Question 3 Write an equilibrium constant expression for the following heterogeneous equilibrium: MnO₂ (s) + H₂O (1) + SO3- (aq) →→→→Mn(OH)₂ (s) + SO² (aq) О Кс Ο Kg = О Кс О Кс [sO] (so; ] [sol] (SO H₂O [SO Mn(OH)₂ [SO]H₂OMnO₂] [SO][MnO₂ [So Mn(OH)₂) [s0 H₂O[MnO₂l
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![Question 3
Write an equilibrium constant expression for the following heterogeneous equilibrium:
MnO₂ (s) + H₂O (1) + SO3- (aq) + Mn(OH)₂ (s) + SO² (aq)
О Кс=
О Ко
О Кс
О Кс
О Кс
[SO]
[SO]
[SO]
(SO ₂0
[SO Mn(OH)₂
[SO][H₂OMnO₂]
[SO][MnO₂]
[SO][Mn(OH)₂)
[So ][H₂OMnO₂l
[SO Mn(OH)₂]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff3a38996-6782-40c2-af9f-f624a7021da3%2Fa9966eb6-291b-4f6f-8c85-7f23e363f4c8%2Fg3f7se_processed.jpeg&w=3840&q=75)
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- Observations and Interpretations 1) Balance the chromate / dichromate equilibrium equation: CrO42-(aq) + H+(aq) Cr2O72-(aq) + H2O(l) (unbalanced equation) 2) What was the original color of the K2CrO4 solution? If the above equilibrium is established in the original solution, which species, CrO42-(aq), or Cr2O72-(aq) appears to be present in greatest amount? 3) What color did you observe after adding the 3M H2SO4 solution? 4) What color did you observe after adding the 1M NaOH solution? 5) Assume that the dynamic equilibrium represented in the equation in 1 is present in the original solution you placed in the test tube. Based on LeChatelier’s Principle, as stated above on page one, you will interpret the observations made in 2, above: (Notethat H2SO4 produces H+ in solution.) a) When sulfuric acid was added, which reaction (forward or reverse) was favored? What evidence supports this? Why would this reaction be…Observations and Interpretations 1) Balance the chromate / dichromate equilibrium equation: CrO42-(aq) + H+(aq) Cr2O72-(aq) + H2O(l) (unbalanced equation) 2) What was the original color of the K2CrO4 solution? If the above equilibrium is established in the original solution, which species, CrO42-(aq), or Cr2O72-(aq) appears to be present in greatest amount? 3) What color did you observe after adding the 3M H2SO4 solution? 4) What color did you observe after adding the 1M NaOH solution? 5) Assume that the dynamic equilibrium represented in the equation in 1 is present in the original solution you placed in the test tube. Based on LeChatelier’s Principle, as stated above on page one, you will interpret the observations made in 2, above: (Notethat H2SO4 produces H+ in solution.) a) When sulfuric acid was added, which reaction (forward or reverse) was favored? What evidence supports this? Why would this reaction be…The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq) which is a common ion then what would be the concentration of the Arsenate ion AsO43-(aq) in grams per Liter at equilibrium? Question 15 options: 2.44 3.31 4.47 4.23 2.61 3.02 3.78 3.96 2.87 3.57
- 3.) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to dissolve 2.52 g of CuCl2 in 1.000 L of a solution 0.946 M in NaCN. The addition of CuCl2 does not alter the volume (the final volume is still 1.000 L).If the equilibrium constant for a reaction A + B <=> 2C is measured as Keq = 1.318. What would the value be for the same reaction if written as 2C <=> A + B. Keq' = ____. 3 sig. fig.Observations and Interpretations 1) Balance the chromate / dichromate equilibrium equation: CrO42-(aq) + H+(aq) Cr2O72-(aq) + H2O(l) (unbalanced equation) 2) What was the original color of the K2CrO4solution? If the above equilibrium is established in the original solution, which species, CrO42-(aq), or Cr2O72-(aq) appears to be present in greatest amount? 3) What color did you observe after adding the 3M H2SO4 solution? 4) What color did you observe after adding the 1M NaOH solution? 5) Assume that the dynamic equilibrium represented in the equation in 1 is present in the original solution you placed in the test tube. Based on LeChatelier’s Principle, as stated above on page one, you will interpret the observations made in 2, above: (Notethat H2SO4 produces H+ in solution.) a) When sulfuric acid was added, which reaction (forward or reverse) was favored? What evidence supports this? Why would this reaction be…
- Consider the insoluble compound copper(II) carbonate , CuCO3 . The copper(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Cu(NH3)42+ , Kf = 6.8×1012 . Be sure to specify states such as (aq) or (s). + + KGive only typing answer with explanation and conclusion This is a numerical problem. Report your answer to three decimal places. Do NOT include units. A reaction with 0.1500 M Fe(NO3)3 is reacted with a solution of [SCN-] M SCN. The amount of 02+at equilibrium is determined to be 0.067. What is the amount of Fe(NO3)3 at equilibrium?3. A weak electrolyte with initial concentration of 0.500 M HA undergoes 1.20 % ionization to reach equilibrium. What is the value of the ionization constant of HA? A. 1.80 x 10-5 B. 0.010 C. 0.0204 D. 7.29 x 10-5 E. 2.04 x 10-4
- For the reaction, 2NH3(g)--> <---3H2 (g)+ N2 (g) the equillibrium concentrations were found to be [NH3 ]=0.250 M, [H2 ]=0.540 M, and [N2 ]= 0.750 M. What is the equilibrium constant for this reaction? Kc=?Write the equilibrium constant for the following reactions: a. 3NO(g) ↔ N2O(g) + NO2(g) b. Ni(CO)4(g) ↔ Ni(s) + 4CO(g) c. C(s) + 2H2(g) ↔ CH4(g)Consider the reaction IO−4(aq)+2H2O(l)⇌H4IO−6(aq);Kc=3.5×10−2IO4−(aq)+2H2O(l)⇌H4IO6−(aq);Kc=3.5×10−2 If you start with 22.0 mLmL of a 0.908 MM solution of NaIO4NaIO4, and then dilute it with water to 500.0 mLmL, what is the concentration of H4IO−6H4IO6− at equilibrium? Express your answer to two significant figures and include the appropriate units.