What mass of carbon dioxide is produced from the complete combustion of 2.90×10−3 g of methane?

2015-09-14T12:10:12-04:00

When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is CH4(g)+O2(g)→CO2(g)+H2O(g) This type of reaction is referred to as a complete combustion reaction. What mass of carbon dioxide is produced from the complete combustion of 9.00×10−3 g of methane? Express your answer with the appropriate units. What mass of water is produced from the complete combustion of 9.00×10−3 g of methane? Express your answer with the appropriate units. What mass of oxygen is needed for the complete combustion of 9.00×10−3 g of methane?

Express your answer with the appropriate units.

2015-09-16T03:18:55-0400

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We first need to write down the balanced equation for this reaction, that is

#CH_4(g)+2O_2(g)->CO_2(g)+2H_2O(g)#

As we can see here, the mole ratio between methane #(CH_4)# and carbon dioxide #(CO_2)# is #1:1#, i.e. one mole of methane will produce one mole of carbon dioxide in return.

In here, we burn #2.6*10^-3 \ "g"# of methane. So, we need to convert that amount into moles.

Methane has a molar mass of #16 \ "g/mol"#. So, in here, we have

#(2.6*10^-3cancel"g")/(16cancel"g""/mol")=0.0001625~~1.63*10^-4 \ "mol of" \ CH_4#

Since the mole ratio between the two compounds is #1:1#, then we will also produce #1.63*10^-4# moles of carbon dioxide.

Carbon dioxide has a molar mass of #44 \ "g/mol"#.

So, the mass of carbon dioxide produced is

#1.63*10^-4cancel"mol"*44 \ "g/"cancel"mol"=0.007172 \ "g"#

Now, we can convert into scientific notation, which will be

#7.17*10^-3 \ "g"#

Since this answer asks us to give the answer in appropriate units, I suggest you use milligrams as the answer, as #1 \ "g"=1*10^3 \ "mg"#.

#<=>7.17*10^-3 \ "g" = 7.17 \ "mg"#