For the production of ammonia...#N_2(g)+3H_2(g) rightleftharpoons2NH_3(g)#..what is true at equilibrium...?
#"(1) The concentration of ammonia is "2.0*mol*L^-1#
#"(2) The concentration of dinitrogen is constant."#
#"(3) The concentration of ammonia is variable."#
#"(4) The concentration of ammonia cannot be determined."#
Chemical equilibria are a type of kinetic phenomena where the rate of the forward reaction is clearly stated to be equal to the rate of the backward reaction.
By the way, dinitrogen reduction is incredibly hard to accomplish and without it, we wouldn't have nitrogenous fertilizer; this equation represents arguably one of the most significant reactions on the planet.
It's also important to understand this result, by the way. Feel free to voice any questions or objections here, and someone will assist you.
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At equilibrium:
- The rate of the forward reaction equals the rate of the reverse reaction.
- The concentrations of N2, H2, and NH3 remain constant.
- The ratio of [NH3]^2 / ([N2] * [H2]^3) is equal to the equilibrium constant (Kc).
- Changes in pressure, temperature, or concentration may disturb equilibrium, but the system will adjust to re-establish equilibrium.
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At equilibrium:
- The rate of the forward reaction (formation of NH3) is equal to the rate of the reverse reaction (breakdown of NH3).
- The concentrations of N2, H2, and NH3 remain constant over time.
- The equilibrium constant expression for the reaction can be written as [NH3]^2 / ([N2][H2]) = Kc, where Kc is the equilibrium constant.
- Changes in pressure or temperature can shift the position of the equilibrium, but the value of the equilibrium constant remains constant at a given temperature.
- The equilibrium position can favor the formation of ammonia (NH3) or the reactants (N2 and H2) depending on the conditions such as pressure and temperature.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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