When O2 reacts with C2H6, according to the equation: 2 C2H6 + 7 O2 = 4 CO2 + 6 H2O, how much CO2 is produced from 60.0 g of C2H6?

Here is a worked example of a stoichiometry problem.

http://www.jiskha.com/science/chemistry/stoichiometry.html

144

To determine the amount of CO2 produced from 60.0 g of C2H6, we can use stoichiometry. Stoichiometry is a calculation method that allows us to relate the amounts of reactants and products in a chemical equation.

First, we need to determine the number of moles of C2H6. The molar mass of C2H6 is 30.07 g/mol (2*12.01 g/mol + 6*1.01 g/mol). We can calculate the moles of C2H6 by dividing the given mass by its molar mass:

60.0 g C2H6 * (1 mol C2H6 / 30.07 g C2H6) = 1.99 mol C2H6

According to the balanced equation, for every 2 moles of C2H6, 4 moles of CO2 are produced. Therefore, we can use this ratio to find the moles of CO2 produced.

1.99 mol C2H6 * (4 mol CO2 / 2 mol C2H6) = 3.98 mol CO2

Finally, we can convert the moles of CO2 to grams by multiplying it by the molar mass of CO2, which is 44.01 g/mol.

3.98 mol CO2 * (44.01 g CO2 / 1 mol CO2) = 175.6 g CO2

Therefore, 60.0 g of C2H6 will produce approximately 175.6 g of CO2.