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

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

c (diamond),

sio2 (quartz)