04:19What Is Dynamic Equilibrium? | Reactions | Chemistry | FuseSchoolFuseSchool - Global Education461views1rank
Multiple ChoiceWhich one of the following statements does not describe the equilibrium state?a. While at equilibrium, a dynamic process is still occurring. b. The concentration of the reactants is equal to the concentration of the products.c. The concentration of the reactants and products reach a constant level.d. At equilibrium, the net concentration of all species is not changing.e. All are true. 2878views1rank2commentsHas a video solution.
Multiple ChoiceState which is greater in amount:reactants or products, based on the given equilibrium constant, K. 1463views6rank1commentsHas a video solution.
Multiple ChoiceThe decomposition of nitrogen monoxide can be achieved under high temperatures to create the products of nitrogen and oxygen gas. 6 NO(aq) ⇌ 3 N2(aq) + 3 O2(aq) a) What is the equilibrium equation for the reaction above?b) What is the equilibrium expression for the reverse reaction. 1616views5rank4commentsHas a video solution.
Multiple ChoiceThe equilibrium constant, K, for 2 NO (g) + O2 (g) ⇌ 2 NO2 (g) is 6.9 x 102. What is the [NO] in an equilibrium mixture of gaseous NO, O2, and NO2 at 500 K that contains 1.5 x 10 –2 M O2 and 4.3 x 10 –3 M NO2?3755views11rank15commentsHas a video solution.
Multiple ChoiceIn which of the given reactants is Kp greater than, less than and equal to Kc?a) SO3 (g) + NO (g) ⇌ SO2 (g) + NO2 (g)b) P4 (s) + 5 O4 (g) ⇌ P4O10 (s)c) 4 NH3 (g) + 3 O2 (g) ⇌ 2 N2 (g) + 6 H2O (g)2651views3rank6commentsHas a video solution.
Multiple ChoiceGiven the hypothetical reaction 2 A (s) + ? B (g) ⇌ 3 C (g), Kp = 0.0105 and Kc = 0.45 at 250 degrees Celsius. What is the value of the coefficient of B? 1838views1rank9commentsHas a video solution.
Multiple ChoiceWrite the equilibrium constant expression for the following reaction: CH4 (g) + 2 H2S (g) ⇆ CS2 (g) + 4 H2 (g)218views
Multiple ChoiceWhich of the following is true about the role of solids and liquids in equilibrium processes?115views
Multiple ChoiceMethane (CH4) reacts with hydrogen sulfide to yield hydrogen gas and carbon disulfide, a solvent used in the manufacturing rayon and cellophane. What is the value of Kc at 1000 K if the partial pressures in an equilibrium mixture at 1000 K are 0.20 atm methane, 0.15 atm hydrogen sulfide, 0.30 atm carbon disulfide and 0.10 atm hydrogen gas? CH4 (g) + 2 H2S (g) ⇌ 4 H2 (g) + CS2 (g)1795views4rank9commentsHas a video solution.
Multiple ChoiceWhich of the following does not represent a heterogenous equilibrium? I) CH4(g) + 2 O2(g) ⇌ CO2(g) + 2 H2O(g) II) CO2(g) + C(s) ⇌ 2 CO(g)III) 2 H2O(l) ⇌ 2 H2(g) + O2(g)IV) CH3COOH(aq) + H2O(l) ⇌ CH3COO–(aq) + H3O+(aq)180views9rankHas a video solution.
Textbook QuestionThe following diagrams represent a hypothetical reaction A ¡ B, with A represented by red spheres and B represented by blue spheres. The sequence from left to right represents the system as time passes. Does the system reach equilibrium? If so, in which diagram(s) is the system in equilibrium? [Sections 15.1 and 15.2] 765viewsHas a video solution.
Textbook QuestionThe following diagram represents a reaction shown going to completion. Each molecule in the diagram represents 0.1 mol, and the volume of the box is 1.0 L. (d) Assuming that all of the molecules are in the gas phase, calculate n, the change in the number of gas molecules that accompanies the reaction. [Section 15.2] 317viewsHas a video solution.
