Calculate the mass of butane needed to produce 46.8 g
of carbon dioxide.
Just follow the same procedure for the earlier problem I worked for you. Post your work if you get stuck.
https://www.jiskha.com/questions/1849656/calculate-the-mass-of-water-produced-when-3-64-g-of-butane-reacts-with-excess-oxygen
Why did the butane go to the gym?
To get in shape for all that burning! 💪
But let's get serious for a second and calculate the mass of butane needed to produce 46.8 g of carbon dioxide.
First, we need to know the balanced chemical equation for the combustion of butane:
C4H10 + 13/2 O2 → 4 CO2 + 5 H2O
From the equation, we can see that 1 mole of butane (C4H10) produces 4 moles of carbon dioxide (CO2).
Now, we need to calculate the number of moles of carbon dioxide produced:
Number of Moles = Mass / Molar Mass
The molar mass of carbon dioxide (CO2) is approximately 44 g/mol.
Number of Moles of CO2 = 46.8 g / 44 g/mol ≈ 1.0636 mol
Since 1 mole of butane produces 4 moles of carbon dioxide, we can set up a proportion:
Number of Moles of Butane / 1 mol = 1.0636 mol / 4 mol
Simplifying this equation, we find:
Number of Moles of Butane ≈ 0.2659 mol
Finally, we can calculate the mass of butane needed:
Mass of Butane = Number of Moles of Butane × Molar Mass of Butane
The molar mass of butane (C4H10) is approximately 58.12 g/mol.
Mass of Butane = 0.2659 mol × 58.12 g/mol ≈ 15.46 g
So, approximately 15.46 grams of butane is needed to produce 46.8 grams of carbon dioxide. Remember, don't try to burn butane without proper supervision!
To calculate the mass of butane needed to produce a certain amount of carbon dioxide, we need to use the balanced chemical equation for the reaction of butane (C4H10) with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O):
2 C4H10 + 13 O2 -> 8 CO2 + 10 H2O
From the balanced equation, we see that it takes 2 moles of butane (C4H10) to produce 8 moles of carbon dioxide (CO2).
First, we need to calculate the moles of carbon dioxide produced from the given mass of 46.8 g. We can use the molar mass of carbon dioxide (44.01 g/mol) to convert from grams to moles:
Moles of CO2 = Mass of CO2 / Molar mass of CO2
Moles of CO2 = 46.8 g / 44.01 g/mol
Moles of CO2 ≈ 1.063 mol
Since the balanced equation shows that 2 moles of butane produce 8 moles of carbon dioxide, we can set up a ratio:
2 moles of butane / 8 moles of CO2 = x moles of butane / 1.063 moles of CO2
To find the moles of butane required, we can rearrange the equation:
x moles of butane = 2 moles of butane * (1.063 moles of CO2 / 8 moles of CO2)
x moles of butane ≈ 0.266 mol
Finally, we can calculate the mass of butane needed using the molar mass of butane (58.12 g/mol):
Mass of butane = Moles of butane * Molar mass of butane
Mass of butane = 0.266 mol * 58.12 g/mol
Mass of butane ≈ 15.43 g
Therefore, approximately 15.43 grams of butane are needed to produce 46.8 grams of carbon dioxide.
Butane, C4H10, reacts with oxygen, O2, to form water, H2O, and carbon dioxide, CO2, as shown in the following chemical equation:
2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g)
molar mass of butane is: 58.12