15. Consider the following reaction. N2 (g) + 3 H2 (g) 2 NH3 (g) 1.0 atm of N2 a

Question

15. Consider the following reaction. N2 (g) + 3 H2 (g) 2 NH3 (g) 1.0 atm of N2 and 1.0 atm of H2, are mixed in a container at 1000 K. At this temperature, Kp = 2 x 10-3 The equilibrium expression was used to determine the equilibrium partial pressures of each species. Letting x=amt of N2 reacted gives the following four values for x. (2 x)2 Ie-Solve Oues_ {(x-7.58436}, {x-... 0 . 02 52 6 3 6), {x 0.0201571), (x 9.58947)) Choose the appropriate value of a and determine the equilibrium pressure for each 0.002,x -x (1-3x)02 species in the reaction? (a) (b) (c) (d) x=-7.58 x =-0.0253 x = 0.0212 x=9.59

Explanation / Answer

N2 + 3H2 <-----> 2NH3

1       1                  0       initial

1-x     1-3x             2x      equilibrium

Kp = (NH3)^2/(N2)(H2)^3

2*10^-3= (2x)^2/((1-x)(1-3x)^3)

x= 0.02

As the initial pressure is 1 atm then we have to choose 0.02 atm is the right option.

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