since the concentration of water is constant throughout the reaction it will not affect the value of equilibrium constant.
concentration of complex formed as product is 0.016 means that 0.016 moles of each component in the reactant is involved in the reaction to produce the complex .hence
equilibrium concentration of reactants are 0.025-0.016=0.009 and 0.050-0.016=0.034 respectively
we know that the equilibrium constant of a particular reaction is the ratio of product of concentration of product to the concentration of reactants
kc=(0.016*0.016)/(0.009*0.034)
=0.8366
The reaction between the compound [Fe (H2O).] (NO3)3 and Na (NSC) produces a red ferric thiocyanate...
The reaction between the compound [Fe (H2O).) (NO3)2 and Na (NSC) produces a red ferric thiocyanate complex, [Fe (H2O):(NSC)] (NO3)2. Initial concentration of [Fe (H2O).) (NO3)3 and Na (NSC) were determined to be 0.025M and 0.050M. Equilibrium concentration of [Fe (H2O)s(NSC)) (NO3)2 was determined to be 0.016M. Calculate the equilibrium, Kc. [Fe (H20).] (NO3)2 (aq) + Na (NSC) (aq) → [Fe (H2O):(NSC)] (NO3)2 (aq) +NaNO3(aq) + H20(1)
15. The pH of a solution of ferric nitrate, Fe(NO3)3, is not 7.00. This fact is best explained by the equation: A) NO3-(aq) + H2O(1) + HNO3(aq) + OH(aq) B) Fe3+(aq) + 6 H2O(1) Fe(OH)3(aq) + 3 H30+(aq) C) [Fe(OH2)6]3+(aq) + H20(1) 3 H3O+(aq) + [Fe(OH2)5(OH)]2+(aq) D) H3O+(aq) + OH-(aq) + 2 H2O(1) E) HNO3(aq) + H2O() H30+(aq) + NO3-(aq)
In this experiment, we will be studying the reaction of the iron(III) ion with the thiocyanate ion to form the red-colored complex ion pentaaquathiocyanatoiron(III), [Fe(H20)s(SCN)]?". As we will learn later, the Fetion in water is actually better represented as a complex ion with 6 water molecules attached to the central iron, [Fe(H20)] (aq). The SCN ion replaces one of the water molecules attached to the Fe" in the following reaction. [Fe(H2O).] (aq) + SCN (aq) [Fe(H2O)(SCN)]2(aq) + H2O(1) AH° (-)...
In a dilute nitric acid solution, Fe3+ reacts with thiocyanate ion (SCN−) to form a dark red complex: [Fe(H2O)6]3+ + SCN− ⇌ H2O + [Fe(H2O)5NCS]2+ The equilibrium concentration of [Fe(H2O)5NCS]2+ may be determined by how dark the colored solution is (measured by a spectrometer). In one such experiment, 1.0 mL of 0.20 M Fe(NO3)3 was mixed with 1.0 mL of 9.2 ×10−3M KSCN and 8.0 mL of dilute HNO3. The color of the solution quantitively indicated that the [Fe(H2O)5NCS]2+ concentration was...
The metathesis reaction between iron (III) nitrate and sodium sulfide is shown below 2 Fe(NO3)3(aq) + 3 Na2S (aq) ➝ 6 NaNO3(aq) + Fe2S3(s) How many grams of solid iron (III) sulfide can be produced by the reaction of 250.0 ml of 0.400 M iron (III) nitrate solution with 350.0 ml of 0.250 M sodium sulfide solution? Determine the final concentration of each ion in solution at the end of the precipitation reaction. Na+ NO3– Fe+3 S–2
The reaction of cobalt(II) nitrate and potassium thiocyanate produces a coloured complex, [Co(SCN)4]2-(aq). The initial concentrations of the reactants after mixing (before any reaction) were 0.250 mol/L Co(NO3)2(aq) and 0.500 mol/L KSCN (aq). After 20 minutes, the absorbance of the solution was 0.825. The complex, [Co(SCN)4]2-, is the only absorbing species (ε b = 9.29 (mol/L)-1). Determine the concentration of Co2+ at equilibrium.
The reaction of cobalt(II) nitrate and potassium thiocyanate produces a coloured complex, [Co(SCN)4]2-(aq). The initial concentrations of the reactants after mixing (before any reaction) were 0.250 mol/L Co(NO3)2(aq) and 0.500 mol/L KSCN (aq). After 20 minutes, the absorbance of the solution was 0.825. The complex, [Co(SCN)4]2-, is the only absorbing species (ε b = 9.29 (mol/L)-1). Determine the concentration of Co2+ at equilibrium. The reaction of cobalt(II) nitrate and potassium thiocyanate produces a coloured complex, Co(SCN).J(aq). The initial concentrations of...
HW 14 <Question 24 (of 29) 0.68 points 10 attempts left Check my work Enter your answer in the provided box. In a dilute nitric acid solution, Fe' reacts with thiocyanate ion (SCN) to form a dark red complex: [Fe(H2O)6]3t + SCN-→ H2O + [Fe(H2O)sNCS] 2+ The equilibrium concentration of [Fe(H,oNCSmay be determined by how dark the colored solution is (measured by a spectrometer). In one such experiment, 1.0 mL of 0.20 M Fe(NO)s was mixed with L.0 mL of...
1. A student mixes 5.00 mL of 2.00 x 10 M Fe(NO3)3 with 5.0 mL of 2.00 x 10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN+2 is 1.2 x 104 M. Find the Kc for the reaction of Fe (aq) + SCN (aq) → FeSCN2(aq) using the following steps. a. Find the initial concentration of Fe and SCN. (Use Equation 4). Record the value in the ICE Chart below. b. What is the equilibrium...
Complete &Balance the following Reaction: Fe(NO3)3(aq)+Na2S (aq) 2Fe(NO3)3(aq)+ 3Na2S(aq) --> Fe2S3ls)+ 6NaNO3 (aq) OFe(NO3)3laq)+Na S(aq)>Na(N03)alaq) + FeSls) O3Fe(NO3)3(aq)+2Na S(aq)Fe3S2(s)+4NaNO3 (aq) Fe(NO3)3(aq)+ Na2S(aq)FeS3(s) NagNO3 (aq)