I did the work, but I need help checking it...
A compound contains 83.24% by mass carbon. Calculate the molar mass of the compound if it contains 5 moles of carbon per mole of compound.
This was my process:
I took 100g of compound and found that there are 83.24 g C in that much compound.
Then:
(83.24 g C) * (1 mol C / 12.011 g C) * (1 mol compound / 5 mol C) * (X g compound / 1 mol compound)
= 1.386 g compound
Is this correct..?
To check if your calculation is correct, we can use the given information and the molar mass of carbon to calculate the molar mass of the compound.
First, let's calculate the mass of carbon in 1 mole of the compound. Since it contains 5 moles of carbon per mole of the compound, the mass of carbon in 1 mole of the compound can be found by multiplying the molar mass of carbon (12.011 g/mol) by 5:
Mass of carbon in 1 mole of compound = 12.011 g/mol × 5 mol = 60.055 g/mol
Now, we can calculate the molar mass of the compound using the mass-percent composition of carbon. We know that the compound contains 83.24% carbon by mass. This means that in 100 g of the compound, there are 83.24 g of carbon.
Molar mass of compound = 100 g of compound / (83.24 g of carbon/60.055 g/mol)
Molar mass of compound ≈ 1.201 g/mol
Based on your calculation, you obtained a molar mass of 1.386 g/mol. This value seems incorrect as the molar mass of the compound should be higher since it contains more than just carbon.
Therefore, there seems to be a mistake in your calculation. I would recommend double-checking your calculations to find the error.