Textbook QuestionThe concept of chemical equilibrium is very important. Which one of the following statements is the most correct way to think about equilibrium? (a) If a system is at equilibrium, nothing is happening. (b) If a system is at equilibrium, the rate of the forward reaction is equal to the rate of the back reaction. (c) If a system is at equilibrium, the product concentration is changing over time.819viewsHas a video solution.
Textbook QuestionEthene 1C2H42 reacts with halogens 1X22 by the following reaction: C2H41g2 + X21g2 Δ C2H4X21g2 The following figures represent the concentrations at equilibrium at the same temperature when X2 is Cl2 (green), Br2 (brown), and I2 (purple). List the equilibria from smallest to largest equilibrium constant. [Section 15.3] 313viewsHas a video solution.
Textbook QuestionThe diagram shown here represents the equilibrium state for the reaction A21g2 + 2 B1g2 Δ 2 AB1g2. (a) Assuming the volume is 2 L, calculate the equilibrium constant Kc for the reaction. [Sections 15.5 and 15.7] 433viewsHas a video solution.
Textbook QuestionFor the general, single-step reaction A1g2 + B1g2 ∆ AB1g2, Kc = 4.5 * 10-6, which of the following statements is true? (LO 15.16) (a) Ea 1forward2 6 Ea 1reverse2 (b) The equilibrium mixture contains mostly products. (c) kr 7 kf (d) The reaction is exothermic.170viewsHas a video solution.
Textbook QuestionSuppose that the gas-phase reactions A ¡ B and B ¡ A are both elementary processes with rate constants of 4.7 * 10-3 s-1 and 5.8 * 10-1 s-1, respectively. (b) Which is greater at equilibrium, the partial pressure of A or the partial pressure of B?298viewsHas a video solution.
Textbook QuestionThe equilibrium constant for the dissociation of molecular iodine, I21g2Δ2 I1g2, at 800 K is Kc = 3.1 * 10-5. (b) Assuming both forward and reverse reactions are elementary processes, which reaction has the larger rate constant, the forward or the reverse reaction?953viewsHas a video solution.
Textbook QuestionWrite the expression for Kc for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. (e) 2 Ag1s2 + Zn2+1aq2 Δ 2 Ag+1aq2 + Zn1s2430viewsHas a video solution.
Textbook QuestionWrite the expressions for Kc for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. (g) 2 C8H181l2 + 25 O21g2 Δ 16 CO21g2 + 18 H2O1l2342viewsHas a video solution.
Textbook QuestionWrite the expressions for Kc for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. (b) Ti1s2 + 2 Cl21g2 Δ TiCl41l2299viewsHas a video solution.
Textbook QuestionWhich of the following reactions lies to the right, favoring the formation of products, and which lies to the left, favoring formation of reactants? (b) 2 HBr1g2 Δ H21g2 + Br21g2 Kc = 5.8 * 10-18421viewsHas a video solution.
Textbook QuestionWhich of the following statements are true and which are false? (c) As the value of the equilibrium constant increases, the speed at which a reaction reaches equilibrium increases.826viewsHas a video solution.
Textbook QuestionIf Kc = 0.042 for PCl31g2 + Cl21g2 Δ PCl51g2 at 500 K, what is the value of Kp for this reaction at this temperature?994viewsHas a video solution.
Textbook QuestionWrite an expression for the equilibrium constant of each chemical equation. a. SbCl5(g) ∆ SbCl3(g) + Cl2(g)740viewsHas a video solution.
Textbook QuestionFind and fix each mistake in the equilibrium constant expressions. b. CO(g) + Cl2(g) ⇌ COCl2(g) K = [CO][Cl2]/[COCl2]280viewsHas a video solution.
Textbook QuestionFind and fix each mistake in the equilibrium constant expressions. a. 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = [H2][S2]/[H2S]350viewsHas a video solution.
Textbook QuestionWhen this reaction comes to equilibrium, will the concentra- tions of the reactants or products be greater? Does the answer to this question depend on the initial concentrations of the reac- tants and products? A(g)+B(g) ⇌ 2C(g) Kc = 1.4x10^-51239viewsHas a video solution.
