Final answer:
The balanced equation for the combustion of C2H6 is 2C2H6 + 7O2 → 4CO2 + 6H2O. To calculate the missing grams, we need to use the molar masses of CO2 and C2H6. Given that 30 g of C2H6 is consumed in the reaction, the grams of CO2 produced is 175.37 g.
Step-by-step explanation:
The balanced chemical equation for the combustion of C2H6 is:
2C2H6 + 7O2 → 4CO2 + 6H2O
To calculate the missing grams, we need to use the molar masses of CO2 and C2H6. The molar mass of CO2 is 44.009 g/mol, and the molar mass of C2H6 is 30.07 g/mol.
Given that 30 g of C2H6 is consumed in the reaction, we can use the ratio of the coefficients in the balanced equation to find the moles of CO2 produced:
Moles of CO2 = (4/2) * (30 g / 30.07 g/mol) = 3.98 mol
Finally, we can calculate the grams of CO2 produced:
Grams of CO2 = 3.98 mol * 44.009 g/mol = 175.37 g