Question

3. Consider the ammonia production reaction, N2(g)+3H2(g) + 2NH3 (g). The equi- librium constant for this reaction at 298K is 6.10 x 105. When the system starts with 2 mol of NH3 (no H, or N2), it reaches the equilibrium at the total pressure of 2.0 bar. (a) What is the mole fraction of each species at equilibrium? (b) If we increase the total pressure to 3.0 bar, will it be stimulating the decompo- sition of ammonia? Explain.

Answer 1

Noz (g) + 3H2(g) = 2NH3(g) K= 640x18 op 2 NH3(g) = N2(7) + 3H2(g), Kp = GOXO) Initiallmol.) 2 0 0 Change (mot.) -23 + 2 = + 3% = 4.639410 Equilibrium (mol) (2-27) * 3X... At equilibrium, total no. of males of gases - 2-2x+x+3x 2(1+x) *NH3 = 2(1-23 15 = 12 h and Polits = (1 - 2/2) x2 alin C and Pri2 = 2 2 2 * 2 = ( 2 ) "H2 = 30 and PH2 = 3 x x = (3x) ko Pria* PH2 = 1 + 2 (3) 3 Pritis 321-3322 IN2 = 2 (142) , X2 1X 21+20 Y+ 2(1+70) 1+ 1 - = 1.639x10 (2(1-x22 6 + x.x27x x3 = 1.6397105 1+x)2 x 4 (1-3)2 23 1-22 4*1.639x10 27 ojo ga = 4,93 8104 op (-32)4.93*104122 or 5.93 x 104 4² - 4.93x104 or 3?- (4193) or x = 11493 = 0.912 (5.93) 0.046 Ito:912) 340.912 and X42= 10.00 -0.715 0,912 = 0.238 261401912) 5.93) PIHAH Niz ING

N2(g) + 3H₂(g). 2NH3(g) on = 2- (1+3) = -2 If we increase total pressure, the rate of forward reaction will increase in order to maitain the equilibrium, As a result the . the formation of NH3 will increase. So, if we increase the total pressure, it will not stimulating the decomposition of NHz.