 g of O₂?

Answer 1

mass of CO_2 formed=
`0.75* 44g =33 g`

Step-by-step explanation:

First balance the chemical reaction:

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

molecular mass of
`CH_4=16g/Mol`

molecular mass of
`O_2=32g/Mol`

mass given of
`CH_4=12g`

mole of
`CH_4=12/16mol=0.75mol`

mass given of
`O_2=133g`

mole of
`O_2=133/32mol=4.16 mol`

from the above balanced equation:

1 mole of
`CH_4` need 2 mole of
`O_2` gas

therefore 0.75 mole of
`CH_4` will react with 1.5 mole of
`O_2` only

but we have 4.16 mole
`O_2` gas

hence
`O_2` will be the excess reagent and
`CH_4` will be the limiting eagent so production of
`CO_2` will depenf on the quantity of limiing reagent i.e.
`CH_4`

from the above balanced equation:

1 mole of
`CH_4` gives 1 mole of
`CO_2` on complete reacion with
`O_2`

hence,

0.75 mole of
`CH_4` gives 0.75 mole of
`CO_2` on complete reacion with
`O_2`

mass of CO_2 formed=
`0.75* 44g =33 g`