Question

gen chem 1: A sample of PbCO3 , XPb(OH)2 was heated with excess sulfuric acid, yielding PbSO4, H2O, and CO2. If 2.280g of PbSO4 and 0.1104g of CO2 were obtained, what is the value of X?

Answer 1

So, PbCO3 XPb(OH)2 + H2SO4 ---> PbSO4 + H2O unbalanced

Answer 2

oops i meant PbCO3 XPb(OH)2 + H2SO4 ---> PbSO4 + H2O + CO2 unbalanced

Answer 3

I traced CO2 to PbCO3, one mole of PbCO3 = one mole of CO2.

Answer 4

I saw a yahoo answer that said the next solution is to trace PbSO4 to XPb(OH)2, I wonder how that's possible since there are two sources of Pb

Answer 5

did u get the answer?

Answer 6

no =/

Answer 7

so you find the moles of PbSO4 and CO2, their ratio is 3:1

use the equation:

PbCO3 XPb(OH)2 + H2SO4 ---> PbSO4 + H2O + CO2
3 1

notice that the only source of SO4 is H2SO4, so:

PbCO3 XPb(OH)2 + H2SO4 ---> PbSO4 + H2O + CO2
3 3 1
only source of C from CO3 is C from CO2,

PbCO3 XPb(OH)2 + H2SO4 ---> PbSO4 + H2O + CO2
1 3 3 1

the result from 3 moles of Pb produced, 3:

so , PbCO3 XPb(OH)2 + H2SO4 ---> PbSO4 + H2O + CO2
1 2 3 3 1

now just add up the oxygens

Answer 8

thanks

Answer 9

no prob