C3H8 + 5O2 3CO2 + 4H2O
How many grams of oxygen are required to burn 7.0 g of C3H8?
How do we know the difference between products and reactants with no arrow???
1. Write and balance the equation.
2. Convert 7.0 g C3H8 to moles. moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles C3H8 to moles O2.
4. Convert moles O2 to grams. g = moles x molar mass.
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To determine how many grams of oxygen are required to burn 7.0 g of C3H8, you need to use the balanced chemical equation and the molar masses of the compounds involved.
The balanced chemical equation is:
C3H8 + 5O2 -> 3CO2 + 4H2O
From the equation, we can see that 1 mole of C3H8 reacts with 5 moles of O2.
1 mole of C3H8 has a molar mass of 44.1 g/mol.
So, 7.0 g of C3H8 is equal to 7.0 g / 44.1 g/mol = 0.158 moles of C3H8.
According to the stoichiometry of the equation, 0.158 moles of C3H8 would require 0.158 moles * 5 moles O2/mole C3H8 = 0.79 moles of O2.
Now, we need to find the mass of 0.79 moles of O2.
The molar mass of O2 is 32.0 g/mol.
So, 0.79 moles of O2 is equal to 0.79 moles * 32.0 g/mol = 25.28 g of O2.
Therefore, 7.0 g of C3H8 would require 25.28 g of O2 to burn.
To answer this question, we need to use the balanced chemical equation provided:
C3H8 + 5O2 -> 3CO2 + 4H2O
From the equation, we can see that 1 mole of C3H8 requires 5 moles of O2 to completely burn. We need to find the number of moles of C3H8 first and then use the stoichiometry from the equation to calculate the number of moles of O2.
The molar mass of C3H8 (propane) is 44.10 g/mol. To find the number of moles, we divide the given mass of C3H8 by its molar mass:
moles of C3H8 = mass of C3H8 / molar mass of C3H8
= 7.0 g / 44.10 g/mol
≈ 0.1585 mol
Now, using the stoichiometry from the balanced equation, we can determine the moles of O2 required to burn the given amount of moles of C3H8. From the equation, we know that 5 moles of O2 are required for every 1 mole of C3H8:
moles of O2 = moles of C3H8 × (5 moles of O2 / 1 mole of C3H8)
= 0.1585 mol × (5 mol O2 / 1 mol C3H8)
≈ 0.7925 mol
To find the mass of oxygen required, we need to multiply the moles of O2 by its molar mass. The molar mass of O2 is 32.00 g/mol:
mass of O2 = moles of O2 × molar mass of O2
= 0.7925 mol × 32.00 g/mol
≈ 25.36 g
Therefore, approximately 25.36 grams of oxygen are required to burn 7.0 grams of C3H8.