A) moles of iron nitrate = 0.2*10 = 2 millimole
moles of KSCN = .001 * 1 = .001 millimole
total volume = 20 ml
0.001 milli mole of KSCN will react to form .001 millimole of FeSCN
concentration of FeSCN = (.001/1000)/( 20*1000) = .00005 M
B)
moles of iron nitrate = 0.2*10 = 2 millimole
moles of KSCN = .001 * 2 = .002 millimole
total volume = 20 ml
0.002 milli mole of KSCN will react to form .002 millimole of FeSCN
concentration of FeSCN = (.002/1000)/( 20*1000) = .0001 M
C)
moles of iron nitrate = 0.2*10 = 2 millimole
moles of KSCN = .001 * 3 = .003 millimole
total volume = 20 ml
0.003 milli mole of KSCN will react to form .003 millimole of FeSCN
concentration of FeSCN = (.003/1000)/( 20*1000) = .00015 M
moles of iron nitrate = 0.2*10 = 2 millimole
moles of KSCN = .001 * 1 = .001 millimole
total volume = 20 ml
0.001 milli mole of KSCN will react to form .001 millimole of FeSCN
concentration of FeSCN = (.001/1000)/( 20*1000) = .00005 M
D)
moles of iron nitrate = 0.2*10 = 2 millimole
moles of KSCN = .001 * 4 = .004 millimole
total volume = 20 ml
0.004 milli mole of KSCN will react to form .004 millimole of FeSCN
concentration of FeSCN = (.004/1000)/( 20*1000) = .0002 M
E) zero KSCN added so no FeSCN formed .
Q&A CH2630 LB (5 points) Name: Given the information in Table 1 below, calculate the concentrations...
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....
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...
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...
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...
1. You prepare a mixture to use to create a colorimetry calibration curve for FeSCN2+ by mixing these things in a 25.00 mL volumetric flask and then diluting to the volume of the flask with 0.3 M HNO3. 5.00 mL 0.00200 M NaSCN 10.00 mL 0.30 M Fe(NO3)3 What is the concentration of FeSCN2+ in this mixture? [Pay attention to the values to determine which reactant is being driven to completely react...] 2. You prepare a mixture to use to...
Use the information in the Table below to calculate the concentrations of [Fe3+], [SCN-] and [FeSCN2+]. Can you check to see if the concentrations in the first table is correct also? Solution 0.05M 0.00200M 0.200M [Fe(NO3)3FeSCN2 [KSCN] HNO3 KSCN Fe(NOs)3 0.04 M 5.0 mL 2.0 x 10 M 1 17.5 mL 2.5mL 2.0 x 104 M 0.04 M 18.0 mL 2.0 mL 2 5.0 mL 1.6 x 104 M 1.6 x 104 M 0.04 M 1.5 mL 3 18.5 mL...
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...
are theses correct? please correct me if they are not. Results Fe Test Tube 2: FeSCN (aa) SCN () Fe Chemical equation: Explanation: The equilibrium shifted toward the increased the due to the addition of Fe(NO,)) because it of the Test Tube 3: FESCN 0) SCN () (as Chemical equation: Fe(ag) Explanation: Test Tube 4: Chemical equation: Fe(agk FeSCN( (aq)h Explanation: Test Tube 5: Chemical equation: Fe"( SCN () FESCN 3+ + (sq) Explanation: Test Tube 6 Chemical equation: Fe(a...
Data and Calculations: Determination of the Equilibrium Constant for a Chemical Reaction Method II Volume in mL 2.00 x 103 M Fe(NO) Volume in mL, Depth in mm Volume in ml. 2.00 x 103 M Method I Mixture Unknówn KSCN Water Absorbance Standard FESCNP 4mL 1 5.00 x 10 M 1,00 .227 3mL 2 5,00 202 x 10 M 2,00 90 x 10 M .304 3 5,00 3.00 2mL 955 x 104 M I ImL 4 5.00 4,00 19x 10...
please do 1 through 4. Thank you. 0 1. Fe 1.SCN Procedure B: 1. Prepare ICE tables for beakers 2 - 6 using the example below as a guideline (you will have 5 different ICE tables). Table 3. Sample "ICE" table. Fe(aq)*3 + SCN(aq) = FeSCN2 Initial: **M calculated **M calculated using your Table 2 using your Table 2 volumes volumes Change: - 1x - 1x Equilibrium: M 1x 1x = concentration calculated from Procedure A slope-intercept equation +1x M...