CaCO
3(s)
CaO(s) + CO
2(g)
Kp for this reation is 1.16 at 800°C. A 5.00 L vessel containing 10.0g of CaCO
3 was evacuated to remove the air, sealed, and then heated to 800C. Ignoring the volume occupied by the solid, what will be the overall mass percent of carbon in the solid once equilibrium is reached?
Attempt
Kp= 1.16
P =1.16 atm ; PV=nRT
n= 0.0659 mol CO
2 which is equal to 2.90 CO
210.0- 2.90
remaining solid weight : 7.1 g
Stoich
2.90 g * 1mol CO2/ 44g CO2 * 1 mol CaCO3 /1mol CO2 * 100.09 g CaCO
3/1 mol CaCO3
6.60g of CaCO
3 will be consumed.
7.1-6.60 = 0.5 g of CaO-- Is this logical right so far XD
6.60 g 1mol CaCO
3 / 100.09g * 1 mol C/1mol CaCO
3 * 12.01g/1mol C
=0.79 g of C
Percent : 0.79/ 6.60 x 100 = 12.0%
Some source says it was 5% only pls help