How many grams of carbon dioxide are produced in the combustion of 2.60 grams of ethane?

Question

How many grams of carbon dioxide are produced in the combustion of 2.60 grams of ethane?

Answer 1

1 C2H6 --> 2 CO2

using molar  masses:

2.60 g C2Hg @ (2 moles) (44.0g/mol CO2) / 30.07 g/mol = 7.61

your answer is 7.61 g CO2

Answer 2

2(C2H6) + 7(O2) ---> 4(CO2) + 6(H2O)

molar ration of CO2 to Ethane for this reaction: 4:2 or 2

2.60 g of Ethane = 0.087 moles

0.087 moles x 2 = 0.173 moles

0.173 moles x 44 g/mol (molecular weight of CO2) = 7.62 g

Answer 3

First, let's write the combustion equation:

2C2H6 + 7O2 -> 4CO2 + 6H2O

Now, we need to determine how many moles of ethane are equivalent to 2.60 grams. The molecular weight of ethane is 30.07 g/mol, so:

(2.60 g) * (1 mol / 30.07 g) = 0.0865 moles of ethane

We can use the stoichiometric ratio from the combustion equation to relate the moles of ethane to the moles of carbon dioxide:

Twice as much CO2 is produced as ethane is used:

2 * (0.0865) = 0.173 moles carbon dioxide

Using the molecular weight of carbon dioxide as 44.0095 g/mol:

(44.0095 g / mol) * (0.173 mol) = 7.61 grams of carbon dioxide