8 of 9 Constants | Periodic Table The reaction CO2( g )+C( s )2CO( g ) has K = 4

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

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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