20. The reaction [Co(H,O)"(aq) + 4Cr(aq) = pink (COCLJ*(aq) + 6H,0(1) blue is exothermic in the forward direction. Which of the following changes to an equilibriun mixture will produce a predominantly pink solution? I Cooling the solution 2 The uddition of concentrated HCI 3 The addition of aqueous silver nitrate A D

20. The reaction [Co(H,O)"(aq) + 4Cr(aq) = pink (COCLJ*(aq) + 6H,0(1) blue is exothermic in the forward direction. Which of the following changes to an equilibriun mixture will produce a predominantly pink solution? I Cooling the solution 2 The uddition of concentrated HCI 3 The addition of aqueous silver nitrate A D

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 20QAP

See similar textbooks

Similar questions

The equilibrium constant for the reaction 2CrO42(aq)+2H+(aq)Cr2O72(aq)+H2O is 31014 . What must the pH be so that the concentrations of chromate and dichromate ion are both 0.10 M?
(a) If Qc > Kc, how must the reaction proceed to reachequilibrium? (b) At the start of a certain reaction, onlyreactants are present; no products have been formed.What is the value of Qc at this point in the reaction?
For the liquid-phase reaction A + 2B ⇄ C + 2D , it was found that when 2 mol A, 4 mol B and 2 mol C were mixed in 1 L of water and allowed to come to equilibrium at 25 0C, the resulting mixture contained 2 mol of D. Calculate equilibrium constant, K, for this reaction.
The reaction quotient, Q, is 9.00 × 10⁻¹² The Ksp of zinc fluoride is 3.04 x10⁻² at 25°C. Comparing this value to the Q obtained in the previous step, predict if the zinc fluoride will precipitate.
In the formation of soluble silver-ammonium complex, in an AgCl solution that occured in a 3-step process: If log K2 is 4.21 and log K1 is 4.21, what is Kf? As a chemist, you already know that Kf for Ag(NH3)2+ is equal to K1 multiplied to K2.
The equilibium constants of the reactions FeO(s) + CO(g) = Fe(s) + CO2(g) ; K1 FeO (s) + H2(g) = Fe(s) + H2O (g) ; K2 Temp (oC) 600 700 800 900 1000 ------------------------------------------- K1 0.900 0.673 0.535 0.453 0.396 K2 0.332 0.422 0.499 0.594 0.668 Calculate the Equilibium constant of the reaction CO (g) + H2O (g) = CO2(g) + H2(g) at the above temperature Also calculate the heat of the reaction for the production of hydrogen from carbon monoxide and water vapour, assuming it to be independent of temperature
The equilibrium constant Kc for C + CO2 <=> 2CO is 1.9 at 1000 K and 0.133 at 298K. Is the reaction endothermic or exothermic?
1. You determined the equilbrium constant, K eq^ prime for the reaction using a number of different [Fe^ 3+ ] 0; [SCN] 0 ratios . Does K eq depend on the relative intial concentraion of the reactants? Is this what you would expect? Explain your answer.
The equilibrium constant at 25 °C for the dissolution of silver iodide is 8.5 × 10–17. AgI (s) D Ag+ (aq) + I– (aq) If an excess quantity of AgI(s) is added to water and allowed to equilibrate, what is the equilibrium concentration of I–?
At 276.7 oC, the Kp for the reaction 2 A (g) + 1 B (g) ↔ 5 AB is Kp = 3.07⋅10-2 What is Keq?
The equilibrium constant for the reaction Na2(g) → 2Na(g) is 2.47 at 1000. K. Calculate the value of ∆G∘ for this reaction under these conditions.
Write down the thermodynamic equilibrium constant expressions of the following reactions. If possible, associate them with Kc and Kp.(a) Si (k) + 2 Cl₂ (g) ↔ SiCl ₄ (g)(b) Cl₂ (g) + H₂O (s) ↔ HOCl (aq) + H⁺ (aq) + Cl- (aq)