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Equilibrium Concentrations for a Simple Addition Reaction At a certain temperature K = 1.10x103 for the reaction: Fe3+(...
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-]...
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 =...
Equilibria can be treated mathematically with the equilibrium constant, K. For the reaction Fe3+ + SCN...
Equilibria can be treated mathematically with the equilibrium
constant, K. For the reaction Fe3+ + SCN − equilibrium reaction
arrow FeSCN2+, the equilibrium constant expression is [FeSCN2+ ] K
= [Fe3+ ] · [SCN − ] where, for example, [Fe3+ ] is the molar
concentration (mol Fe3+ / L solution) present in an equilibrium
mixture. At some temperature, a chemist found the following
equilibrium concentrations. [Fe3+ ] = 8.17 ✕ 10−3 M, [SCN − ] =
8.60 ✕ 10−3 M,...
At a certain temperature, K = 8.60 x 10^-4. for the reaction FeSCN2+(aq) ⇄ Fe3+(aq) +...
At a certain temperature, K = 8.60 x 10^-4. for the reaction FeSCN2+(aq) ⇄ Fe3+(aq) + SCN-(aq) Calculate the concentrations of Fe3+, SCN-, and FeSCN2+ in a solution that is initially 2.0 M FeSCN2+.
Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL...
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)...
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...
Fe3(aq) FESCN (aq) SCN (aq) In this experiment, we'll be examining the temperature-dependence of the rate constant...
Fe3(aq) FESCN (aq) SCN (aq) In this experiment, we'll be examining the temperature-dependence of the rate constant for the reaction above. 1. Using the UV-Vis instrument, you measured a room temperature absorbance for FESCN2 at 477 nm of 0.815. What is its concentration in molarity (M)? Please show all work. The molar absorptivity for FeSCN2 is 4,258 м"сm1 a. Answer: b. You calculated the [FeSCN2] above from the observed room temperature absorbance. Which one of the following statements about the...
At a certain temperature, Keq = 150 for the reaction being studied in today’s lab. Use...
At a certain temperature, Keq = 150 for the reaction being studied in today’s lab. Use Equation (3) to calculate the concentrations of Fe3+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 10-5 M. Assume the equilibrium concentrations of Fe3+ and SCN are equal.
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution KSCN (mL) Fe(NO3)3 (mL) 0.5 5 [FeSCN2+] (mol/L)* 1 4.0x10^-5 Add 1.0 M 2 1.0 5 8.0x10^-5 HNO3 3 1.5 5 1.2x10^-10 4 2.0 5 1.6x10-4 to each to adjust the volume to 25 mL. 5 2.5 5 2.0x10-4 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2+] (in Soln 1) = [SCN-]...
The reaction of cobalt(II) nitrate and potassium thiocyanate produces a coloured complex, [Co(SCN)4]2-(aq). The initial concentrations...
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...
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...
Equilibria can be treated mathematically with the equilibrium
constant, K. For the reaction Fe3+ + SCN − equilibrium reaction
arrow FeSCN2+, the equilibrium constant expression is [FeSCN2+ ] K
= [Fe3+ ] · [SCN − ] where, for example, [Fe3+ ] is the molar
concentration (mol Fe3+ / L solution) present in an equilibrium
mixture. At some temperature, a chemist found the following
equilibrium concentrations. [Fe3+ ] = 8.17 ✕ 10−3 M, [SCN − ] =
8.60 ✕ 10−3 M,...
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...
Fe3(aq) FESCN (aq) SCN (aq) In this experiment, we'll be examining the temperature-dependence of the rate constant for the reaction above. 1. Using the UV-Vis instrument, you measured a room temperature absorbance for FESCN2 at 477 nm of 0.815. What is its concentration in molarity (M)? Please show all work. The molar absorptivity for FeSCN2 is 4,258 м"сm1 a. Answer: b. You calculated the [FeSCN2] above from the observed room temperature absorbance. Which one of the following statements about the...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution KSCN (mL) Fe(NO3)3 (mL) 0.5 5 [FeSCN2+] (mol/L)* 1 4.0x10^-5 Add 1.0 M 2 1.0 5 8.0x10^-5 HNO3 3 1.5 5 1.2x10^-10 4 2.0 5 1.6x10-4 to each to adjust the volume to 25 mL. 5 2.5 5 2.0x10-4 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2+] (in Soln 1) = [SCN-]...
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...
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