5.00 mL of .00400 M Fe3+ and 5.00 mL of .00400 M SCN- are mixed and an absorbance of 1.987 is obtained. Calculate the equilibrium constant to 3 significant figures. Є =2900
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5.00 mL of .00400 M Fe3+ and 5.00 mL of .00400 M SCN- are mixed and...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250 M NaSCN, the following reaction occurs: Fe3+ (aq) + SCN(aq) $ FeSCN2+(aq) At equilibrium the concentration of FeSCN2- is found to be 6.00 x 10-2 M. A. Fill in the table below with the proper numerical values. (Remember to take into account the effects of dilution when calculating the initial molarity of Fe3+ (aq) and SCN'(aq) Fes- (aq) SCN (aq) FeSCN-(aq) Initial Molarity Change...
3. An equilibrium solution was prepared by mixing 3.20 mL of 0.00200 M SCN ,5.00 mL of 0.00200 M Fe3+, and 1.80 mL of 0.050 M HNO, Calculate the initial concentrations of SCN and Fe' in the solution
How do I calculate [SCN-]i given that:
Stock [Fe3+] = 0.00200 M
Stock [SCN-] = 0.00200 M
[Fe+3] [SCN]: of Table 2. Initial Data to Determine Keq Trial Volume Volume Total | Absorbance of Fe+3 volume KSCN(mm) (mm) (mL) hao 5.00 10.00 10.110 | 2 200 5.00 10.00 0.225 3 3.00 5.00 10.00 0.359 4 4.00 5.00 10.00 0.479 5 5.00 5.00 10.00 0.626 11.00×10 -3 2.00x104
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-] = 1.239; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.454 M. What is the numerical value of KC for this equilibrium? KC = __________________ 2) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.370; [SCN-] = 0.777; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.285 M. What is the equilibrium concentration of Fe3+? [Fe3+]eq =...
Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M and an initial [SCN−] of 8.2×10−4 M . At equilibrium, [FeSCN2+]= 1.8×10−4 M . Calculate the value of the equilibrium constant (Kc)(Kc). Express your answer using two significant figures.
For this equilibrium : Fe3+ + SCN- <====> [FeSCN]2+ If Z = 4.28103 M -1. A solution at equilibrium that initially contained 1.59 x10-3[SCN] and 8.46x10-4 M [Fe2+] was found to have an absorbance of 0.402 units. What is the equilibrium constant? please explain
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M. Part A: Calculate the number of moles of Fe3+ initially added to the solution. Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium....
A 25.0 mL volume of 0.0200 M Fe(NO3)3 is mixed with 50.0 mL of 0.00200 M NaSCN and 25.0 mL of 0.100 HNO3. The blood-red FeSCN2+ ion forms and the equilibrium is established: Fe3+(aq) + SCN-(aq) <---> FeSCN2+(aq) The equilibrium concentration of FeSCN2+ ([FeSCN2+]) was measured spectrophotometrically and found to be 7.0 x 10-4 mol/L. To calculate the equilibrium constant (Kc) for thr equilibrium system, proceed through the following steps: A. Moles of Fe3+, initial B. Moles of SCN-, initial...
-Equilibrium Concentration of [Fe(SCN)2+] – Reacted Concentration of Fe3+ – Reacted Concentration of SCN- – Equilibrium Concentration of Fe3+ – Equilibrium Concentration of SCN- – Equilibrium Constant, Kc M(Fe) M(SCN) 0.00229 0.00206 Test Solutions Concentration Absorbance 1 0 0 2 0.0000618 0.154 3 0.000103 0.22 4 0.000144 0.352 5 0.000206 0.514 From Graph: y = 0.1226x - 0.1198 R² = 0.9844
Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL 2.00 × 10−3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28 × 10−4 M. Find Kc for the reaction Fe3+(aq) + SCN−(aq) ↔ FeSCN2+(aq). a. What is the initial concentration of Fe3+ in the reaction mixture? [Fe3+] = ___ x 10-3 M b. What is the initial concentration of SCN- in the reaction mixture? [SCN-] = ___...