For the reaction below, the concentration of HI is 0.210 M and the concentrations of H₂, and 1₂ are both 0.564 M. What must happen for the reaction to reach equilibrium?

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Question 9 of 17
For the reaction below, the concentration of
HI is 0.210 M and the concentrations of H₂,
and 1₂ are both 0.564 M. What must happen
for the reaction to reach equilibrium?
=
2 HI (g) H₂ (g) + 1₂ (g) Kc = 7.21 (Note Kc
is sometimes called K.)
A) The reaction needs to shift in the
forward direction.
Submit
B) The reaction needs to shift in the reverse
direction.
C) The reaction is already at equilibrium
and no shift needs to take place.
D) There is not enough information to
determine how the reaction will reach
equilibrium.
Tap here or pull up for additional resources
Transcribed Image Text:9:43 Question 9 of 17 For the reaction below, the concentration of HI is 0.210 M and the concentrations of H₂, and 1₂ are both 0.564 M. What must happen for the reaction to reach equilibrium? = 2 HI (g) H₂ (g) + 1₂ (g) Kc = 7.21 (Note Kc is sometimes called K.) A) The reaction needs to shift in the forward direction. Submit B) The reaction needs to shift in the reverse direction. C) The reaction is already at equilibrium and no shift needs to take place. D) There is not enough information to determine how the reaction will reach equilibrium. Tap here or pull up for additional resources
Expert Solution
Step 1

To determine how the reaction will reach equilibrium, we need to compare the initial reaction quotient, Qc, to the equilibrium constant, Kc. The reaction quotient is calculated in the same way as the equilibrium constant, except that it uses the initial concentrations of the reactants and products rather than the concentrations at equilibrium.

 

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