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11 Nov 2019
15 Question (1 point) The value of the equilibrium constant K, for the formation of ammonia, N2(g) +3H2(g)-2NH3(g) is 4.50 x 10-5 at 450°C. 1st attempt What is the value of Kp for the following reaction? : 2NH3(g)-3H2 (g)-N2(g)
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Jarrod Robel
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12 Jun 2019
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Related questions
08 Question (1 point) a See page 704 An important industrial process for synthesizing the ammonia used in agricultural fertilizers involves the combination of N2 and H2: N2(g) + 3H2(g)-2NH3(g) K-3.552x 108 at 63.86â 1st attempt See Periodic Table See Hint What is the value of Kp of this reaction at 63.86°C?
08 Question (1 point) a See page 704 An important industrial process for synthesizing the ammonia used in agricultural fertilizers involves the combination of N2 and N2(g) +3H2(g)-2NH3(g) KC-3.552 x 108 at 63.86â 1st attempt See Periodic Table See Hint hat is the value of Kp of this reaction at 63.86"C?
R= 0.08206 L.atm/mol.K
R = 8.314 J/mol.K
Kp = Kc (RT)?n
1. For the reaction N2 (g) + 3H2 (g) ?? 2NH3 (g) write:
a) An expression for the equilibrium constant (Kc ) of the forwardreaction:
b) An expression for the equilibrium constant (Kc )of the reverse(backward) reaction:
c) An expression for the Kp of the gases of the forwardreaction:
d) The equilibrium constant for N2 (g) + 3H2 (g) ?? 2NH3 (g) is Kc= 655 @ 250 C.
Calculate Kc for the followings:
2NH3 ?? N2 (g) + 3H2 (g) Kc ?
NH3 ?? 1/2N2 + 3/2H2 Kc ?
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