(21) Consider the equilibria below and choose the statement that is NOT true. C₂04² (aq) + H3O+ H₂O(1) + HC₂O4 (aq) Fe³(aq) + C₂04² (aq) [Fe(C₂O4)3] (aq) (A)) Kb = 6.7 x 10-11 K = 2 x 10²0 The second equilibrium will be shifted left by the addition of acid The first equilibrium will be shifted left by the addition of (B) Fe³(aq) (0) Neither equilibrium will be affected if the solutions are buffered to a pH = 7.00 (D) The second equilibrium heavily favors the products (E) The first equilibrium heavily favors the reactants

(21) Consider the equilibria below and choose the statement that is NOT true. C₂04² (aq) + H3O+ H₂O(1) + HC₂O4 (aq) Fe³(aq) + C₂04² (aq) [Fe(C₂O4)3] (aq) (A)) Kb = 6.7 x 10-11 K = 2 x 10²0 The second equilibrium will be shifted left by the addition of acid The first equilibrium will be shifted left by the addition of (B) Fe³(aq) (0) Neither equilibrium will be affected if the solutions are buffered to a pH = 7.00 (D) The second equilibrium heavily favors the products (E) The first equilibrium heavily favors the reactants

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

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 =
15.0 g of glucose reacts with oxygen in a 15.0 L container. At 250°C the system reaches equilibrium. At equilibrium it is determined that there are 5.25 mol of oxygen, 1.84 mol of carbon dioxide and 5.66 mol of steam. Calculate the value of the the equilibrium constant Kc. C6H12O6(s) + 602(g) = 6 CO2(g) + 6H2O(g) O9.64 x 10-5 O5.35 x 10 6 9- O1.87 x 105 O 0.0164 60.9
For the reaction 2A(g) <===> B(g)+2C(g), a reaction vessel initially contains only A at a pressure of PA=895torr . At equilibrium, PA=65torr. First convert torr to atm by dividing by 760, and next use an ICE table to help calculate the value of Kp. (Assume no changes in volume or temperature.) Express your answer using two significant figures.
Chlorine and bromine gases will react with one another according to the following equation Cl₂(g) + Br₂(g) = 2ClBr(g); Kp = 2.25 If the initial pressure at 298 K of the gases are Cl₂ (9) 1.00 atm, Br₂ (g) 1.00 atm and ClBr(g) 1.50 atm, what will happen as the reaction system moves towards equilibrium? Additional Cl₂ (g) will be formed. O cannot be determined from the given data O additional Cl₂ (g) and Br₂ (g) will be formed O additional ClBr(g) will be formed Onothing, the system is at equilibrium 10-2min- inization the con
Consider the following reactions and their respective equilibrium constants: NO(g) + Br2 (9) =NOB|(9); K = 5.3 2NO(g) = N2(9)+O2 (g); K = 2.1 x 1030 Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: N2(9) + O2 (g) +Br2 (g) 2NOB1(g) Express your answer using two significant figures. | ? K =
The equilibrium constant for the following reaction is 67.6 at 232 °C. PCI 3(g) + Cl₂(g) PCI5(g) K = 67.6 at 232 °C Calculate the equilibrium constant for the following reactions at 232 °C. (a) PCI5(g) PCl3(g) + Cl₂(g) K= (b) 2 PCI5(g) 2 PCI3(g) + 2 Cl₂(g) K=
Consider the following reactions: CO (g) + 2 H2S (g) D CS2 (g) + H2O (g) + H2 (g) K1 = 1.3 x 105 ½ CH4 (g) + H2S (g) D ½ CS2 (g) + 2 H2 (g) K2 = 180 1. Find the equilibrium constant for: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) 2. What molecules in the steps are reaction intermediates? 3. If 0.500 atm of CO, H2, CH4, and H2O are initially placed in the same container, then given your answer in part a., determine which direction the reaction will shift in order to establish equilibrium.
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…
Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) K = 4.3 x 10-25 2NO(g) + O2(g) == 2NO,(g) K= 6.4 × 10' Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 202(g) = 2NO2(g) K. - x 10 (Enter your answer in scientific notation.)
The equilibrium constant, Kċ, for the following reaction is 1.29×10-² at 600 K. Calculate Kp for this reaction at this temperature. COCI₂(g) ⇒CO(g) + Cl₂(9) Кр || =
Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N₂(g) + O₂(g) 2NO(g) Ke=4.3 × 10-25 2NO(g) + O₂(g) = 2NO₂(g) K=6.4 × 10⁹ Determine the value of the equilibrium constant for the following equation at the same temperature: N₂(g) +20₂(g) = 2NO₂(g) Ke= 10 (Enter your answer in scientific notation.)
Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those obtained when gasoline burns in an automobile engine. At 2000°C, K for the reaction N2(g) + O2(g) ⇆ 2NO(g) is 0.010. If 0.40 moles of N2, 0.10 moles of O2, and 0.080 moles of NO are placed in a 1.0-liter container, what will be the concentration of O2 at equilibrium?