What mass of propane (C3H8) is needed to produce 346g carbon dioxide in the following reaction?
C3H8(g)+5O2(g)->3CO2(g)+4H2O(g)
A. 68.8gS
B. 3.07gS
C. 13.5gS
D. 41.0gS
Well, let's see. According to the balanced chemical equation, we need 1 mole of C3H8 to produce 3 moles of CO2. To find the mass of propane needed, we need to convert grams of CO2 to moles, and then use the mole ratio to find the moles of C3H8 needed.
346g CO2 * (1 mole CO2/44.01g CO2) * (1 mole C3H8/3 moles CO2) * (44.01g C3H8/1 mole C3H8) ≈ 67.81g C3H8
So, the mass of propane needed is approximately 67.81g. However, none of the answer choices match exactly. I guess you could say this question has us all a little "propaned", doesn't it? But if I had to choose the closest option, I'd go with A. 68.8gS. It's not a perfect match, but it's the closest we've got.
To determine the mass of propane needed to produce 346g of carbon dioxide, we need to use stoichiometry.
The balanced equation shows that 1 mole of C3H8 produces 3 moles of CO2. To convert from moles to grams, we need to know the molar mass of C3H8 and CO2.
Molar mass of C3H8 = (3 x 12.01 g/mol) + (8 x 1.01 g/mol) = 44.11 g/mol
Molar mass of CO2 = (1 x 12.01 g/mol) + (2 x 16.00 g/mol) = 44.01 g/mol
Now, we can set up a ratio using the molar masses and the stoichiometric coefficients:
(44.11 g C3H8) / (3 mol CO2) = (x g C3H8) / (346 g CO2)
Cross-multiplying and solving for x gives us:
x = (44.11 g C3H8 * 346 g CO2) / (3 mol CO2)
= 5107.54 g C3H8
Therefore, the mass of propane needed to produce 346g of carbon dioxide is approximately 5107.54 grams.
None of the answer choices provided matches this value. It is possible there was a calculation mistake in the problem or answer choices.
To determine the mass of propane (C3H8) needed to produce a certain mass of carbon dioxide (CO2), you need to set up a stoichiometry calculation using the balanced chemical equation.
First, find the molar masses of propane (C3H8) and carbon dioxide (CO2):
Molar mass of C3H8 = (3 × molar mass of C) + (8 × molar mass of H)
= (3 × 12.01 g/mol) + (8 × 1.01 g/mol)
= 44.11 g/mol
Molar mass of CO2 = (1 × molar mass of C) + (2 × molar mass of O)
= (1 × 12.01 g/mol) + (2 × 16.00 g/mol)
= 44.01 g/mol
Next, calculate the number of moles of carbon dioxide produced using the given mass:
Moles of CO2 = mass of CO2 / molar mass of CO2
= 346 g / 44.01 g/mol
≈ 7.861 mol
According to the balanced equation, the molar ratio between C3H8 and CO2 is 1:3. This means that for every 1 mole of propane, 3 moles of carbon dioxide are produced. Therefore, you can determine the number of moles of propane required by multiplying the moles of CO2 by the ratio:
Moles of C3H8 = moles of CO2 × (1 mol C3H8 / 3 mol CO2)
= 7.861 mol × (1/3)
≈ 2.620 mol
Finally, calculate the mass of propane needed using the molar mass of propane:
Mass of C3H8 = moles of C3H8 × molar mass of C3H8
= 2.620 mol × 44.11 g/mol
≈ 115.6 g
Therefore, the correct answer is D. 41.0gS.