For the reaction, C(s)+CO2(g)2CO(g) the partial pressure of CO2 and CO are 2.0 and 4.0 arm respectively then equilibrium Kp for the reaction will be

Question

For the reaction, C(s)+CO2(g)2CO(g) the partial pressure of CO2 and CO are 2.0 and 4.0 arm respectively then equilibrium Kp for the reaction will be (A)  0.5  (B)  8.0  (C)  4.0  (D)  32

Tardigrade Admin · Accepted Answer

For the reaction, C(s)+ CO 2(g) 2 CO (g) Kp=( text partial pressure of gasseous products / text partial pressure of gasseous reactans ) =(PC O2/PC O2)=(4 × 4/2)=8

Q. For the reaction, $C (s) + C O_{2} (g) 2 CO (g)$ the partial pressure of $C O_{2}$ and $CO$ are $2.0$ and $4.0$ arm respectively then equilibrium $K_{p}$ for the reaction will be

$0.5$

$8.0$

$4.0$

$32$

For the reaction, $C (s) + C O_{2} (g) 2 CO (g)$
$K_{p} = \frac{partial pressure of gasseous products}{partial pressure of gasseous reactans}$
$= \frac{P _{CO}^{2}}{P _{C O_{2}}} = \frac{4 \times 4}{2} = 8$

Q. For the reaction, C(s)+CO2​(g)2CO(g) the partial pressure of CO2​ and CO are 2.0 and 4.0 arm respectively then equilibrium Kp​ for the reaction will be

0.5

8.0

4.0

32