Interpretation:
The correct equilibrium expression (Kc) should be identified for the given aqueous phase (
Concept Introduction:
Equilibrium expression: The equilibrium expression is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divides by the concentrate ions of the product of reactants to the power of their coefficient.
Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.
Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.
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Chemistry: Atoms First
- Consider the following equilibrium for nitrous acid, HNO2 a weak acid: HNO2 (aq) + H2O (l) H30' (aq) + NO2(aq) ΔΗ > O 麷 m In which direction ( shift, if: -a) NaOH is added? Left, Right or No effect will the equilibrium Select l - b) NaNO2 is added? I Select ] c) HCI is added? I Select ] d) The acid solution is made more dilute? l Select Nextarrow_forward(b) N₂ (g) N2 (g) + 3H2 (g) 1 2NH3 (g) AH is negative From the given reaction at equilibrium above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of ammonial (b) Increasing the pressure (c) Increasing the temperature (d) Adding a catalyst (e) Increasing the concentration of hydrogen will shift the equilibrium position to the leftarrow_forwardDinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4(g) ⇌ 2NO2(g) A 1.00-L flask is initially charged with 0.400 mole of N2O4. At equilibrium at 373 K, 0.0055 mole of N2O4 remains. What is the equilibrium constant, Kc, for this reaction? (A) 28 (B) 72 (C) 110 (D) 140arrow_forward
- 9. The equilibrium constant for the reaction 2 BrCl (g) → Br2 (g) + Cl2 (g) at 25°C is Keq = 0.0172. What is the equilibrium constant for the reaction Br2 (g) + Cl2 (g) →2 BrCl (g)? (а) -0.0172 (b) 0.131 (c) 7.62 (d) 58.1 (e) none of thesearrow_forwardThe equilibrium constant for the equilibrium, 3A+ 2B ↔ 2D + E, is 4.22 x 10-3 . What is the equilibrium constant for the equilibrium: D + (1/2)E ↔ (3/2)A + B? (a)237 (b)2.11×10-3 (c)15.4 (d)-2.11×10-3arrow_forwardC Le Chatelier's Principle 3 Factors that affect the direction which a reaction will proceed to re-establish equilibrium are (A). (C) volume and (6) temperature Adding an inert noble gas or a equilibrium. to the system does Reaction 1: Ha (+12 (9) 2 HI (9) LState the direction (left/right) the reaction will shift te achieve equilibrium for each of the following cases. I. Explain the logic behind the shift in each of the following cases. (A) increasing temperature of the reaction (B) adding more Hi (g) Into the reaction (C) decreasing the pressure in the container (D) transferring the reaction mixture into a smaller container. (E) adding more 12 (s) into the reaction system: (F) adding some Neon gas into the system: (G) placing a catalyst into the reaction vessel: affect the direction a reaction will go to achieve AH- +52 KJarrow_forward
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- 3. Several reactions are listed below with their equilibrium constant values. Place an "X" in the appropriate box in the Table to indicate your prediction for the direction of the reaction to produce mostly products (proceed Right) or mostly reactants (proceed Left)? Why? Equilibrium Reaction and/or Condition (a) NH4*(aq) + H₂O(l) NH3 (aq) + H3O+ (aq) (b) Mb + O₂ MbO2 (c) If Q = 8.3 x 106 for (b) above (d) If Q=1500 for (b) above (e) If for (b) above the following initial conditions exist: [Mb], = 2.04 x 104; [0₂]o= 3.00 x 10° M; [MbO₂]0=2.50 x 104 M (f) H₂SO3(aq) H*(aq) + HSO3(aq) K = 5.6 x 10-10 K = 8.6 x 105 K = 8.6 x 105 K = 8.6 x 105 K = 8.6 x 105 K = 0.0120 R L Reasonarrow_forward1.1 (b) AH is negative N₂ (g) + From the given reaction at equilibrium above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of ammonia 3H2(g) (b) Increasing pressure (c) Increasing the temperature (d) Adding a catalyst 2NH3 (e) Increasing the concentration of hydrogen will shift the equilibrium position to the left (State True or False)arrow_forward1.1 (b) negative N₂ + (b) Increasing pressure 3H₂ From the given reaction at equilibrium above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of ammonia (c) Increasing the temperature (d) Adding a catalyst 2NH₂(g) DH is (e) Increasing the concentration of hydrogen will shift the equilibrium position to the left (State True or False)arrow_forward
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