What is "if 6.00 g of carbon is burned completely?

When 6.00 grams of carbon is burned completely, it reacts with oxygen in the air to produce carbon dioxide gas (CO2). The balanced equation for this reaction 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. The molar mass of carbon is approximately 12.01 g/mol.

To calculate the amount of carbon dioxide produced from the combustion of 6.00 grams of carbon, we can use the following steps:

1. Calculate the number of moles of carbon in 6.00 grams using the formula: moles = mass / molar mass moles = 6.00 g / 12.01 g/mol ≈ 0.5 moles

2. Since 1 mole of carbon produces 1 mole of carbon dioxide, the number of moles of carbon dioxide produced will be equal to the number of moles of carbon. moles of CO2 = 0.5 moles

3. Calculate the mass of carbon dioxide produced using the formula: mass = moles x molar mass of CO2 mass = 0.5 moles x 44.01 g/mol ≈ 22.01 grams

Therefore, when 6.00 grams of carbon is burned completely, it produces approximately 22.01 grams of carbon dioxide gas.