Starting with 0.500 M N, and 0.800 M H;, the reaction is allowed to proceed until it reaches equilibrium. The [NHl = 0.150 M at 250°C. Determine K for this reaction at this temperature. Start by filling in the ICE table with the Initlal concentrations. Reaction (N] (M) (H] (M) (NH.] (M) Initial Change Equilibrium b) Next, fill in the Changes in the system, in terms of x, which will deteied by the stolchlometry. Reactants are used up (-) and products are formed (*). c) Next, write equlbrlum expressions, in terms of initial concentrations and the changes that ocur (x). d) Solve for x from the information you have. Detemine the equilibrium concentrations of N, and H. INku". [Hk. Write the equation for K, the equilibrium constant, in terms of the concentrations of reactants and products and determine the numerical value of the equilibrium constant, Kat this temperature. K=

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Starting with 0.500 M N, and 0.800 M H;, the reaction is allowed to
proceed until it reaches equilibrium. The [NHJo = 0.150M at 250°C.
Determine Kfor this reaction at this temperature.
4.
a)
Start by filling in the ICE table with the Initlal concentrations.
Reaction
(N] (M)
[H] (M)
[NH.J (M)
Initial
Change
Equilibrium
b)
Next, fill in the Changes in the system, in terms of x, which
will geseied by the atolchlometry. Reactants are used
up (-) and products are formed (*).
Next, write equilbrlum expressions, in terms of initial
concentrations and the changes that occur (x).
c)
d)
Salve for x from the information you have.
e)
Determine the equlibrium concentrations of N; and H.
(H -
Write the equation for K, the equilibrium constant, in terms
of the concentrations of reactants and producte and
determine the numerical value of the equilibrium constant,
Kat this temperature.
K=
Transcribed Image Text:Starting with 0.500 M N, and 0.800 M H;, the reaction is allowed to proceed until it reaches equilibrium. The [NHJo = 0.150M at 250°C. Determine Kfor this reaction at this temperature. 4. a) Start by filling in the ICE table with the Initlal concentrations. Reaction (N] (M) [H] (M) [NH.J (M) Initial Change Equilibrium b) Next, fill in the Changes in the system, in terms of x, which will geseied by the atolchlometry. Reactants are used up (-) and products are formed (*). Next, write equilbrlum expressions, in terms of initial concentrations and the changes that occur (x). c) d) Salve for x from the information you have. e) Determine the equlibrium concentrations of N; and H. (H - Write the equation for K, the equilibrium constant, in terms of the concentrations of reactants and producte and determine the numerical value of the equilibrium constant, Kat this temperature. K=
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