A flask contains this equilibrium Fe3+(aq) + SCN'-(aq) <======> FeSCN'-(aq) Which direction should equilibrium shift when...
Fe3+ (aq) + ow does the equilibrium shift a) if you add more Fe* SCN (aq) = FeSCN2+ (aq) Fes b) if you remove SCN c) if you remove FeSCN+2 d) if you add more Fe" and you remove FeSCN2 e) if you remove Fe" and you remove FeSCN+2
2. The stock solution at equilibrium used in test tube # 4 contains Fe3 (aq), SCN-(aq) and [FESCNP2 (aq). When NaOH was added to test tube #4 a shift in the equilibrium was observed. What chemical species in the stock solution reacted with NAOH? Write the balanced chemical reaction associated with the change observed from the addition of NaOH to test tube #4? Explain in terms of LeChatelier's Principle the observed results from the addition of 0.1 M KSCN to...
Calculate E°(cell) for the reaction, 2 103"(aq) + 10 Fe2+(aq) <=> 10 Fe3* (aq) + typen the reductor per Fe3+ (aq) + e* <=> Fe2+(aq), E = 0.87 V 2 103(aq) + 10 e<=> 12(aq), E° = 1.10 V A. -7.60 V B. 0.23 V C. -1.97 v D. 1.97 v E. -0.23 V
FesCN (aq), and LeChâtelier's Explain in terms of the equation, Fe" (aq) + SCN (aq) Principle (4 ) Observation after adding KSCN: turned darker more red like original solution brown Explain in terms of the equation, Fe (aq) + SCN (aq) + FeSCN- (aq), and LeChâtelier's Principle. (ps.) Observation after adding AgNO3: Turned milky white + thieverf less transparent Using the ions present in the solution, write a net ionic equation that would explain the precipitate observed Use the above...
Fe (aq)SCN-(aq) FeSCN (aq) thiocyanate iron(II) thiocyanoiron(il) Introduction When the reactants shown above, are combined, chemical equilibrium is reached rapidly. Once equilibrium is established, the equilibrium constant can be calculated if the concentration of all the ions are known: [FeSCNP.he [SCN-... and (Feng Your task is to prepare three different equilibrium systems that contain different concentrations of these ions. Keep in mind that although the concentrations will be different, the value of the equilibrium constant Ke will be indeed constant...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu2 (aq)Fe2 (aq)>Cu (aq) + Fe3 (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant than zero AGo for this reaction would be Submit Answer Retry Entire Group 9 more group attempts remaining Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cd2(aq)21(aq)>Cd(s)I2(s) Hint: Carry at least 5 significant figures during intermediate...
Resume < Question 6 of 10 > Attempt 1 - A standard solution of FeSCN is prepared by combining 9.0 ml of 0.20 M Fe(NO), with 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO3), + KSCN = FeSCN2+ + KNO, +2 NO; What allows us to assume that the reaction goes essentially to completion? The concentration of Fe(NO,), is much higher than the concentration of KSCN. The excess Fe" prevents the formation of...
QUESTION 4 Which is the correct equilibrium constant equation for the reaction indicated below? NH3(aq)+ H20() <-> NH4 (aq) + O(aq) [NH4 IOH K [H20]INH3] [NH4 IOH ] Ke [NH3] [H2O]INH3] Kc= [NH4 IOH [NH31 [NH4 11OH
For the reaction CHs (a) 3 H2 (a) <=---> CgH,2 (a) + heat Determine which of the following will shift the equilibrium to the left a) adding a catalyst b) decreasing the temperature c) increasing the pressure by decreasing the volume of the container d) increasing the concentration of H2 e) increasing the concentration of CeHe f) decreasing the concentration of C H12 g) more than one correct response h) no correct response O0000O
You are given the equilibrium system BiCl_3 (aq) bismuth (III) chloride(colorless) + H_2, O(l) BiOCl (s) bismuth(III) oxychloride (white) + 2HCl (aq) at a point at which the solution is colorless and no BiOCl (s) is observed. a. which way should the equilibrium shift, to the left or to the right, when water is added until a change is observed? What would be observed? Explain the shift in terms of lessthanorequalto Chatelier's principle. b. Which way should the equilibrium shift...