At a certain temperature, the equilibrium constant, Ke, for this reaction is 53.3. H₂(g) + L₂(g) 2 HI(g) Kc = 53.3 At this temperature, 0.300 mol H₂ and 0.300 mol I₂ were placed in a 1.00 - L container to react. What concentration of HI is present at equilibrium? Set up an ICE table using the initial conditions provided in the question for the "I" row. To help determine the "C" row, find Qc. If Qe Ke, reaction will move in reverse. [HI]= M

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At a certain temperature, the equilibrium constant, Ke, for this reaction is 53.3.
H₂(g) + L₂(g) = 2 HI(g)
Kc = 53.3
At this temperature, 0.300 mol H₂ and 0.300 mol 1₂ were placed in a 1.00 - L container to react.
What concentration of HI is present at equilibrium?
Set up an ICE table using the initial conditions provided in the question for the "I" row. To help determine the "C" row, find Qc.
If Qc <Kc, reaction will move forward, if Qc > Kc, reaction will move in reverse.
[HI]=
M
Transcribed Image Text:At a certain temperature, the equilibrium constant, Ke, for this reaction is 53.3. H₂(g) + L₂(g) = 2 HI(g) Kc = 53.3 At this temperature, 0.300 mol H₂ and 0.300 mol 1₂ were placed in a 1.00 - L container to react. What concentration of HI is present at equilibrium? Set up an ICE table using the initial conditions provided in the question for the "I" row. To help determine the "C" row, find Qc. If Qc <Kc, reaction will move forward, if Qc > Kc, reaction will move in reverse. [HI]= M
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