When a 8.45-mg sample of a compound containing carbon is burned completely, 18.1 mg of carbon dioxide is produced. What is the mass percentage of carbon in the compound?

Assuming all of the carbon from compound is converted to carbon dioxide the mass amount of carbon => (12/44)100% = 27.27% of CO2 produced. From this, the mass of carbon in the 18.1mg of CO2 => 18.1(.2727)mg = 4.94mg carbon. Therefore, the %C in sample = (4.94/8.45)100% = 58.41% by wt.

mass C = 18.1 mg CO2 x (atomic mass C/molar mass CO2) = ?

%C = (Mass C/mass sample)*100 = ?

To find the mass percentage of carbon in the compound, you'll need to calculate the mass of carbon in the compound and then divide it by the total mass of the compound.

1. Calculate the mass of carbon:
Given that 18.1 mg of carbon dioxide is produced from 8.45 mg of the compound.
We know that the carbon dioxide contains one atom of carbon (C) per molecule, so the mass of carbon in the compound is the same as the mass of carbon dioxide produced.
Therefore, the mass of carbon is 18.1 mg.

2. Calculate the mass percentage of carbon:
The total mass of the compound is 8.45 mg.
To find the mass percentage of carbon, divide the mass of carbon by the total mass of the compound and then multiply by 100.
Mass percentage of carbon = (mass of carbon / total mass of compound) * 100
Mass percentage of carbon = (18.1 mg / 8.45 mg) * 100

Using a calculator, the mass percentage of carbon in the compound is approximately 214.79%.

To find the mass percentage of carbon in the compound, we first need to determine the amount of carbon in the 8.45 mg sample.

Given that 18.1 mg of carbon dioxide (CO2) is produced when the sample is burned completely, we can conclude that the amount of carbon (C) in the compound is equal to the amount of carbon dioxide produced.

The molar mass of carbon dioxide is 44.01 g/mol, and its chemical formula shows that it contains one carbon atom. Therefore, the mass of carbon in the compound is 18.1 mg.

The mass percentage of carbon is calculated by dividing the mass of carbon in the compound by the total mass of the compound (8.45 mg) and multiplying by 100:

Mass percentage of carbon = (mass of carbon / mass of compound) x 100

Mass percentage of carbon = (18.1 mg / 8.45 mg) x 100 ≈ 214.20%

Therefore, the mass percentage of carbon in the compound is approximately 214.20%.