While creating the E3 reaction mixture, a student obtains the following data. Calculate the initial thiocyanate ion concentration, [SCN=]o, in the reaction mixture in millimolar (mM. Give your answer to three decimal places. Fe(NO3)3 NASCN 0.10 MHNO3 2.042 x 103 M 1.98 × 10-3 M -- initial buret reading (mL) final buret reading (mL) 0.02 0.03 0.05 5.09 2.33 2.93 Your Answer: Answer

While creating the E3 reaction mixture, a student obtains the following data. Calculate the initial thiocyanate ion concentration, [SCN=]o, in the reaction mixture in millimolar (mM. Give your answer to three decimal places. Fe(NO3)3 NASCN 0.10 MHNO3 2.042 x 103 M 1.98 × 10-3 M -- initial buret reading (mL) final buret reading (mL) 0.02 0.03 0.05 5.09 2.33 2.93 Your Answer: Answer

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter7: Reaction Rates And Chemical Equilibrium

Section: Chapter Questions

Problem 7.56P

See similar textbooks

Similar questions

7. How did the reaction below happen? Use catalytic circle to describe the mechanism, assuming the catalyst is the complex [CpRu(CH;CN);[BAr] Catalyst CO2ME + MeO OMe ċO,Me N2 CH2CI2 (0.5 M) 60 °C, 6 h 1a 2A 3aA
After completing part II of the experiment, a student uses her calibration curve to find that the equilibrium concentration of the product in one trial is 1.14x10-4 M. If the "initial" concentrations of Fe3+ and SCN in the reaction mixture are those given below, what is the equilibrium concentration of Fe³+, [Fe³+]eq? Give your answer in millimolar (mM) to three decimal places. [SCN-]0= 6.14x10-4 M [Fe3+] = 1.00x10-³ M [FeNCS2+]eq = 1.14x10-4 M
Determine the equilibrium concentration of [FeSCN]2+ in each test tube y = 6170.7x - 0.0153 Solution 0.002M iron(III) nitrate in 1M nitric acid(mL) 0.002M potassium thiocyanate(mL) DI water(mL) Absorbance(A) 1 3 2 1 0.128 2 2 3 1 0.269
After completing part II of the experiment, a student uses her calibration curve to find that the equilibrium concentration of the product in one trial is 1.19x10-4 M. If the "initial" concentrations of Fest and SCN in the reaction mixture are those given below, what is the equilibrium concentration of Fe3+, [Fe3+]eg? Give your answer in leq millimolar (m M to three decimal places. [SCN¯]0= 6.18x10-4 M [Fe3+]o = 1.12x10-3 M [FENCS2*]eg = 1.19x10-4 M
8 Reactions between certain organic (alkyl) halides and water produce alcohols. Consider the overall reaction for t-butyl bromide (2-bromo-2-methylpropane). (CH3)3CBr(aq) + H2O(1) →(CH3)3COH(aq) + H*(aq) + Br "(ag) k[(CH3)3CB1]. The accepted mechanism for the The experimental rate law is rate = %3D reaction is shown below. (1) (CH3)3C-Br(aq) →(CH3)3C*(aq) + Br "(aq) [slow] (2) (CH3)3C*(aq) + H2O(1) →(CH3)3C-OH2*(aq) [fast] (3) (CH3)3C-OH2*(aq) →H*(aq) + (CH3)3C-OH(aq) [fast] a) Why doesn't H2O appear in the rate law? b) Write rate laws for the elementary steps. c) What intermediates appear in the mechanism? d) Show that the mechanism is consistent with the experimental rate law. ed to the of consumption of N
○ Ni(H₂O)²+(aq) + 3SCN- (aq) = Ni(SCN)3(aq) + 6H₂0(1) (a) Write the Kc expression for this equilibrium. (b) Would there be a shift to the right or to the left if KSCN solution was added to a solution containing this equilibrium? Explain your answer.
Predict the K vs T plot that best reflects this reaction. CH₂CH₂Br(aq) + Cl(aq) → CH₂CH₂Cl(g) + Br(aq) OKA T K Ок T L E OKA T T
ki ki = 2x 102s B, rate constant of forward reaction k-1 9. For the reversible reaction A and for back reaction k.j = 1x 103 s1.What is equilibrium constant for this reaction?
Consider chemical reaction:- X +2Y+ az )XY2Z2 It is faund that mng the [X] quadaup the [2] oubles the hate -) doubling the Cx7 has no effect on the sate doulbl les the late dneponb Cx] (- what is -the fate seaction 9 2 Pse dict the reactants for the Tate determ inA step. what is the molecularlty of the rate-deter step. minir 2) Predict a Complete mechanism Ahat meets the aiteria por this reaction Indicate which is neccessory the slow step the intermediates •J need these answer within 30 min. Thank Xou, Pleaze Consider g reguest my
for the reaction 4PH ₂3 (9) 6 H₂₂ (9) + P4 (9) the equilibrium concentrations were found to be [PH3] = 0.250M, [#₂] = 0.370 M, and [P4]=0.750 M. what is the equilibrium constant for this reaction?
Identify the equilibrium constant expression for the following reaction: Brz(g) + 2 HI(g) =Lg)+2 HBr(g) [Br-][H? [Br2][HI] Keg Keg [L]HBrj? %3D L][HBr] [L][2HB1] O Keq [L2][HBr] Keg %3D %3D [Brz][2HI] [Br2][HI] L]HBr Keq [Br][HI]? DELL
After completing part II of the experiment, a student uses her calibration curve to find that the equilibrium concentration of the product in one trial is 1.19x10 M. If the "initial" concentrations of Fes+ and SCN in the reaction mixture are those given below, what is the equilibrium concentration of Fe*, [Fe*]ea? Give your answer in millimolar (mM) to three decimal places. 3+ 3+1 [SCN ]o= 6.18x10-4 M [Fe3+]o = 1.11x10-3 M %3D [FENCS2+]eg = 1.19x10-4 M