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Chem 136 Winter 2019 Table 6. Caleulation of the Equilibrium Constant for the Reaction. moles Fe ...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part...
. 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...
Data and Calculations: Determination of the Equilibrium Constant for a Chemical Reaction Method II Volume in...
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...
I. Write the equilibrium constant expression, K for the following reaction Fe"(ag) FENCS(ag) SCN (ag) + CFENCS D 2....
I. Write the equilibrium constant expression, K for the following reaction Fe"(ag) FENCS(ag) SCN (ag) + CFENCS D 2. In part A of Experiment 34, it was assumed that all of the SCN added to the reaction mixture was converted to product (FeNCS). Which of the following best explains why that assumption was valid? A) The moles of Fe added equaled the moles of SCN- added. B) In part A, the SCN was the limiting reactant whereas in part B,...
9. Using the reaction below and mixture 1 volumes, a student mixes Foon with KSON n c equilibrium concentrations at 5.71 x 10 M and 3.71 x10+ M, respectively net absorbance of mixture l at 0.090....
9. Using the reaction below and mixture 1 volumes, a student mixes Foon with KSON n c equilibrium concentrations at 5.71 x 10 M and 3.71 x10+ M, respectively net absorbance of mixture l at 0.090. The calibration curve for the equilibrium reactions,-2635 x+0.014. Using the colormetet, she oin the Fe (aq SCN (aq)FescN (ad) a. Using the calibration curve, where y is equal to the absorbance Lapplying the Beer's Law: Absorbance slope (concentration), calaulate the eauilinium con b. Write...
Beers law solve for E3 and E4 showing work Part II. Equilibrium Constant Calculations Calculate the...
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...
equilibrium help!! What is the equilibrium constant for the reaction CO(g) + 3 H2(g) - CH4(g)...
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...
chem 202 determining the equilibrium constant solution set 2 need help filling out the last 4...
chem 202 determining the equilibrium constant solution set
2
need help filling out the last 4 columns. more specifically,
how do I determine "x"
heres a clearer picture, the numbers filled in the other rows
have already been confirmed.
moll' i molt m SON X blank per f ometric Determination of an Equilibri Table 2: Determining the Equilibrium Constant (Solution Set 12) directions on pp. 6-3-64 Constant Report volume of target and Retual volume Initial Solution equilibrim Fe(HO) Volumes or...
Using an equilibrium constant to predict the direction of spontan.. A chem - gineer is studying...
Using an equilibrium constant to predict the direction of spontan.. A chem - gineer is studying the following reaction: HCN(aq)+NH3() CN (aq)+NH(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.2 The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below....
I dont need #6 NOTES S Br HO Br HyO Br- Br он Br Br но...
I
dont need #6
NOTES S Br HO Br HyO Br- Br он Br Br но Br Br но Brm Formula B НBrm Formula A (color) (color) HBrm +H,O-Brm+H,O Figure 8.1. Protonation and deprotonation of HBrm. Prelab As part of your individual preparation for lab, read the experiment and answer the following questions in your lab notebook before going to lab. The copy of your answers on perforated pages from your lab notebook is due at the begin- ning of...
2. If the reaction between iron(III) ion and thiocyanate ion yielded an equilibrium concentration of 0.30...
2. If the reaction between iron(III) ion and thiocyanate ion yielded an equilibrium concentration of 0.30 M for each of these ions, what is the equilibrium concentration of the red iron(III)-thiocyanate complex? (Hint: The equilibrium constant for the reaction is in the Background section.) Show your work 3. In the reaction below, NH3(g) + H2O(1) - NH; +H30+ the equilibrium constant is 10-34. Is this reaction likely to take place? Explain your answer. iron(III) and thiocyanate ions, the equilibrium expression...
. 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...
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...
I. Write the equilibrium constant expression, K for the following reaction Fe"(ag) FENCS(ag) SCN (ag) + CFENCS D 2. In part A of Experiment 34, it was assumed that all of the SCN added to the reaction mixture was converted to product (FeNCS). Which of the following best explains why that assumption was valid? A) The moles of Fe added equaled the moles of SCN- added. B) In part A, the SCN was the limiting reactant whereas in part B,...
9. Using the reaction below and mixture 1 volumes, a student mixes Foon with KSON n c equilibrium concentrations at 5.71 x 10 M and 3.71 x10+ M, respectively net absorbance of mixture l at 0.090. The calibration curve for the equilibrium reactions,-2635 x+0.014. Using the colormetet, she oin the Fe (aq SCN (aq)FescN (ad) a. Using the calibration curve, where y is equal to the absorbance Lapplying the Beer's Law: Absorbance slope (concentration), calaulate the eauilinium con b. Write...
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...
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...
chem 202 determining the equilibrium constant solution set
2
need help filling out the last 4 columns. more specifically,
how do I determine "x"
heres a clearer picture, the numbers filled in the other rows
have already been confirmed.
moll' i molt m SON X blank per f ometric Determination of an Equilibri Table 2: Determining the Equilibrium Constant (Solution Set 12) directions on pp. 6-3-64 Constant Report volume of target and Retual volume Initial Solution equilibrim Fe(HO) Volumes or...
Using an equilibrium constant to predict the direction of spontan.. A chem - gineer is studying the following reaction: HCN(aq)+NH3() CN (aq)+NH(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.2 The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below....
I
dont need #6
NOTES S Br HO Br HyO Br- Br он Br Br но Br Br но Brm Formula B НBrm Formula A (color) (color) HBrm +H,O-Brm+H,O Figure 8.1. Protonation and deprotonation of HBrm. Prelab As part of your individual preparation for lab, read the experiment and answer the following questions in your lab notebook before going to lab. The copy of your answers on perforated pages from your lab notebook is due at the begin- ning of...
2. If the reaction between iron(III) ion and thiocyanate ion yielded an equilibrium concentration of 0.30 M for each of these ions, what is the equilibrium concentration of the red iron(III)-thiocyanate complex? (Hint: The equilibrium constant for the reaction is in the Background section.) Show your work 3. In the reaction below, NH3(g) + H2O(1) - NH; +H30+ the equilibrium constant is 10-34. Is this reaction likely to take place? Explain your answer. iron(III) and thiocyanate ions, the equilibrium expression...
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