Question

Calculate the amount of carbon dioxide formed by the complete combustion of 80g of methane as per the
reaction:
CH4 (g) + 2O2 (g) CO2 (g) + 2 H2O (g)
(Atomic mass of C = 12.01u, H = 1.008u, O = 16u)

Answer 1

Answer:

CH4 (16g)   +     2O2 (64g)      =    CO2 (44g)    + 2H2O (36g)

1 mole                 2 mole                      1 mole           2 mole

amt of CO2 required for complete combustion of 1 mole of CH4   = 44g

amount of CO2 required for complete combution of 80 g of CH4  = ( 80/16 ) * 44g

​                                                                                                          = 5*44

                                                                                                         = 220 g

Explanation:

Answer 2

Answer:

The amount of Carbon dioxide formed is 76.93g .

Explanation:

Given

Mass of methane = 80g

Molar mass of methane = 16g/ mole

Molar mass of Carbon dioxide = 14.026

First calculate the moles of CH4-

Moles of CH4= Given mass of CH4

Molar mass of CH4

= 80 = 5 moles

16

Balance chemical reaction

CH4(g) + 2O2→CO2+2H2O

From the reaction ,we conclude that-

1 mole of methane react to give 1 mole of CO2-

5 moles of methane react to give 5 moles of carbon dioxide

To calculate the mass of carbon dioxide -

Mass of carbon dioxide= moles of carbon dioxide x molar mass of carbon dioxide

Mass of carbon dioxide- 5 moles x 44 g/ mole

Mass of carbon dioxide= 220 g

The amount of Carbon dioxide formed is 76.93g .

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