Consider the reaction: NOC) = NO) + Cl2 (@) a.) At equilibrium, the number of moles for each chemical species in a 6.0 L container was determined to be 1.0 mol NOCI, 0.63 mol NO and 0.51 mol Cl2. What is the Ke of the reaction? b.) At a specific point of the reaction, number of moles for each chemical species in a 4.5 L container was determined to be 0.42 mol NOCI, 0.21 mol NO and 0.48 mol Cl2. Based on the reaction's Q, will the equilibrium shift, yes or no? Which reaction will be favored? c.) Given the Ke computed in (a), what would be the equilibrium concentrations of NO and Clz if the equilibrium concentration of NOCI is 0.675?

Consider the reaction: NOC) = NO) + Cl2 (@) a.) At equilibrium, the number of moles for each chemical species in a 6.0 L container was determined to be 1.0 mol NOCI, 0.63 mol NO and 0.51 mol Cl2. What is the Ke of the reaction? b.) At a specific point of the reaction, number of moles for each chemical species in a 4.5 L container was determined to be 0.42 mol NOCI, 0.21 mol NO and 0.48 mol Cl2. Based on the reaction's Q, will the equilibrium shift, yes or no? Which reaction will be favored? c.) Given the Ke computed in (a), what would be the equilibrium concentrations of NO and Clz if the equilibrium concentration of NOCI is 0.675?

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

For this reaction, H;(g) + F:(g)→ 2HF(g)_ AH=-537 kl and K.= 1.15x102 Using LeChatlier's principle predict which direction the equilibrium will proceed when the following changes are made? A catalyst is added- F, is removed- The reaction vessel is compressed to half of its volüme H, is added. Temperature is increased Choose the suitable Word backward.forwardnochange
6. A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH3OH(g) → CO(g) + 2 H2(g), Ke= 6.90×10-². If the concentration of H₂ in the equilibrium mixture is 0.426M, what mass of methanol was initially introduced into the vessel?
= The reaction 2HBr(g) ⇒ H₂(g) + Br₂(g) measures [HBr] = 0.177 M, [H₂] = 0.223 M, and [Br₂] = 0.111 M after 5 seconds. If Kc = 1.05 at 25°C, in which direction is the reaction moving to reach equilibrium? Q = 0.790, moving forward (to the right) to reach equilibrium Q = 0.140, moving forward (to the right) to reach equilibrium Q = 0.140, moving reverse (to the left) to reach equilibrium Q = 0.790, moving reverse (to the left) to reach equilibrium
Suppose a 250. mL flask is filled with 1.0 mol of N, and 2.0 mol of NH,. This reaction becomes possible: N2 (g) + 3H,(g) – 2NH, (g) 2NH3 (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N2 H, NH, initial ? change equilibrium
At 700 K, the reaction 2SO,(g) + O2(g) 2SO3(g) has the equilibrium constant K = 4.3 x 106, and the following concentrations are present: [SO2] = 0.10M; [SO3] = 10. M; [02] = 0.10 M. Is the mixture at equilibrium? O There is not enough information to be able to predict the direction. O It is always at equilibrium O Yes, the mixture is at equilibrium. O No it is not at eqilibrium
. Consider the equilibrium 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H₂O(g). Predict the effect on the equilibrium concentration by the addition of N₂. A The equilibrium will shift to produce more nitrogen. B The equilibrium will shift to produce more reactants. C The equilibrium will shift to produce more products. D The reaction is already at equilibrium. E None of the above Given: 2P(g) + 3Cl2(g) → 2PC13(g) K Calculate the equilibrium constant for the following reaction. P(g) + 3/2Cl2(g) → PCI(g) AK BK¹ C 2K D 0.5K EK¹/2
Suppose a 500. mL flask is filled with 1.2 mol of H, and 1.6 mol of I,. The following reaction becomes possible: H2 (g)+ I½ (g) – 2HI (g) The equilibrium constant K for this reaction is 9.90 at the temperature of the flask. Calculate the equilibrium molarity of I,. Round your answer to two decimal places. M
For the reaction... N2 (g) + 3 H2(g) 2 NH3 (g) If the pressure in the system is increased, which substance will increase in concentration?
A mixture of 0.10 mole NO, 0.050 mole H₂, and 0.10 mole H₂O is placed in a 2.0 L vessel. The following equilibrium is established: + 2 H₂ (g) = N2(g) + 2 H₂O (g) 2 NO At equilibrium [NO] = 0.030 M. The initial concentration of N₂ was not mentioned so you must assume [N₂] = 0. Calculate the equilibrium concentrations (in M) of: More Information X H₂ (g) XN₂ (g) X H₂O (g) Question Answer Your answer -.020 is Your answer .035 is in Your answer .170 is i Tol: 0.0001 Tol: 0.001 Tol: 0.001
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.4 x 103 at a particular temperature. If the equilibrium concentrations of H,0 and H, are 0.11 M and 0.019 M, respectively, determine the concentration of O, at equilibrium.. 2 2 H,O(g) = 2 H,(g) + 0,(g) 2 NEXT > If [x] represents the equilibrium concentration of O, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms.. 2' K. = = 2.4 x 103 5 RESET [О.11] [0.019] 2[0.11] 2[0.019] [0.11]? [0.019]? [x] [x]? [2x] [2x]?
At a certain temperature, 0.900 mol SO, is placed in a 5.00 L container. 2 SO₂(g) 2 SO₂(g) + O₂(g) At equilibrium, 0.170 mol O₂ is present. Calculate Ke.
5. The reaction: 2NO₂(g) + 7H₂(g) = 2NH3(g) + 4H₂O(g) was allowed to reach equilibrium at 455 K. Analysis showed that there was 34.6 g of NO2, 53.2 g of H₂, 52.6 g of NH3 and 87.4 g H₂O present in a 2.65 L vessel once equilibrium was achieved. a. Determine the equilibrium concentration for both reactants. b. Determine the equilibrium concentration for both products. C. Write the Kc expression. d. Solve for the Kc. e. Solve for the Kp at the same temperature.