The volume of CO2 produced by the combustion of 20g of graphite containing 10% impurity will be?

To find the volume of CO2 produced by the combustion of graphite, we can follow these steps:

Step 1: Calculate the moles of graphite.
To do this, we need to determine the molar mass of pure carbon (graphite), which is 12.01 g/mol. We can use the following formula:

Moles of Graphite = Mass of Graphite / Molar Mass of Graphite

Given that the mass of graphite is 20g, we can calculate the moles of graphite as follows:

Moles of Graphite = 20g / 12.01 g/mol

Step 2: Calculate the moles of pure carbon.
Since the graphite contains 10% impurities, only 90% of the 20g is actual carbon. We can calculate the mass of carbon as follows:

Mass of Carbon = 20g * 0.90

Next, we can calculate the moles of pure carbon using the molar mass of carbon (12.01 g/mol):

Moles of Pure Carbon = Mass of Carbon / Molar Mass of Carbon

Step 3: Calculate the volume of CO2 produced.
During combustion, 1 mole of carbon produces 1 mole of CO2. Therefore, the moles of CO2 produced will be the same as the moles of pure carbon.

Finally, we can calculate the volume of CO2 using the ideal gas law, assuming standard temperature and pressure (STP), where 1 mole of gas occupies 22.4 liters:

Volume of CO2 = Moles of Pure Carbon * 22.4 liters/mol

By following these steps, we can find the volume of CO2 produced.

To calculate the volume of CO2 produced by the combustion of graphite, you need to know the molecular weight of CO2, the mole ratio between graphite and CO2, and the density of CO2 at the given conditions.

Here's the step-by-step approach to finding the answer:

1. Calculate the number of moles of pure graphite:
- Determine the molecular weight of pure graphite (C), which is 12 g/mol.
- Divide the mass of pure graphite (20g) by its molecular weight to find the number of moles. In this case, 20g/12 g/mol = 1.67 mol.

2. Calculate the number of moles of impurities:
- Assuming the impurities are not combusted and do not contribute to the formation of CO2, they can be excluded from the calculations.

3. Calculate the number of moles of CO2 produced:
- The balanced chemical equation for the combustion of graphite is: C + O2 -> CO2.
- From the equation, you can see that 1 mole of graphite reacts to form 1 mole of CO2.
- Therefore, the number of moles of CO2 produced is also 1.67 mol.

4. Calculate the volume of CO2 produced:
- The density of CO2 varies with temperature and pressure. At standard temperature and pressure (STP), the density of CO2 is approximately 1.98 g/L.
- Convert the number of moles of CO2 to grams by multiplying it by the molecular weight of CO2. The molecular weight of CO2 is 44 g/mol.
- Multiply the resulting weight of CO2 with its density to find the volume. In this case, (1.67 mol * 44 g/mol) * (1 L/1.98 g) ≈ 37.9 L.

So, the volume of CO2 produced by the combustion of 20g of graphite containing 10% impurity would be approximately 37.9 liters at standard temperature and pressure (STP).

C + O2 --> CO2

20g at 90% purity = 18 g pure C.
Can you take it from there?