When 0.100 mol of carbon is burned in a close vessel with 8.00g of oxygen, how many grams of carbon dioxide can form?

To find the number of grams of carbon dioxide that can form when 0.100 mol of carbon reacts with 8.00g of oxygen, we need to determine the balanced chemical equation for the reaction between carbon and oxygen, and then use stoichiometry to convert between moles of carbon dioxide and grams of carbon dioxide.

The balanced chemical equation for the combustion of carbon can be written as:

C + O2 -> CO2

According to the equation, one mole of carbon reacts with one mole of oxygen to produce one mole of carbon dioxide.

First, we convert the mass of oxygen into moles using its molar mass. The molar mass of oxygen (O2) is approximately 32.00 g/mol since oxygen has an atomic mass of 16.00 g/mol.

moles of oxygen = mass of oxygen / molar mass of oxygen
moles of oxygen = 8.00 g / 32.00 g/mol
moles of oxygen = 0.25 mol

From the balanced chemical equation, we know that the mole ratio between carbon and oxygen is 1:1. Therefore, the number of moles of carbon is also 0.100 mol.

Now, we can determine the number of moles of carbon dioxide formed using the mole ratio of carbon dioxide to carbon.

moles of carbon dioxide = moles of carbon

Since carbon dioxide has a molar mass of approximately 44.01 g/mol (12.01 g/mol for carbon and 32.00 g/mol for oxygen), we can convert the moles of carbon dioxide to grams.

grams of carbon dioxide = moles of carbon dioxide x molar mass of carbon dioxide
grams of carbon dioxide = moles of carbon x molar mass of carbon dioxide
grams of carbon dioxide = 0.100 mol x 44.01 g/mol
grams of carbon dioxide = 4.401 g

Therefore, when 0.100 mol of carbon reacts with 8.00g of oxygen, approximately 4.401 grams of carbon dioxide can form.