Can someone please check this for me?
C4H8+5O2-->3CO2+4H2O+C Butane is a gas and .01 g of it is burned. Is .00218 g of carbon the result?
Thanks
I have a slight difference.
0.01 g x (1 mole C4H8/56.1 g C4H8) x (1 mole C/1 mole C4H8) x (12.01 g C/1 mole C)= 0.00214 g but we're allowed only 1 sig figure anyway which would be 0.002 g C.
Thank you very much!
To determine if 0.00218 g of carbon is the result of burning 0.01 g of butane, we need to calculate the molar masses of the substances involved and use stoichiometry.
Let's start by calculating the molar mass of butane (C4H8) and carbon (C):
Molar mass of butane (C4H8):
C = 4 * atomic mass of carbon
H = 8 * atomic mass of hydrogen
Using the atomic masses from the periodic table:
C = 4 * 12.01 g/mol = 48.04 g/mol
H = 8 * 1.01 g/mol = 8.08 g/mol
Molar mass of butane = 48.04 g/mol + 8.08 g/mol = 56.12 g/mol
Since we have 0.01 g of butane, we can convert this mass to moles:
moles of butane = mass of butane / molar mass of butane
moles of butane = 0.01 g / 56.12 g/mol = 0.000178 mol
According to the balanced chemical equation:
C4H8 + 5O2 → 3CO2 + 4H2O + C
We can see that for every mole of butane burned, 1 mole of carbon is produced. Therefore, the moles of carbon produced will be equal to the moles of butane burned.
moles of carbon produced = moles of butane burned = 0.000178 mol
Now we can calculate the mass of carbon produced:
mass of carbon produced = moles of carbon produced * molar mass of carbon
mass of carbon produced = 0.000178 mol * 12.01 g/mol = 0.00214 g
Based on the calculation, the result of burning 0.01 g of butane should produce approximately 0.00214 g of carbon. Therefore, the value of 0.00218 g of carbon you provided seems to be very close to the expected result.