Question

Using this equation: C3H8 + 302 - 3C02 + 4H2
How many grams of CO2 are produced when we react 1.03 grams of Oxygen?

Answer 1

To calculate the grams of CO2 produced, we first need to determine the amount of propane (C3H8) consumed in the reaction. From the equation, we can see that 3 moles of O2 react with 1 mole of C3H8.

1 mol O2 = 32 g
32g of O2 corresponds to 3 moles of O2
1.03g O2 corresponds to 1.03g * 3 moles / 32g = 0.09 moles O2

Using the mole ratio from the balanced equation, we determine the moles of CO2 produced:

1 mol O2 : 3 moles CO2
0.09 moles O2 : x moles CO2
x = 0.09 moles O2 * 3 mol CO2 / 1 mol O2 = 0.27 moles CO2

Now, calculate the grams of CO2 produced:

1 mol CO2 = 44 g
0.27 moles * 44 g / mol = 11.88 grams of CO2

Therefore, when 1.03 grams of Oxygen reacts, 11.88 grams of CO2 are produced.