Textbook QuestionEthene (C2H4) can be halogenated by this reaction: C2H4(g) + X2(g) ⇌ C2H4X2(g) where X2 can be Cl2 (green), Br2 (brown), or I2 (purple). Examine the three figures representing equilibrium concentrations in this reaction at the same temperature for the three different hal- ogens. Rank the equilibrium constants for the three reactions from largest to smallest. 1147views1rankHas a video solution.
Textbook QuestionAt 1000 K, Kp = 1.85 for the reaction SO21g2 + 12O21g2 Δ SO31g2 (c) What is the value of Kc for the reaction in part (b)?871viewsHas a video solution.
Textbook QuestionH2 and I2 are combined in a flask and allowed to react according to the reaction: H2(g) + I2(g) ⇌ 2 HI(g) Examine the figures (sequential in time) and answer the questions: a. Which figure represents the point at which equilibrium is reached?557viewsHas a video solution.
Textbook QuestionA chemist trying to synthesize a particular compound attempts two different synthesis reactions. The equilibrium constants for the two reactions are 23.3 and 2.2 * 104 at room temperature. However, upon carrying out both reactions for 15 minutes, the chemist finds that the reaction with the smaller equilibrium constant produces more of the desired product. Explain how this might be possible.977viewsHas a video solution.
Textbook QuestionConsider the equilibrium N21g2 + O21g2 + Br21g2 Δ 2 NOBr1g2 Calculate the equilibrium constant Kp for this reaction, given the following information (at 298 K): 2 NO1g2 + Br21g2Δ2 NOBr1g2 Kc = 2.0 2 NO1g2ΔN21g2 + O21g2 Kc = 2.1 * 1030745viewsHas a video solution.
Textbook QuestionThe equilibrium 2 NO1g2 + Cl21g2 Δ 2 NOCl1g2 is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (b) If the vessel has a volume of 5.00 L, calculate Kc at this temperature.701views1commentsHas a video solution.
Textbook QuestionThe equilibrium 2 NO1g2 + Cl21g2 Δ 2 NOCl1g2 is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (a) Calculate Kp for this reaction at 500.0 K.251viewsHas a video solution.
Textbook QuestionPhosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl31g2 + Cl21g2 Δ PCl51g2. A 7.5-L gas vessel is charged with a mixture of PCl31g2 and Cl21g2, which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.124 atm, PCl2 = 0.157 atm, and PPCl5 = 1.30 atm. (a) What is the value of Kp at this temperature?1091viewsHas a video solution.
Textbook QuestionConsider the reaction: N (g) + 3H (g) ⇌ 2NH (g) Complete the table. Assume that all concentrations are equilib- rium concentrations in M. T (K) [n2] [H2] [nH3] Kc 500 0.115 0.105 0.439 575 0.110 ________ 0.128 775 0.120 0.140 ________ ________ 9.6 0.0584562viewsHas a video solution.
Textbook QuestionConsider the following reaction: H2(g) + I2(g) ⇌ 2 HI(g) Complete the table. Assume that all concentrations are equilib- rium concentrations in M. T (°C) [H2] [i2] [Hi] Kc 25 0.0355 0.0388 340 ________ 0.0455 445 0.0485 0.0468 0.922 ________ 0.387 9.6 ________ 50.21016viewsHas a video solution.
Textbook QuestionConsider the reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g) Kp = 28.4 at 298K In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 126 torr. What is the partial pressure of NOBr in this mixture?1423viewsHas a video solution.
Textbook QuestionConsider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kp = 2.91*10^3 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of Cl2 is 285 torr. What is the partial pressure of SO2Cl2 in this mixture?1267viewsHas a video solution.
Textbook QuestionConsider the interconversion of A molecules (red spheres) and B molecules (blue spheres) according to the reaction A ∆ B. Each of the series of pictures at the right represents a separate experiment in which time increases from left to right: (b) What is the value of the equilibrium constant Kc for the reaction A ∆ B?346viewsHas a video solution.
Textbook QuestionAt 900 K, the following reaction has Kp = 0.345: 2 SO21g2 + O21g2 Δ 2 SO31g2 In an equilibrium mixture the partial pressures of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?772viewsHas a video solution.
Textbook QuestionThe following picture represents the equilibrium state for the reaction 2 AB ∆ A2 + B2. Which rate constant is larger, kf or kr? Explain.584views1rankHas a video solution.
