The Kc for the following reaction at 100 °C is 2.0. If the equilibrium mixture contains 2.0 M NO and 1.0 M Br2, what is the molar concentration of NOBr?

2NOBr (g) ⇌ 2NO(g) + Br2 (g)

The answer to your question is [NObr] = 1.41

Explanation:

Data

Kc = 2

[NO] = 2 M

Br₂ = 1.0 M

NOBr = ?

Process

1.- Write the Equation of the Kc

                    Kc =

2.- Solve for [NOBr]

                   [NOBr]² =

3.- Substitution

                   [NOBr]² =

4.- Simplification

                    [¨NOBr]² =

                    [NOBr]² = 2

5.- Result

                    [NOBr] =

                    [NOBr] = 1.41

The molar concentration of NOBr is 1.414 M

Explanation:

Step 1: Data given

Kc = 2.0

The equilibrium mixture contains:

2.0 M NO

1.0 M Br2

Step 2: The balanced equation

2NOBr (g) ⇌ 2NO(g) + Br2 (g)    Kc = 2.0

Step 3: Define Kc

Kc = [Br2]*[NO]²/[NOBr]²

⇒ with Kc = 2.0

⇒with [Br2] = 1.0M

⇒with [NO] = 2.0 M

⇒with [NOBr] = TO BE DETERMINED

Step 4: Calculate the molar concentration of NOBr

Kc = [Br2]*[NO]²/[NOBr]²

2.0 = (1.0*2.0²) / NOBr²

NOBr² = 4.0 / 2.0 = 2.0

NOBr = √2.0 = 1.414 M

The molar concentration of NOBr is 1.414 M

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.