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EQUILIBRIUM LAW

EQUILIBRIUM LAW. When you use concentration data to FIND OUT whether you can get a constant value by manipulating it, you are finding Q, the reaction quotient. E.g. 2HI  H 2 + I 2 These are all Q values. These constant values indicate the equilibrium law.

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EQUILIBRIUM LAW

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  1. EQUILIBRIUM LAW

  2. When you use concentration data to FIND OUT whether you can get a constant value by manipulating it, you are finding Q, the reaction quotient. E.g. 2HI  H2 + I2 These are all Q values. These constant values indicate the equilibrium law.

  3. K is the equilibrium constant at a given temperature (no units) General equation: K = Where [X] means molar concentration of X m, n are coefficients from balanced equation

  4. e.g. For 2NO(g) + O2(g) 2NO2(g) K = [NO2]2 [NO] 2[O2] Write the equilibrium law for a) 2H2 + O2 2H2O b) 3H2 + N2  2NH3 a) K = [H2O]2 b) K = [NH3]2 [H2]2[O2 ] [H2]3[N2]

  5. If the concentrations for the substances in the equilibrium 3H2 + N2  2NH3 are [H2] = 0.521 mol/L, [N2] = 0.171 mol/L, and [NH3] = 0.285 mol/L at 300 K, what is the equilibrium constant for that temperature? K = [NH3]2 [H2]3[N2] K = 3.36 What does a large K indicate about the position of the equilibrium? Small K?

  6. If the equilibrium constant for the reaction 2H2 + O2 2H2O at 600C is K=7.32×105, and concentra-tions of these substances in a closed system are [H2] = 5.81×103 mol/L, [O2] = 9.16×104 mol/L, and [H2O] = 7.33×106 mol/L, is the system at equilibrium? *Find Q and compare to K Q = [H2O]2 [H2]2[O2 ] Q = 1.74×103  K not at eqbm.

  7. In what direction must the water system shift to attain equilibrium? The position of the equilibrium must shift toward reactants, so that the value of Q gets smaller.

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