At 450 degrees celcius, 3.60 mol of ammonia is placed in
a2.00-l vessel and allowed to decompose to the elements.

if the experimental value of k is 6.3 for
thisreaction at this temperature, calculate the
equilibriumconcentration of each reagent. what is the total
pressure in theflask?

x = 12.4 atm

Explanation:

step1: To calculate the pressure of NH3 in theflask using ideal gas equation            

             PV = nRT

Hence, we have

              P = 3.60 mol * 0.0821L.atm / mol.K * (450 +273)K /2.00L

                  = 106.84 atm

step2: To calculate the equilibrium concentration of each component

                2NH3 ↔        N2    +        3H2

  initial(p)   106.84atm       0                    0

change       -2x                  +x                +3x

equilibrium (106.84-2x )      x                   3x

   k = PN2 PH23 /PNH32

6.3 = x * (3x)3 / (106.84-2x ) 2

since k is small , we ignore 2x compared to 106.84

otherwise to get the exact value of x u have to solve the equation above

   taking approx x = 12.4atm

then substitute the value of x in the respective equilibrium values

then find PT = PN2+ PH2+PNH3

the answer is c i took the test