The following reactions all have K < 1. 1) CgHyOs" (aq) + HCOOH (aq) =HCgHy©s (aq) + HCOO" (aq) 2) HCOO° (aq) + HCN (aq) = 3) HCN (aq) + C₂H₂O4 (aq) HCOOH (aq) + CN* (aq) CN (aq) + HC₂H₂O4 (aq) Arrange the substances based on their relative acid strength. CN HCgHyOs HCOOH HCOO CgH704 HCN Clear All strongest acid intermediate acid weakest acid not a Bronsted-Lowry acid

The following reactions all have K < 1. 1) CgHyOs" (aq) + HCOOH (aq) =HCgHy©s (aq) + HCOO" (aq) 2) HCOO° (aq) + HCN (aq) = 3) HCN (aq) + C₂H₂O4 (aq) HCOOH (aq) + CN* (aq) CN (aq) + HC₂H₂O4 (aq) Arrange the substances based on their relative acid strength. CN HCgHyOs HCOOH HCOO CgH704 HCN Clear All strongest acid intermediate acid weakest acid not a Bronsted-Lowry acid

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

At a particular temperature, Kc=6.5x10^-2 for
18. Given these equilibrium expressions for the dissolution of CO2 gas in water: CO2(aq)+H2O(1) H2CO3(aq) H2CO3(aq)+ H2O(1)HCO3(aq) + H3O*(aq)
1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) ΔΗ, 298
The following reactions all have K > 1. 1) HNO2 (aq) + CIO¯ (aq)= NO2 (aq) + HCIO (aq) 2) CH,COОH (аq) + CIO (aq) HCIO (aq) + CóH;C00" (aq) 3) HNO2 (aq) + C6H5C00 (aq)= NO; (aq) + CgH;CООН (aq) Arrange the substances based on their relative acid strength. Clear All C,H;COOH C,H;C00 strongest acid NO2 intermediate acid CIO weakest acid HNO2 not a Bronsted-Lowry acid HCIO
Balance each of the following examples of heterogeneousequilibria and write its reaction quotient, Q꜀:
Given that Ka for HIO is 3.2 × 10-1" at 25 °C, what is the value of K, for IO¯ at 25 °C? Kp = Given that Kp for CH, NH, is 5.0 x 10-4 at 25 °C, what is the value of Ka for CH, NH; at 25 °C? Ka =
> Given the two reactions HS (aq) +H (aq), K₁=9.70x108, and 1 1. H₂S(aq) 2. HS (aq) S² (aq) +H(aq), K₂=1.55x10-19, what is the equilibrium constant Kfinal for the following reaction? Enter your answer numerically. ▸View Available Hint(s) 1D ΑΣΦΑ Kfinal 1.078 1026 Submit ● Part R Previous Answers S² (aq) + 2H* (aq) = H₂S(aq) X Incorrect; Try Again; 9 attempts remaining ?
Consider the following reactions, where the equilibrium constants are represented by the variables x and y: 2 FeCl3(aq) + Zn(s) ⇄⇄ 2 FeCl2(aq) + ZnCl2(aq) K=x FeCl3(aq) + CrCl2(aq) ⇄⇄ FeCl2(aq) + CrCl3(aq) K=y Write an expression for the equilibrium constant for the reaction below, in terms of x and y. 2 CrCl3(aq) + Zn(s) ⇄⇄ 2 CrCl2(aq) + ZnCl2(aq) (Answer should be = x/y2)
O Ni(H₂O)2+ (aq) + 3SCN- (aq) = Ni(SCN); (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.
Use the data in the supporting materials to calculate the equilibrium constant (Kp) for the following reaction at 25°C. 2 SO2(g) + O2(g) =2 S03(g) Кра 4.24e24 Calculate Kp for the reaction at 49°C using the following equations. (a) the van't Hoff equation below. (P), A,H° RT? a In K Кр = 1.138e22 (b) the Gibbs-Helmholtz equations below to find A-G° at 49°C and hence, Kp at the same temperature. AG ΔΗ (i) = - T2 A-G2 A;G1 1 (ii) T2 T1 T1 Kp = 1.138e22 (c) A-G° = ArH° – TA¡S° to find A-G° at 49°C and hence, Kp at the same temperature. Кр 3D 1.7742е22 State the approximations employed in each case. The assumption that A,H° is temperature independent and equal to the value calculated at 298.15 K is required by all three parts A second assumption that AS° is temperature independent and equal to the value calculated at 298.15 K is required by part (c) Compare your results. The answers calculated in parts (a) and (b) ▼ in part (c) are very close as expected because the formulas used to…
help use sig figs
12.48 The following reaction is in equilibrium in lake water: HCO3(aq) + H+ (aq) = H₂CO3(aq) Predict the change in the reaction quotient, Q, for each disturbance below and use that prediction to explain how the equilibrium is shifted by the stress. (a) NaHCO3 is added to the lake. (b) H₂CO3 is added. (c) NaOH is added.