For the equilibrium, n2o4(g)< > 2no2(g), the equilibrium constant kp = 0.316. calculate the equilibrium partial pressure of no2 if the equilibrium partial pressure of n2o4(g) is 3.48 atm. 1.05 atm 1.10 atm 3.32 atm 0.301 atm

- Equilibrium partial pressure of is 1.05 atm.

Solution:- The given balanced equation is:

Equilibrium expression for the equation is written as:

(In this expression p stands for partial pressure.)

If we consider the initial partial pressure for the reactant gas as m and the product gas as 0 since initially there is no product. Let's say the change in pressure is n. Then equilibrium partial pressure of reactant gas will be (m-n) and reactant gas equilibrium partial pressure be 2n since it's coefficient is two.

Equilibrium partial pressure of reactant gas is given as 3.48 atm. It means (m-n) = 3.48

Let's plug in the values in the equilibrium expression:

On cross multiply:

Taking square root to both sides:

So, the equilibrium partial pressure of is 1.05 atm.

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.

the correct answer is:

a. formation of precipitation