The balanced chemical equation for the combustion of propane (C₃H₈)is given below.How many grams of carbon dioxide (CO₂)are released when 35 g of propane are burned in the presence of excess oxygen? C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O A) 0.80 g B) 12 g C) 35 g D) 105 g E) 1,500 g

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The balanced chemical equation for the combustion of propane (C3H8) is: C3H8 + 5O2 → 3CO2 + 4H2O. To find the grams of CO2 produced from 35 g of propane, first, calculate the molar mass of propane (C3H8) which is (3*12.01 + 8*1.01) = 44.11 g/mol. Then, find the moles of propane by dividing the mass of propane by its molar mass: 35 g / 44.11 g/mol = 0.793 mol of C3H8. Since the reaction produces 3 moles of CO2 for every mole of C3H8, the moles of CO2 produced are 3 * 0.793 = 2.379 mol. The molar mass of CO2 is (12.01 + 2*16.00) = 44.01 g/mol. Therefore, the mass of CO2 produced is 2.379 mol * 44.01 g/mol = 104.7 g, which rounds to 105 g.

The Balanced Chemical Equation for the Combustion of Propane (C3H8)is

The Balanced Chemical Equation for the Combustion of Propane (C₃H₈)is