When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 24.0 of carbon were burned in the presence of 76.8 of oxygen, 12.8 of oxygen remained unreacted. What mass of carbon dioxide was produced?
Oh, I love chemistry! It's like setting up a little carbon-oxygen dating game. So, we have 24.0 grams of carbon and 76.8 grams of oxygen. But uh-oh, it seems like our carbon isn't very good at flirting because it didn't snatch up all the oxygen. 12.8 grams of oxygen got left on the shelf. Poor oxygen, always looking for love. Anyway, let's find out how much carbon dioxide was actually formed.
To find the mass of carbon dioxide, we need to calculate the difference between the initial mass of oxygen and the final mass of oxygen. That's 76.8 grams minus 12.8 grams, which gives us 64.0 grams of oxygen that reacted.
Now, here comes the math magic: since the mass ratio of carbon to oxygen in carbon dioxide is 1:2, we need to double the mass of oxygen that reacted to find the mass of carbon dioxide. That means 64.0 grams of oxygen reacted will give us 128.0 grams of carbon dioxide.
So, after this little love affair between carbon and oxygen, we ended up with 128.0 grams of carbon dioxide. It's like a chemistry love story with a happy ending.
To find the mass of carbon dioxide produced, we need to determine the amount of oxygen that reacted with carbon and the amount of oxygen that remained unreacted.
1. Calculate the amount of oxygen that reacted with carbon:
Mass of oxygen reacted = Initial mass of oxygen - Mass of oxygen remaining unreacted
Mass of oxygen reacted = 76.8 g - 12.8 g
Mass of oxygen reacted = 64.0 g
2. Determine the amount of carbon dioxide produced:
The balanced chemical equation for the combustion of carbon is:
C + O2 -> CO2
From the equation, we can see that 1 mole of carbon reacts with 1 mole of oxygen to produce 1 mole of carbon dioxide.
Convert the mass of oxygen reacted to moles:
Moles of oxygen reacted = Mass of oxygen reacted / molar mass of oxygen (O2)
Molar mass of oxygen (O2) = 32.00 g/mol
Moles of oxygen reacted = 64.0 g / 32.00 g/mol
Moles of oxygen reacted = 2.0 mol
Since the stoichiometry is 1:1 for carbon and oxygen, the moles of carbon dioxide produced will be the same as the moles of oxygen reacted.
3. Calculate the mass of carbon dioxide produced:
Mass of carbon dioxide produced = Moles of carbon dioxide produced x molar mass of carbon dioxide (CO2)
Molar mass of carbon dioxide (CO2) = 44.01 g/mol (12.01 g/mol for carbon + 2 * 16.00 g/mol for oxygen)
Mass of carbon dioxide produced = 2.0 mol x 44.01 g/mol
Mass of carbon dioxide produced = 88.02 g
Therefore, the mass of carbon dioxide produced is 88.02 grams.
To find the mass of carbon dioxide produced, we need to calculate the amount of oxygen that reacted with the carbon, and then use the stoichiometry of the reaction to determine the amount of carbon dioxide formed.
1. Calculate the amount of oxygen that reacted with carbon:
- The initial amount of oxygen present was 76.8 g.
- The amount of oxygen remaining unreacted is 12.8 g.
- Therefore, the amount of oxygen that reacted is 76.8 g - 12.8 g = 64.0 g.
2. Calculate the amount of carbon dioxide formed:
- The balanced chemical equation for the combustion of carbon is:
C + O2 -> CO2
According to the equation, 1 mole of carbon reacts with 1 mole of oxygen to produce 1 mole of carbon dioxide.
- The molar mass of carbon dioxide (CO2) is approximately 44.01 g/mol.
- To find the amount of carbon dioxide formed, we need to convert the mass of oxygen (64.0 g) to moles.
- The molar mass of oxygen (O2) is approximately 32.00 g/mol.
- Therefore, the number of moles of oxygen reacted is 64.0 g / 32.00 g/mol = 2.00 mol.
- Since the ratio of moles of carbon dioxide to moles of oxygen is 1:2, the amount of carbon dioxide formed is also 2.00 mol.
3. Calculate the mass of carbon dioxide formed:
- Use the molar mass of carbon dioxide (44.01 g/mol) to convert the amount of carbon dioxide from moles to grams.
- The mass of carbon dioxide formed is therefore 2.00 mol × 44.01 g/mol = 88.02 g.
Therefore, the mass of carbon dioxide produced is 88.02 grams.
I will assume you mean 24 grams of carbon burned
C + O2 --> CO2
C is about 12 grams/mol
O2 = 2*16 = 32 grams/mol
CO2 = 12+32 = 44 grams/mol therefore
24/2 = 2 mols carbon
that means 2 mols O2 and 2 mols CO2
2 mols CO2 = 88 grams --- answer
they also gave you redundant information again, check it
76.8-12.8 = 64 grams of O2 they say we used, check that
2 mols O2 = 2*32 = 64 grams, sure enough