How much carbon can be obtained from 65.3 g of #Ca(C_2H_3O_2)_2#?

Answer 1

Owen Ambrose

Approximately #19.8# grams

Approximate the molar mass of the constituent elements as follows:

#Ca: 40# g/mol

#C: 12# g/mol

#H: 1# g/mol

#O: 16# g/mol

Then the mass of #Ca(C_2H_3O_2)_2# is:

#40+2((2*12)+(3*1)+2*(16))#

#=40+2(24+3+32)#

#=40+2*59#

#=158# g/mol

of which #4*12 = 48# g/mol is carbon.

So in #65.3"g"# of #Ca(C_2H_3O_2)_2#, the mass of carbon is:

#65.3*48/158 ~~ 19.8"g"#

By signing up, you agree to our Terms of Service and Privacy Policy

Answer 2

Henry Antrim

The mass of carbon obtained is approximately 4.95 g. The molar mass of Ca(C₂H₼O₂)₂ is approximately 158.17 g/mol. This means that 65.3 g of Ca(C₂H₃O₂)₂ contains about 0.413 moles of the compound. Since each mole contains one mole of carbon, the amount of carbon is also 0.413 moles.

By signing up, you agree to our Terms of Service and Privacy Policy

Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.