Problem: Which factors will affect both the position of equilibrium and the value of the equilibrium constantfor this reaction?           N2(g) + 3H2(g) 2NH3(g)                                                                 ∆H = –92kJ A. Increasing the volume of the containerB. Adding more nitrogen gasC. Removing ammonia gasD. Lowering the temperature

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Which factors will affect both the position of equilibrium and the value of the equilibrium constant

for this reaction?

          N2(g) + 3H2(g) 2NH3(g)                                                                 ∆H = –92kJ

A. Increasing the volume of the container

B. Adding more nitrogen gas

C. Removing ammonia gas

D. Lowering the temperature

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