At 700.°C, the total pressure of the system is found to be 3.01 atm. If the equilibrium constant KP is 1.52, calculate the equilibrium partial pressures of CO2 and CO.

Pco = 1.51 atm

Pco = 1.5 atm

Explanation:

C (s) + CO2 (g) ⇔ 2 CO (g)

T = 700°C, P (total) = 3.01 atm, KP = 1.52

Mathematically,

KP =

According to Dalton' Law which states that at equilibrium, the sum of the partial pressures of each component is equal to the total pressure

Mathematically,

P (total) = Pco + Pco = 3.01 atm

Pco = P (total) - Pco

Pco = 3.01 - Pco

Substitute Pco into the KP equation, we have

KP = ⇒ 1.52 =

Let y = Pco

1.52 = = = 1.52 (3.01 - y)

= 4.5752 - 1.52y ⇒   + 1.52y - 4.5752 = 0

Using the quadratic formula y = and y =

y = 1.51 or −3.03

We choose the positive root because Pco cannot be negative (Remember Pco = y)

Hence, Pco = 1.51 atm

Pco = 3.01 - Pco = 3.01 - 1.51

Pco = 1.5 atm

43.452

step-by-step explanation:

284 times .153 = 43.452

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2