Consider the following balanced equation for the combustion of methane, a compon

Question

Consider the following balanced equation for the combustion of methane, a component of natural gas.
CH4(g)+2O2(g)?CO2(g)+2H2O(g)Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed.

A. Complete the first row.

B. Complete the second row.

C. Complete the third row.

D. Complete the fourth row.

E. Complete the fifth row

F. Complete the sixth row.

Mass CH4 Mass O2 Mass CO2 Mass H2O _____ 3.07 g _____ _____ 19.32 g _____ _____ _____ _____ _____ _____ 14.32 g _____ _____ 3.84 g _____ 3.58 kg _____ _____ _____ _____ _____ 1750 kg _____

Explanation / Answer

CH4(g) + 2 O2 (g) ---------------> CO2 (g) + 2 H2O (g)

16 g          64 g                              44.01 g      36 g

   ?              3.07 g                               ?               ?

A)

16 g CH4 --------------> 64 g O2

??          --------------> 3.07 g O2

mass of CH4 = 3.07 x 16 / 64

                     = 0.768 g

mass of CO2 = 3.07 x 44.01 / 64

                      = 2.11 g

mass of H2O = 3.07 x 36 / 64

                      = 1.73 g

Mass CH4 Mass O2 Mass CO2 Mass H2O 0.768 g 3.07 g 2.11 g 1.73 g 19.32 g 77.28 g 53.14 g 43.47 g 6.36 g 25.46 g 17.51 g 14.32 g 1.40 g 5.58 g 3.84 g 3.14 g 3.58 kg 14.32 kg 9.85 kg 8.06 kg 636 kg 2545 kg 1750 kg 1432 kg

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