The equilibrium constant (K) of the reaction below is K = 2.5 x 10-3, with initialconcentrations as follows: [H₂] = 1.0 x 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 104 M.N2(g) + 3 H₂(g) 2 NH3(g)If the concentration of the product NH3 was increased from 1.0 x 10-4 M to 5.6 x10-3 M, then the reaction quotient (Q) is1.60x10^-7towards theforwardA The equilibrium position will shift[left/right/or remain unchanged] The equilibrium constant (K) of the reaction below is K = 2.5 x 10-3, with initialconcentrations as follows: [H₂] = 1.0 x 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 104 M.N₂(g) + 3 H₂(g) 2 NH3(g)If the concentration of the reactant H₂ was decreased from 1.0 x 10-2 M to 2.7 x 10-4 M, then the reaction quotient (Q) is [Report answer in scientific notation]towards theThe equilibrium position would shift[left/right/or remain unchanged]

Answered: Image /qna-images/answer/39086409-d220-4690-b361-178f75965108.jpg

The equilibrium constant (K) of the reaction below is K = 2.5 x 10-3, with initial concentrations as follows: [H₂] = 1.0 x 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 10 4 M. N2(g)+ 3 H₂(8) 2 NH3(g) If the concentration of the product NH3 was increased from 1.0 x 10-4 M to 5.6 x 10-3 M, then the reaction quotient (Q) is 1.60x10^-7 towards the forward A/ [left/right/or remain unchanged] The equilibrium position will shift A/

The equilibrium constant (K) of the reaction below is K = 2.5 x 10-3, with initial concentrations as follows: [H₂] = 1.0 x 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 10 4 M. N2(g)+ 3 H₂(8) 2 NH3(g) If the concentration of the product NH3 was increased from 1.0 x 10-4 M to 5.6 x 10-3 M, then the reaction quotient (Q) is 1.60x10^-7 towards the forward A/ [left/right/or remain unchanged] The equilibrium position will shift A/

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 60QRT

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