Data and Calculations: Determination of the Equilibrium Constant for a Chemical Reaction Method II Volume in...
Section Name Experiment 23 Advance Study Assignment: Determination of the Equilibrium Constant for a Chemical Reaction 1. A student mixes 5.00 mL 2.00 X 10M Fe(NO), with 5.00 ml 2.00 x 10-M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN is 1.40 x 10M. Find K for the reaction Fe(aq) + SCN (aq) FeSCN2(aq). Step 1 Find the number of moles Fe and SCN initially present. (Use Eq. 3.) (5.00 x103 LX (300X163) = (x 103...
Beers law solve for E3 and E4 showing work Part II. Equilibrium Constant Calculations Calculate the initial moles of Fe3+ and SCN- for solutions E2 through E6 and record these values in the table on your Data Sheet. You obtain the moles of the reactants by multiplying their molarity by the volume (in L) of their solution used. Determine the equilibrium concentration of FeSCN2+ for each of the solutions E2-E6 from your Beer’s Law plot. Using these equilibrium concentrations, the...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part II (y values and the best-fit line equation from Part I to calculate the [FeSCN2"), at equilibrium. Show two sets of calculations and complete Table 6 below. Sample Calculation with hypothetical values of Absorbance from Table 4 & fitted egn. from Table 3 y = mx + b (y is absorbance) 0.0620 - 2000x -0.0250 x-0.0620+ 0.0250 2000 = 4.35 x 10 с D...
equilibrium help!! What is the equilibrium constant for the reaction CO(g) + 3 H2(g) - CH4(g) + H2O(g) if at 20 °C the equilibrium molar concentrations are [CO] -0.613, [H2] = 1.839, (CH4) = 0.387, and [H20) - 0.387? Format Β Ι Ο The reaction for the formation of the diamine-silver ion is as follows: Ag (aq) + 2NH3(aq) + Ag(NH3)2(aq) a. Write the equilibrium constant expression for this reaction. for the above b. An experiment was carried out to...
What's the concentration of [FeSCN2+] using limiting reactant theory and equation? For each test tube solution enter the initial concentration of Fe+ and SCNthe equilibrium concentration of FeSCN2: into the ICE table given. Complete entries for the rest of the table and calculate the K value for each of the tables. The values of K should be confined to a narrow range to reflect constancy. Comment on the quality of your work in this regard and calculate the average K....
can you please help me with this Data and Calculations Trial 0:29 Absorbance 0.378 Je 0.086 Trial 2 0.47 Trial 3 0.632 Trial 4 0.729 0.686 Absorbance of standard Triw. 329 0.6 6 Temperature ke [Fe(SCN) 2+]/([Fe3+] [SCN-]) Ferrag) + SCN Cag) 2 FescN2t (ag) Absorbance of standard (Trial) Temperature 0.3 Ke expression: [Fe] 0.0010 [SCN) 10.00040 [FeSCN? Jeg [Fe [SCN ] Ke value Average of Ke values Percent error (see pg 7): (Discuss this result as part of your...
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...
A student made solution #3 using the experimental method in this lab, and measured an absorbance of 0.559. The starting reagents are 2.00 x 10-3 M Fe(NO3)3 and 2.00 x 10-3 M KSCN. The amount of absorption is proportional to the concentration of FeSCN2+. This relationship – true for many solutions – is called “Beer’s Law”, and has the simple equation: A = bc where “A” is the absorption, “b” is 5174.6 for FeSCN2+ and “c” is molarity Make Five...
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-] = ___...
For each equilibrium sample, calculate the initial concentrations (assuming no reaction occurred) of SCN– and Fe3+ based on the dilution factors used. Enter the absorbance values for each sample. For the standard solution, assume that, when equilibrium is reached, the [FeSCN2+]eq is equal to [SCN–]ini. Why is this a good assumption? For the equilibrium solutions, calculate the [FeSCN2+]eq (Ceq) using Eq. 4. Using Eq. 5 and 6, calculate [Fe3+(aq)]eq and [SCN–(aq)]eq for each equilibrium solution. Calculate values for the equilibrium...