What is the value of K for the reaction of molecular oxygen to ozone if the equi

Question

What is the value of K for the reaction of molecular oxygen to ozone if the equilibrium concentration of axygen is the equlbrun oncertraton of angenis09902 Mandofoore is 03201 M arks: 1 Answer 1045 What is the value of Ke for the reaction of nitrogen and oxygen to make dinitrogen 1.0958 atm and the partial pressure of dinitrogen monoxide is 0.0346 atm? monoxide he equibrium partial pressures of nitrogen is 1.3347 atm, the partial pressure of axygen Marks: 1 Answer 00061 ofhydomi. 00290 Mandofamn.1140M7 what is the value of a te reaction of nivogen ard hydrogen to make "montte onontabn ofnbogen-00284 Marks: 1 Answer What is the value of Q for the reaction of nitrogen and oxygen to make dintrogen telroxide if the partial pressures of ntrogen is 1.3166 atm the partial pressure of oxygen i t .0eso Marks 1 Answer O a st to the right by increasing the concentaon of the prosdacs O b shit to the right by increasig the concenration of the reactans Marks 1

Explanation / Answer

First, let us define the equilibrium constant for any species:

The equilibrium constant will relate product and reactants distribution. It is similar to a ratio

The equilibrium is given by

rReactants -> pProducts

Keq = [products]^p / [reactants]^r

For a specific case:

aA + bB = cC + dD

Keq = [C]^c * [D]^d / ([A]^a * [B]^b)

Note that the concentrations MUST be in equilibrium. If these are not in equilibrium, then the reaction will take place until there is equilibrium achieved.

For this, we use Q, the reaction quotient of products/reactants, it allows us to understand the ratio distribution and the direction/shit of equilibrium

Q is defined as:

Q = [C]^c * [D]^d / ([A]^a * [B]^b)

In this Case, the concentrations are NOT in equilibrium

then

Q = [NH3]^2 /[N2][H2]^3)

Q = (1.14^2) /((0.0264)(0.0266^3))

Q = 2615536.9 = 2.6*10^6

Q8

N2 + 2O2 = N2O4

Qp= P-N2O4 / ((P-N2)(P-O2)^2)

Qp = ( 0.030706)) /((1.3166)(1.085^2))

Qp = 0.01981116

Q9

If Q > Keq; this has much more products than reactants, therefore expect products to form more reactants in order to achieve equilibrium

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.