(b) Given the following initial concentrations, what are the equilibrium concentrations of Fe³+, HSCN, and FeSCN²* and the value of K for the equilibrium? Trial 1 2 3 4 5 Initial Concentrations Fe³+ HSCN (M) (M) 0.001 0.0002 0.001 0.0004 0.001 0.0006 0.001 0.0008 0.001 0.0010 Fe³ (M) Equilibrium Concentrations HSCN (M) FeSCN²+ (M) H* (M) 0.5 0.5 0.5 0.5 0.5 Kea

(b) Given the following initial concentrations, what are the equilibrium concentrations of Fe³+, HSCN, and FeSCN²* and the value of K for the equilibrium? Trial 1 2 3 4 5 Initial Concentrations Fe³+ HSCN (M) (M) 0.001 0.0002 0.001 0.0004 0.001 0.0006 0.001 0.0008 0.001 0.0010 Fe³ (M) Equilibrium Concentrations HSCN (M) FeSCN²+ (M) H* (M) 0.5 0.5 0.5 0.5 0.5 Kea

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

1) Given the following reaction: X + 2Y = Z + W, if K is 4.2 x 10 -2, calculate the value for K for: X+ 2YZ+W a) Z+W X + 2Y b) 3X+6Y3Z+3W c) 2 Z+2 W = 2 X+4Y Manl
The reaction HSO3 (ag) + H* (aq) + SO3 (ag) has K = 0.01 at 300 K. An equilibrium mixture at 300 K contains 0.1 M HSO3 and 0.01 M H*. What is the concentration of SO3 in that equilibrium mixture? O None of the other answers are correct 0.01 M 10 М O 0.1 M O 1 M « Previous Next
Consider the reaction. A(aq) 2 B(aq) K.- 2.52 x 10-6 at 500 K If a 2.90 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] =
.Suppose that 0.50 moles of hydrogen gas, 0.50 mol of iodine gas, and 0.75 moles of hydrogen iodide gas are introduced into a 2.0 Liter vessel and the system is allowed to reach equilibrium. H2(g) + I2(g). 2 HI(g) Calculate the concentrations of all three substances at equilibrium. At the temperature of the experiment, Kc equals 2.0 x 10-3. Answer: [H2] = [I2] = 0.43 M [HI] = 0.020 M
Starting with initial concentrations of 0.040 mol/L of N2 and 0.040 mol/L of O2, calculate the equilibrium concentration of NO in mol/L N2(g) + O2(g) ⇄ 2NO(g) Kc = 0.10 at 2000oC
The initial concentrations of Na+ and C1 in the reaction below are each 0.0434 M. If the initial concentration of NaCl is 0 M and the equilibrium constant is Kc = 8.21 under certain conditions, what is the equilibrium concentration of Nat? NaCl(aq) = Na+ (aq) + Cl¯ (aq) Select the correct answer below: 0.0287 M 0.0354 M 0.0432 M -4 6.81 x 10 M
The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g) ---> 2NO(g) + Br2(g)If an equilibrium mixture of the three gases in a 14.7 L container at 298K contains 0.295 mol of NOBr(g) and 0.352 mol of NO, the equilibrium concentration of Br2 is _______M.
When determining the equilibrium concentrations for the reaction [A][B] AB(g) = A(g) + B(g) [AB] a simplifying assumption can be used under certain conditions to avoid solving a quadratic equation. x2 K. = [AB] - x [AB] Classify each situation by whether the simplifying assumption can be used or whether the quadratic formula is required. Simplifying assumption can be used Quadratic formula required Answer Bank [AB] = 0.2209 M, Ke = 4.5 × 10-6 [AB] = 0.0394 M, Ke = 8.12 × 10-5 [AB] = 0.00103 M, K. = 7.4 × 10¬8 [AB] = 0.0207 M, Ke = 2.88 × 10-6 [AB] = 0.243 M, Ke = 7.11 × 10¬4
When determining the equilibrium concentrations for the reaction AB(g) A(g) + B(g) [A][B] [AB] a simplifying assumption can be used under certain conditions to avoid solving a quadratic equation. Ke Kc = [AB]-x [AB] Classify each situation by whether the simplifying assumption can be used or whether the quadratic formula is required. Simplifying assumption can be used [AB] = 0.00178 M. Kc = 9.91 x 107 [AB]=0.0353 M, K, 3.67 x 10 Answer Bank [AB]=0.484 M, K, 8.18 x 10 Quadratic formula required [AB] 0.176 M. K=144 x 10¹ [AB]=0.0160 M, K - 7.46 x 10
What is the value of the equilibrium constant Ko for the following reaction at the temperature of the mixture? 2NO,(g) N,0,(g) 3rd attempt See Periodic Table O See Hint Analyses of an equilibrium mixture of N204(g) and NO2(g) gave the following results: [NO2(g)] = 4.210×10-3 M [N204(g)] = 2.706×10³ M 221.3
Iodine and bromine react to give iodine monobromide, IBr. I1 (9) + Brz (9) = 2IB:(9) What is the equilibrium composition of a mixture at 154°C that initially contained 1.10 x 10- mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant K, for this reaction at 154°C is 130. [1:] =( M [Bra] =( M [IBr] = M
Question 10 In an experiment where the initial concentration of Fe3+ was 0.00133 M and the initial concentration of SCN* was 0.000468 M, a student measured the final equilibrium concentration of FENCS2* to be 0.000177 M. Fe3*(aq) + SCN'(aq) FENCS2*(aq) Calculate the final equilibrium concentration of SCN'. Your Answer: Answer