8 of 9 Constants | Periodic Table The reaction CO2( g )+C( s )2CO( g ) has K = 4
ID: 580025 • Letter: 8
Question
8 of 9
Constants | Periodic Table
The reaction CO2(g)+C(s)2CO(g) has K = 48.3 at 1200 K.
Part A
Part complete
Calculate the total pressure at equilibrium when 4.81 g of CO2 is introduced into a 10.0-L container and heated to 1200 K in the presence of 2.90 g of graphite.
Express your answer to two significant figures and include the appropriate units.
2.1 atm
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Correct
Part B
Repeat the calculation of part A in the presence of 0.31 g of graphite.
Express your answer to two significant figures and include the appropriate units.
I have a just need help solving b! It's due really soon haha
Ptotal =2.1 atm
Explanation / Answer
CO2(g) + C(s) <===> 2CO(g) has K = 48.3 at 1200 K.
initial pressure of CO2 = nRT/V
= (w/M)RT/V
= ((4.81/44)*0.0821*1200)/10
= 1.07 atm
at equilibrium
pressure of CO2 = 1.07-x atm
pressure of CO = 2x
Kp = pCO^2/pCO2
48.3 = (2X)^2/(1.07-X)
x = 0.99 atm
Total pressure = 1.07-x + 2x
= 1.07-0.99+2*0.99
= 2.06 atm
answer: 2.1 atm
part B,
no of mol of CO2 = W/M
= 4.81/44
= 0.109 mol
no of mol of C = 0.31/12 = 0.026 mol
to reach equilibrium ,
No of mol of C required = n = 0.99*10/0.0821*1200 = 0.1 mol
but available is only 0.026 mol.
so that,
No of mol of CO produced = 0.026*2 = 0.052 mol
No of mol of CO2 left = 0.109-0.026 = 0.083 mol
total mol of gas = 0.083+0.052 = 0.135 mol
total pressure(P) = nRT/V
= 0.135*0.0821*1200/10
= 1.3 atm
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