Textbook QuestionIdentify the true statement about the rate of the forward and reverse reaction once a reaction has reached equilibrium. (a) The rate of the forward reaction and the reverse reaction is zero. (b) The rate of the forward reaction is greater than the rate of the reverse reaction. (c) The rate of the reverse reaction is greater than the rate of the forward reaction. (d) The rate of the forward reaction is equal to the rate of the reverse reaction.846viewsHas a video solution.
Textbook QuestionAt 373 K, Kp = 0.416 for the equilibrium 2 NOBr1g2 Δ 2 NO1g2 + Br21g2 If the pressures of NOBr(g) and NO(g) are equal, what is the equilibrium pressure of Br21g2?364viewsHas a video solution.
Textbook QuestionAt 218 C, Kc = 1.2 * 10-4 for the equilibrium NH4SH1s2 Δ NH31g2 + H2S1g2 Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH4SH is placed in a closed vessel at 218 C and decomposes until equilibrium is reached.719views2rankHas a video solution.
Textbook QuestionAt 80 C, Kc = 1.87 * 10-3 for the reaction PH3BCl31s2 Δ PH31g2 + BCl31g2 (b) If the flask has a volume of 0.250 L, what is the minimum mass of PH3BCl31s2 that must be added to the flask to achieve equilibrium?163views1rankHas a video solution.
Textbook QuestionAt 80 C, Kc = 1.87 * 10-3 for the reaction PH3BCl31s2 Δ PH31g2 + BCl31g2 (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80 C and decomposes until equilibrium is reached.314viewsHas a video solution.
Textbook QuestionFor each of the equilibria in Problem 15.56, write the equi-librium constant expression for Kp and give the equation that relates Kp and Kc. (a)207views1rankHas a video solution.
Textbook QuestionAt 25 C, the reaction CaCrO41s2ΔCa2+1aq2 + CrO4 2-1aq2 has an equilibrium constant Kc = 7.1 * 10-4. What are the equilibrium concentrations of Ca2 + and CrO4 2- in a saturated solution of CaCrO4?279viewsHas a video solution.
Textbook QuestionThe vapor pressure of water at 25 °C is 0.0313 atm. Cal- culate the values of Kp and Kc at 25 °C for the equilibrium H2O1l2 ∆ H2O1g2.762viewsHas a video solution.
Textbook QuestionFor each of the following equilibria, write the equilibrium constant expression for Kc. Where appropriate, also write the equilibrium constant expression for Kp. (a) Fe2O31s2 + 3 CO1g2 ∆ 2 Fe1l2 + 3 CO21g2322viewsHas a video solution.
Textbook QuestionWhich of the following reactions yield appreciable equilib- rium concentrations of both reactants and products? (a) 2 Cu1s2 + O21g2 ∆ 2 CuO1s2; Kc = 4 * 1045440viewsHas a video solution.
Textbook QuestionThe value of Kc for the reaction 3 O21g2 ∆ 2 O31g2 is 1.7 * 10-56 at 25°C. Do you expect pure air at 25 °C to contain much O3 (ozone) when O2 and O3 are in equilib- rium? If the equilibrium concentration of O2 in air at 25 °C is 8 * 10-3 M, what is the equilibrium concentration of O3?392viewsHas a video solution.
Textbook QuestionAn equilibrium mixture of N2, H2, and NH3 at 700 K con- tains 0.036 M N2 and 0.15 M H2. At this temperature, Kc for the reaction N21g2 + 3 H21g2 ∆ 2 NH31g2 is 0.29. What is the concentration of NH3?601viewsHas a video solution.
Textbook QuestionThe value of Kc for the reaction of acetic acid with ethanol is 3.4 at 25°C: CH3CO2H1soln2 + CH3CH2OH1soln2 ∆ Acetic acid Ethanol CH3CO2CH2CH31soln2 + H2O1soln2 Kc = 3.4 (a) How many moles of ethyl acetate are present in an equi- librium mixture that contains 4.0 mol of acetic acid, 6.0 mol of ethanol, and 12.0 mol of water at 25 °C?1004viewsHas a video solution.
