For the reaction 2nobr (g) ↔ 2no (g) + br2 (g), when the concentrations are [nobr] = 0.10 m, [no] = 0.010 m, and [br2] = 0.0050 m, what is the equilibrium constant of this reaction? a. 5.0 × 10–5 m b. 0.000005 m c. 5.0 × 105 m d. 5.0 m e. none of the above

 B. 0.000005

Explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

The given balanced equilibrium reaction is,

At eqm. conc.            0.10 M      0.010 M      0.0050 M

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

Thus the value of the equilibrium constant is 0.000005 M .

the grams   of   barium that   are in   2.3 x 10^23   atoms of barium   is   52.4 g (answer c)

    calculation

mass = moles   of ba   x molar   mass of ba

  molar mass of ba from periodic table=   137.3 g/mol

  use the   avogadro's law   constant   to   calculate the moles of barium

  that   is     1 mole =   6.02   x 10^23 atoms

                    ? moles = 2.3 x 10^23   atoms

by cross   multiplication

=(1 mole   x 2.3x 10^23 atoms)   / 6.02   x10^23 atoms)=   0.382   moles

mass   is therefore = 137.3   g/mol x 0.382 mol = 52.4 ( answer c)

explanation: