what is Keq for the reaction N2+3H2 = 2NH3 if the equilibrium concentrations are NH3 = 2 M, and H2 = 1 M

0.5

Explanation:

What is Keq for the reaction N2 + 3H2  = 2NH3 if the equilibrium concentrations are [NH3] = 2 M, [N2] = 1 M, and [H2] = 2 M?

Step 1: Given data

Equilibrium concentrations:

[N₂] = 1 M

[H₂] = 2 M

[NH₃] = 2 M

Step 2: Write the balanced equation

N₂(g) + 3 H₂(g)  ⇄ 2 NH₃(g)

Step 3: Calculate the concentration equilibrium constant (Keq)

The concentration equilibrium constant is equal to the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients.

Keq = [NH₃]² / [N₂] × [H₂]³

Keq = 2² / 1 × 2³ = 0.5

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.