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12 Dec 2019

The equilibrium constant for the chemical equation N2 (g)+3H2 (g) yields 2NH3 (g) is Kp = 103 at 181 °C. Calculate the value of the Kc for the reaction at 181 °C.

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Deanna Hettinger
Deanna HettingerLv2
13 Dec 2019

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Related questions

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 ?
1) The equilibrium constant for the chemical equation?
N2(g) + 3H2(g)<---->2NH3(g)
is Kp = 0.273 at 219

Part A

For the reaction

2CH4(g)?C2H2(g)+3H2(g)

Kc=0.150 mol2 L?2 at 1785?C . What is Kp for the reaction at this temperature?

Part B

What is the unitless thermodynamic equilibrium constant K for the reaction in part A?

Part C

For the reaction

N2(g)+3H2(g)?2NH3(g)

Kp=3.75

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