The reaction below reaches equilibrium in a closed reaction vessel. 4 HCl(aq) + MnO2 (s) = Cl₂(g) + 2 H₂O(l) + Mn2+ (aq) + 2 CI (aq) + energy Which of the following actions increases the concentration of Cl(aq) in the equilibrium mixture? decreasing volume decreasing temperature neutralizing HCl(aq) adding Mn(NO3)2 (aq) adding Cl₂(g)

The reaction below reaches equilibrium in a closed reaction vessel. 4 HCl(aq) + MnO2 (s) = Cl₂(g) + 2 H₂O(l) + Mn2+ (aq) + 2 CI (aq) + energy Which of the following actions increases the concentration of Cl(aq) in the equilibrium mixture? decreasing volume decreasing temperature neutralizing HCl(aq) adding Mn(NO3)2 (aq) adding Cl₂(g)

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

Which of the following, when added to an equilibrium mixture represented by the equilibrium below, will not alter the composition of the original equilibrium mixture? MgOH2 (s) ↔ Mg2+ (aq) + 2OH- (aq) Addition of HCl (aq) to the equilibrium mixture Addition of Fe(NO3)3 (aq) to the equilibrium mixture Addition of NaOH (s) to the equilibrium mixture Addition of Mg(NO3)2 (s) to the equilibrium mixture Addition of Mg(OH)2 (s) to the equilibrium mixture
Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 25.0 L tank with 5.3 mol of ammonia gas and 2.4 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.4 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = -0 ☐ x10 G
Consider this reaction at equilibrium. B(g) +2C(aq) 2D(g) The rates of the forward and reverse reactions are equal at equilibrium. There are 4 processes listed below that are applied individually to put a stress on the equilibrium. For each process, determine how that stress affects the rates of the forward and reverse reactions. Then drag the purple number that identifies the process to the gray arrow that will have the faster rate after that stress is applied There can be more than 1 number in each gray box. 1 Some B is added 3 Some D is added 2 Some C is removed 4 The volume of the gases is reduced. B(g) + 2C(aq) 2D(g)
Consider the following equilibrium reaction: N2(g) + 6 HCl(g) 2 NH3(g) + 3Cl2(g) The equilibrium constant expression for the above reaction is: 3 [NH3)² [Cl₂1³ [Nz][HC?]® [NH3][Cl₂] |HCl][Ng] [HC] [NH3)² [Nz][HCỤ* [NH3)² [Cl₂]³ [NH3)²+[Cl₂]³ [N2]+[HC®
Solid Ca₃(PO₄)₂ is placed into 10.0 L of water. When equilibrium is established, the concentration of Ca²⁺ is 2.3 × 10⁻⁴ M. What is Kc for this equilibrium? Ca₃(PO₄)₂ (s) ⇌ 3 Ca²⁺ (aq) + 2 PO₄³⁻ (aq) (i already asked this question but was given the wrong answer 2.74 x 10^-19)
Consider the decomposition of nitrosyl bromide into nitrogen monoxide and bromide gas, which has an equilibrium constant Kc = 6.2 x 10-5 when the reaction occurs at a certain temperature. If the initial concentration of nitrosyl bromide is 0.832 M, what will be the equilibrium concentration of nitrogen monoxide gas? 2 BrNO (g) <---> 2 NO (g) + Br2 (g)
Using the equilibrium constants given for reactions (1) and (2), what is the equilibrium constant for reaction (3)? 1) 2NO(g) + O2(g) → N2O4(g) Kp = 1.49 × 1013 2) 2NO(g) + O2(g) → 2NO2(g) Kp = 1.66 × 1012 3) N2O4(g) → 2NO2(g) 80.3 0.111 None of the following 8.98 0.0123
Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2) CO(g) + Cl2(g) ⟷ COCl2(g)If the equilibrium constant for this reaction is Kc = 248, predict what will happen when [CO] = [Cl2] = [COCl2] = 0.0200 M. Group of answers The reaction will proceed in the forward direction to reach equilibrium. The reaction is at equilibrium already before every substance is at the same concentration. Because K > 1, the reaction will proceed in the forward direction to reach equilibrium. The reaction will proceed in the reverse direction to reach equilibrium. The temperature needs to be specified before a prediction can be made.
4
Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O,(g)→2 HgO(s) At a certain temperature, a chemist finds that a 5.5 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 20.1 g O2 16.1 g HgO 6.8 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = | x10
Consider the following diagrams which show the progress for the reaction A (blue) = B (red). The equilibrium constant (K) for this reaction is 0.8. At which point does the reaction reach equilibrium? BERE
The equilibrium constant, Ke, for the reaction of iodine bromide to form iodine and bromine is 2.5 x 10 If an equilibrium mixture contains 0.30 M IBr and 3.8 x 10-2 M I2, what is the molar concentration of Br2? PIBI(g) =I2(8) + Br2(g)