What mass of propane (C3H8) is needed to produce 346 g carbon dioxide in the following reaction?
C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g)
A. 346 g C3H8
B. 115 g C3H8
C. 5075 g C3H8
D. 1.86 g C3H8
You have the balanced equation.
Convert 346 g CO2 to mols. mol = g/molar mass
Using the coefficients in the balanced equation, convert mols CO2 to mols propane.
Now convert mols propane to grams. g = mols x molar mass. Post your work if you get stuck.
115 g c3hg
To find the mass of propane (C3H8) needed to produce 346 g of carbon dioxide (CO2), you need to use the stoichiometry of the balanced chemical equation.
The balanced chemical equation is:
C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g)
From the equation, you can see that the molar ratio between C3H8 and CO2 is 1:3. This means that for every 1 mole of C3H8, 3 moles of CO2 are produced.
To find the mass of C3H8 needed, you can follow these steps:
Step 1: Calculate the number of moles of CO2 produced using the given mass.
m(CO2) = 346 g
First, convert the mass of CO2 to moles using its molar mass. The molar mass of CO2 is approximately 44 g/mol.
n(CO2) = m(CO2) / M(CO2) = 346 g / 44 g/mol ≈ 7.86 mol
Step 2: Use the mole ratio from the balanced chemical equation to determine the moles of C3H8.
From the balanced chemical equation, the mole ratio between C3H8 and CO2 is 1:3. So, for every 3 moles of CO2, we need 1 mole of C3H8.
n(C3H8) = (7.86 mol CO2) * (1 mol C3H8 / 3 mol CO2) ≈ 2.62 mol C3H8
Step 3: Calculate the mass of C3H8 using its molar mass.
The molar mass of C3H8 is approximately 44 g/mol.
m(C3H8) = n(C3H8) * M(C3H8) = 2.62 mol * 44 g/mol ≈ 115 g
Therefore, the mass of propane (C3H8) needed to produce 346 g of carbon dioxide (CO2) is approximately 115 g.
The correct answer is B. 115 g C3H8.