Consider the following equilibrium: Fe(OH)3 (s) + 3H* (ag) Fe3* (ag) + 3H₂O (1) a) Given a Kap of 9.1 x 103, what is the concentration of Fe³+ at pH 3? b) If we now consider the following equilibrium: Fe³+ + e Fe2+ (pE0= 13.2) At a RE of 17.3, what will the relative concentration of Fe2+ to Fe³+ be? (i.e., calculate the ratio [Fe2+]/[Fe³+])

Consider the following equilibrium: Fe(OH)3 (s) + 3H* (ag) Fe3* (ag) + 3H₂O (1) a) Given a Kap of 9.1 x 103, what is the concentration of Fe³+ at pH 3? b) If we now consider the following equilibrium: Fe³+ + e Fe2+ (pE0= 13.2) At a RE of 17.3, what will the relative concentration of Fe2+ to Fe³+ be? (i.e., calculate the ratio [Fe2+]/[Fe³+])

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

A student ran the following reaction in the laboratory at 288 K: 2CH₂Cl₂(9) CH4(9) + CCl4(9) When she introduced 7.50x 10-2 moles of CH₂Cl₂(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(9) to be 3.48x10-² M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
Hydrogen gas and iodine gas react via the following equation. H2 (g) + I2 (9) = 2 HI(g) K. = 79 (at 650 K) If 0.042 mol HI is placed in an empty 1.0 L flask at 650 K, what are the equilibrium concentrations of HI, I2, and H2? [H2]eq [12]eq = HI ea M M M
Consider the following equilibrium: Cu2+(aq)+ 4NH3(aq) ⇌ Cu(NH3)42+(aq); Kf= 1.7 x 1013; Determine [Cu2+], [Cu(NH3)42+], [NH3],and [SO42–], respectively, in solution that results from mixing 20.0-mL solution of 0.10 MCuSO4and a 30.0-mL solution of 3.0 M NH3 are mixed.
5) Determine the value of Ke for the following reaction if the equilibrium concentrations are as follows: [N2]eq =1.5 M, [H2]eq = 1.1 M, [NH3]eq = 0.47 M. N2(g) + 3 H2(g) = 2 NH3(g)
A student ran the following reaction in the laboratory at 1083 K: 2503(g) 2sO2(g) + 02(g) When she introduced 7.36x10-2 moles of SO3(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 4.23x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc II
At 25 °C, K. = 1.6 x 10-34 for the reaction %3D 2HCI(g) + I2(s) 2HI(g) + Cl2(g) Suppose 0.100 mol of HCI and solid I, are placed in a 1.00 L container. What will be the equilibrium concentrations of HI and Cl, in the container?
ul Constant for the reaction. 2. Consider the reaction: A+B=C+3D A solution was prepared by mixing 50.00 mL of 1.00 x 10 M A, 100 mL of 2.00 x 10 MB, 10.0 mL of 1.0 M C and 75 mL of 1.50 x 10³M D. At equilibrium, the concentration of D was measured to be 6.0 x 10 M. a) Calculate the equilibrium concentrations of each species b) Calculate the equilibrium constant. 3. Consider the reaction: 2NO2(g) + Cl₂)* 2NOCI The initial pressure of NO, was 1.577 atm and the initial pressure of Cl₂ was 0.427 atm. At equilibrium, the partial pressure of NOCI is 0.624 atm. Calculate K.
A student records the following equilibrium concentrations for the iron(III) thiocyanate equilibrium. [Fe(SCN)2+] = 0.00023 M [Fe³+] = 0.0037 M [SCN-] = 0.0038 M What is the value of Ke for this equilibrium? Enter your answer in scientific notation like this 10,000 = 1*10^4.
C2,H2905S- (ag) + NH,CI (ag) → C2,H29O5SH (ag) + NH3 (aq) Yellow Blue Reaction after it reaches equilibrium appears Green A. Assume the reaction mixture is at equilibrium, appearing green in color, and at room temperature before each of the following disturbances. Explain which direction the reaction shifts to re-establish equilibrium and predict how the color of the solution will change 1.100 mL of water, H2O is added to the reaction mixture. 2. Solid platinum, Pt, is added to the reaction mixture. It reacts with NH3 to form N and H2 gasses. B. When the green reaction mixture at equilibrium is heated the color changes to green-blue, and then eventually, a dark blue color. When the green reaction mixture at equilibrium is placed in an ice water bath the solution color changes to a yellow-green, and eventually a bright yellow color. Is the reaction exothermic or endothermic? |
Interconvert K and K values. Calculate Ko for the following reactions at the indicated temperature. (a) 2 NOCI(g) 2 NO(g) + Cl₂(g) K = 2.69x10-³ at 560 K Kp = (b) NHAl(s)NH₂(g) + HI(g) Kc = 5.59×10-4 at 634 K Kp =
A student ran the following reaction in the laboratory at 642 K: 2HI=H2+I2 When she introduced 0.368 moles of HI into a 1.00 liter container, she found the equilibrium concentration of I2 to be .0363 M Calculate the equilibrium constant, KC, she obtained for this reaction.
15.43 At 100°C, the equilibrium constant for the reaction COCI2(8) CO(g) + Cl2(g) has the value K= 2.19 x 10 10, Are the following mixtures of COCI2, CO, and Cl2 at 100 °C at equilibrium? If not, indicate the direc- tion that the reaction must proceed to achieve equilibrium. (a) [COCI2]= 2.00 x 103 M, [CO] = 3.3 x 10M, [Cl2] 6.62 x 106 M (b) [COCI2] = 4.50 x 102 M, [CO] = 1.1 x 107 M, [Cl2] 2.25 x 106 M (c) [COCI2] 0.0100 M, [CO] [Cl2] = 1.48 x 10-6 M