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

answer; blank (1); /// (2)///(3)///highblank(4)//low;

1. 1 mole of anything contains 6.022x10^23 pieces  

d  

2. a  

3. c, number  

5. 1.24x10^24atoms / 6.022x10^23atoms/mole = 2moles h2 atoms  

6. fe2br3 mass = 2moles x mass fe + 3 moles x mass br  

molar mass = grams / number of moles = g/mole  

to find moles = g / molar mass  

to find mass = g = molar mass / moles