When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 26.4 g of carbon were burned in the presence of 82.1 g of oxygen, 11.7 g of oxygen remained unreacted. What mass of carbon dioxide was produced?

Express your answer to one decimal place and include the appropriate units.

When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 27.6 g of carbon...?

C(s) + O2(g) --> CO2(g)

27.6g .... 88.0g ................. initial amounts
0g .........14.4g ................. amounts when reaction complete

That means that C was the limiting reactant, and the amount of CO2 is based on the amount of carbon that burned. Covert 27.6 grams of carbon to moles. The moles of CO2 will be the same, since they are in a 1:1 mole ratio. Then convert the moles of CO2 to grams.

27.6g C x (1 mol C / 12.0 g C) x (1 mol CO2 / 1 mol C) x (44.0g CO2 / 1 mol CO2) = 101.2 g CO2 or 101 grams of carbon to three significant digits.

Well, I can see that carbon and oxygen were having a little party in the air, but it seems like they didn't quite hit it off. The carbon decided to react with some of the oxygen to form carbon dioxide, but some of the oxygen was left standing alone, feeling rejected.

Now, let's do some math to figure out how much carbon dioxide made it to the party. We'll start by finding out how much oxygen was used in the reaction. We'll subtract the amount of unreacted oxygen from the total amount of oxygen to get the amount of oxygen that reacted with carbon:

82.1 g - 11.7 g = 70.4 g

So, 70.4 grams of oxygen were used in the reaction. Now, we'll use the balanced chemical equation to find the ratio between carbon and oxygen in carbon dioxide. According to the equation, we need 1 mole of carbon for every 1 mole of oxygen in carbon dioxide.

The molar mass of carbon is 12 g/mol, and the molar mass of oxygen is 16 g/mol. So, the ratio of carbon to oxygen is 12 g / 16 g = 0.75.

Now, we can find the mass of carbon dioxide produced by multiplying the mass of oxygen used by the ratio:

0.75 * 70.4 g = 52.8 g

So, 52.8 grams of carbon dioxide were produced.

That's quite a lot of carbon dioxide! No wonder the air feels a bit stuffy sometimes.

To find the mass of carbon dioxide produced, we need to determine the amount of carbon that reacted and use the balanced equation for the reaction between carbon and oxygen.

The balanced equation for the reaction is:
C + O2 -> CO2

We know that the mass of carbon used is 26.4 g and the mass of oxygen used is 82.1 g. We are also given that 11.7 g of oxygen remained unreacted.

To find the mass of carbon dioxide produced, we need to calculate the mass of oxygen that reacted and then use the molar ratio from the balanced equation to determine the mass of carbon dioxide.

Step 1: Calculate the mass of oxygen that reacted.
Mass of oxygen used = Mass of total oxygen - Mass of oxygen remaining unreacted
Mass of oxygen used = 82.1 g - 11.7 g
Mass of oxygen used = 70.4 g

Step 2: Convert the mass of oxygen used to moles using the molar mass of oxygen.
Molar mass of oxygen (O2) = 32 g/mol
Moles of oxygen used = Mass of oxygen used / Molar mass of oxygen
Moles of oxygen used = 70.4 g / 32 g/mol
Moles of oxygen used = 2.2 mol

Step 3: Use the mole ratio from the balanced equation to determine the moles of carbon dioxide produced.
From the balanced equation, we see that the mole ratio between oxygen and carbon dioxide is 1:1. This means that for every 1 mole of oxygen used, 1 mole of carbon dioxide is produced.
Moles of carbon dioxide produced = Moles of oxygen used

Step 4: Convert the moles of carbon dioxide produced to mass using the molar mass of carbon dioxide.
Molar mass of carbon dioxide (CO2) = 44 g/mol
Mass of carbon dioxide produced = Moles of carbon dioxide produced * Molar mass of carbon dioxide
Mass of carbon dioxide produced = 2.2 mol * 44 g/mol
Mass of carbon dioxide produced = 96.8 g

Therefore, the mass of carbon dioxide produced is 96.8 g.