Question

Propane (c3h8), a common fuel, reacts with oxygen to form carbon dioxide and water according to the equation below. c3h8 5o2 → 3co2 4h2o how many grams of oxygen are required to produce 37.15 g co2? 37.15 g co2 = g o2

Answer 1

To produce 37.15 g CO2, 44.96 g of O2 is required.

Step-by-step explanation:

To determine how many grams of oxygen are required to produce 37.15 g CO2, we need to use the balanced equation of the combustion reaction which is: C3H8 + 5O2 → 3CO2 + 4H2O.

From the equation, we can see that 3 moles of CO2 are produced for every 5 moles of O2.

The molar mass of CO2 is 44 g/mol, so 37.15 g CO2 is equal to 0.843 mol CO2 (37.15 g / 44 g/mol).

Using the mole-to-mole ratio from the balanced equation, we can calculate the moles of O2 required, which is (5/3) * 0.843 mol = 1.405 mol O2.

The molar mass of O2 is 32 g/mol, so 1.405 mol O2 is equal to 44.96 g O2 (1.405 mol * 32 g/mol).

Therefore, 37.15 g CO2 requires 44.96 g O2.

Answer 2

Answer: 45.02 (g O2)

Explanation: The person above me is wrong...but this is the right answer on edge! Ik cuz i just did this assignment and got 100% Hope this helps :D