Question

A sample of pure no2 gas heated to 1000k decomposes: 2no2(g) gives 2no +o2.the equlibrium constant kp is 100 atm.analysis shows that the partial pressure of o2 is 0.25atm. at equilibrium. the partial pressure of no2 at equilibrium is

Answer 1

Answer:- 0.025 atm

Solution:- The given balanced equilibrium equation is:

$2NO_2(g)\leftrightarrow 2NO(g)+O_2(g)$

From the equation, there is 2:1 mole ratio between NO and $O_2$ .

Their equilibrium partial pressure would be in the ratio. Equilibrium partial pressure of oxygen is given as 0.25 atm. So, the equilibrium partial pressure of NO = 2(0.25 atm) = 0.50 atm

Equilibrium expression for the given equation is written as:

$Kp=\frac{(P_N_O)^2(P_O_2)}{(P_N_O_2)^2}$

Let's plug in the values in it and solve it for equilibrium partial pressure of $NO_2$ . Let's say the equilibrium partial pressure of nitrogen dioxide is p.

$100=\frac{(0.50)^2(0.25))}{p^2}$

$100=\frac{0.0625}{p^2}$

On rearranging the above equation:

$p^2=\frac{0.0625}{100}$

On taking square root to both sides:

$p=\frac{0.25}{10}$

p = 0.025 atm

So, the equilibrium partial pressure of $NO_2$ is 0.025 atm.

Answer 2

Answer:

0.025 atm

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