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.

Mass CH4 Mass O2 Mass CO2 Mass H2O

_____ 2.67 g _____ _____

16.32 g _____ _____ _____

_____ _____ _____ 15.32 g

_____ _____ 3.64 g _____

2.78 kg _____ _____ _____

_____ _____ 1950 kg _____

Explanation / Answer

1.

Mass of O2 given = 2.67 g

number of moles of O2 = mass/molar mass

= 2.67/32

=0.0834 mol

number of moles of CH4 required = 0.0834/2 = 0.0417 mol

Mass of CH4 = number of moles * molar mass

= 0.0417*16

=0.67 g

number of moles of CO2 = 0.0417 mol

Mass of CO2= number of moles * molar mass

= 0.0417*44

= 1.83 g

number of moles of H2O = 0.0834 mol

Mass of H2O= number of moles * molar mass

= 0.0834*18

= 1.50 g

I have answered about 1st row. Please fill other row accordingly

This question is very lengthy

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