Suppose a 250.0 mL flask is filled with 1.3 mol of I2 and 1.0 mol of HI. The following reaction becomes possible:
H2 (g) +I2 (g) ⇆ 2HI (g)
The equilibrium constant for this reaction is 0.983 at the temperature of the flask.
Calculate the equilibrium molarity of HI. Round your answer to two decimal places.

2.27 M

Explanation:

Given that :

volume = 250.0 mL = 0.250 L

Number of moles of = 1.3 mol

Number of moles of = 1.0 mole

Initial concentration of   =

=

= 5.20 M

Initial concentration of   =

=

= 4.0 M

Equation of the reaction is represented as:

The I.C.E Table is as follows:

                               +             ----->      

Initial(M)                  0.0              5.20                   4.0  

Change                    +x               +x                       - 2x

Equilibrium(M)           x             5.20+x                 4 - 2x

             where K = 0.983

multiplying through by (-) and rearranging in the order of quadratic equation; we have:

using the quadratic formula:

=

=

=     OR  

= 6.133      OR      0.864

since 6.133 is greater than K value then it is void, so we go by the lesser value which is 0.864

so x = 0.864 M

The equilibrium molarity of HI = (4.0- 2x)

= 4.0 - 2(0.864)

= 4.0 - 1.728

= 2.272 M

= 2.27 M to two decimal places

the answer is the first option

explanation:

just googled it m8. not that hard

lol

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.