Question

How many grams of CO2 will be produced when 8.50 g of methane react with 15.9 g of O2, according to the following reaction? 
CH4(g) +2O2(g)→CO2(g) +2H2O(g) 




Answer 1

The amount of $CO_2$ that would be produced will be 10.93 g

Stoichiometric calculations

From the equation of the reaction, the mole ratio of methane to oxygen is 1:2.

Mole of 8.50 g methane = 8.50/16.04 = 0.53 moles

Mole of 15.9 g oxygen = 15.9/32 = 0.4969 moles

Thus, methane is in excess while oxygen is limiting.

Mole ratio of $O_2$ and  $CO_2$  = 2:1

Equivalent mole of  $CO_2$  = 0.4969/2 = 0.25 moles

Mass of 0.25 moles  $CO_2$  = 0.25 x 44.01 = 10.93 g

More on stoichiometric calculations can be found here: brainly.com/question/27287858

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