The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Fe (aq) + SCN (aq) = Fe(SCN)²* (aq) increasing the concentration of Fe“ decreasing the concentration of Fe(SCN)²+ increasing the temperature of the system

The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Fe (aq) + SCN (aq) = Fe(SCN)²* (aq) increasing the concentration of Fe“ decreasing the concentration of Fe(SCN)²+ increasing the temperature of the system

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The reaction below reaches equilibrium in a closed reaction vessel. 4 HCl(aq) + MnO2 (s) = Cl₂(g) + 2 H₂O(l) + Mn2+ (aq) + 2 CI (aq) + energy Which of the following actions increases the concentration of Cl(aq) in the equilibrium mixture? decreasing volume decreasing temperature neutralizing HCl(aq) adding Mn(NO3)2 (aq) adding Cl₂(g)
A student ran the following reaction in the laboratory at 545 K: COC12 (g) CO(g) + Cl₂ (g) When she introduced 0.604 moles of COC12 (g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂ (g) to be 0.0302 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
3. Calculate the equilibrium concentrations of the gaseous products if a sample of solid NH,SH is placed in a closed vessel at 218 °C and decomposes until equilibrium is reached. NH,SH(s) S NH3(g) + H,S(g) K. = 1.2 ×10 4
the equilibrium constant (K) is a quantitative measurement of theextent to which a chemical or physical reaction proceeds to completion. If two reactants ofknown initial concentration are mixed and then the concentrations of the products aremeasured once equilibrium has been established, then the equilibrium constant can becalculated using an ICE table.In this experiment you will measure the equilibrium constant for the formation of iron(III)thiocyanate from the iron(III) cation and thiocyanate anion:Fe3+(aq) + SCN-(aq) FeSCN2+(aq)The product, FeSCN2+, is intensely red, which means that its concentration can be measured byusing an ultraviolet-visible (UV-vis) spectrophotometer. So long as a solution is not tooconcentrated, the absorption of light at a particular wavelength by a chemical species isdescribed by Beer’s Law:A = εℓ[X] where A = absorption of light (unitless number)ε = molar absorptivity constant (cm-1 M-1)ℓ = path length (cm)[X] = concentration (M)The path length for our…
Say that you mix Fe3+ and SCN- together so that after mixing, the concentration of Fe3+ (aq) equals 0.0015 M , and the concentration of SCN- (aq) equals 5.5 x 10-4 M. You measure the concentration of product, FeSCN2+, after equilibrium forms. It is 7.2 x 10-5 M. Calculate the value of the equilibrium constant, K, for the reaction. F e 3 + ( a q ) + S C N − ( a q ) ⟷ F e S C N 2 + ( a q ) K = ? Group of answer choices 0.011 9.52 x 10-3 87.3 105
the equilibrium expressions for the following reactions: 2Fe(s) + 3H2O(g) ↔ Fe2O3(s) + 3 H2(g) A [Fe2O3][H2] = Keq [Fe][H2O] B [Fe2O3][H2]3 = Keq [Fe]2 [H2O]3 C [H2]3 = Keq [H2O]3 D [Fe]2 [H2O]3 = Keq [Fe2O3][H2]3
the equilibrium constant (K) is a quantitative measurement of theextent to which a chemical or physical reaction proceeds to completion. If two reactants ofknown initial concentration are mixed and then the concentrations of the products aremeasured once equilibrium has been established, then the equilibrium constant can becalculated using an ICE table.In this experiment you will measure the equilibrium constant for the formation of iron(III)thiocyanate from the iron(III) cation and thiocyanate anion:Fe3+(aq) + SCN-(aq) FeSCN2+(aq)The product, FeSCN2+, is intensely red, which means that its concentration can be measured byusing an ultraviolet-visible (UV-vis) spectrophotometer. So long as a solution is not tooconcentrated, the absorption of light at a particular wavelength by a chemical species isdescribed by Beer’s Law:A = εℓ[X] where A = absorption of light (unitless number)ε = molar absorptivity constant (cm-1 M-1)ℓ = path length (cm)[X] = concentration (M)The path length for our…
The following reaction is at equilibrium and being monitored by a chemist : 2NOF (9) 2NO (g) + F₂ (g) The Chemist measures these concentrations at equilibrium: [NOF] = 0.56M [NO] = 0.32 M [F₂] = 0.28 M What is the equilibrium constant for this reaction?
Given these initial concentrations: [SCN-] = 0.000644 M, [Fe3+] = 0.000505 M, and [Fe(SCN)2+] = 0.000 M, determine the value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M.
At 503 K the equilibrium constant K. for the dissociation of N,O4, N204(g) 2 2 NO2(g) has the value K = = 40.0. Calculate the concentration of N204 left undissociated when 1.00 mol of this gas is heated to 503 K in a 10.0 L container.
Calculate the equillibrium constant using the balanced chemical equation and the concentration of he substances at equilibrium. Based on the calculated value of K which is favored for the reaction products (fwd) or reactants (rev)? 2NO2 (g)= N2O4 (g) [NO2]=.0760 M [N2O4]=1.26 M