Textbook QuestionThe following equilibria were measured at 823 K: CoO1s2 + H21g2 ΔCo1s2 + H2O1g2 Kc = 67 H21g2 + CO21g2 ΔCO1g2 + H2O1g2 Kc = 0.14 (a) Use these equilibria to calculate the equilibrium constant, Kc, for the reaction CoO1s2 + CO1g2ΔCo1s2 + CO21g2 at 823 K.676viewsHas a video solution.
Textbook QuestionIn Section 11.5, we defined the vapor pressure of a liquid in terms of an equilibrium. (c) What is the value of Kp for any liquid in equilibrium with its vapor at the normal boiling point of the liquid?319viewsHas a video solution.
Textbook QuestionIn Section 11.5, we defined the vapor pressure of a liquid in terms of an equilibrium. (b) By using data in Appendix B, give the value of Kp for this reaction at 30 C.180viewsHas a video solution.
Textbook QuestionIn Section 11.5, we defined the vapor pressure of a liquid in terms of an equilibrium. (a) Write the equation representing the equilibrium between liquid water and water vapor and the corresponding expression for Kp.375viewsHas a video solution.
Textbook QuestionFor the reaction A2 + 2B ∆ 2 AB, the rate of the for- ward reaction is 18 M/s and the rate of the reverse reaction is 12 M/s. The reaction is not at equilibrium. Will the reaction pro- ceed in the forward or reverse direction to attain equilibrium?570viewsHas a video solution.
Textbook QuestionConsider a general, single-step reaction of the type A + B ∆ C. Show that the equilibrium constant is equal to the ratio of the rate constants for the forward and reverse reactions, Kc = kf>kr.367viewsHas a video solution.
Textbook QuestionWhich of the following relative values of kf and kr results in an equilibrium mixture that contains large amounts of reactants and small amounts of products? (a) kf 7 kr (b) kf = kr (c) kf 6 kr813viewsHas a video solution.
Textbook QuestionConsider the reaction of chloromethane with OH- in aque- ous solution: CH Cl1aq2 + OH-1aq2 ∆kf CH OH1aq2 + Cl-1aq2 At 25 °C, the rate constant for the forward reaction is 6 * 10-6 M-1 s-1, and the equilibrium constant Kc is 1 * 1016. Calculate the rate constant for the reverse reac- tion at 25 °C.242viewsHas a video solution.
Textbook QuestionRefining petroleum involves cracking large hydrocar- bon molecules into smaller, more volatile pieces. A simple example of hydrocarbon cracking is the gas-phase thermal decomposition of butane to give ethane and ethylene: (a) Write the equilibrium constant expressions for Kp and Kc.200viewsHas a video solution.
Textbook QuestionThe equilibrium constant Kc for the gas-phase thermal decom-position of cyclopropane to propene is 1.0 * 105 at 500 K: (a) What is the value of Kp at 500 K?255viewsHas a video solution.
Textbook QuestionConsider the sublimation of mothballs at 27 °C in a room having dimensions 8.0 ft * 10.0 ft * 8.0 ft. Assume that the mothballs are pure solid naphthalene 1density 1.16 g>cm32 and that they are spheres with a diameter of 12.0 mm. The equilibrium constant Kc for the sublimation of naphthalene is 5.40 * 10-6 at 27 °C. C10H81s2 ∆ C10H81g2 (b) How many mothballs are required to saturate the room with gaseous naphthalene?224viewsHas a video solution.
Textbook QuestionConsider the sublimation of mothballs at 27 °C in a room having dimensions 8.0 ft * 10.0 ft * 8.0 ft. Assume that the mothballs are pure solid naphthalene 1density 1.16 g>cm32 and that they are spheres with a diameter of 12.0 mm. The equilibrium constant Kc for the sublimation of naphthalene is 5.40 * 10-6 at 27 °C. C10H81s2 ∆ C10H81g2 (a) When excess mothballs are present, how many gaseous naphthalene molecules are in the room at equilibrium?146viewsHas a video solution.
Textbook QuestionOzone is unstable with respect to decomposition to ordi-nary oxygen: 2 O31g2 ∆ 3 O21g2 Kp = 1.3 * 1057 How many O3 molecules are present at equilibrium in 10 mil-lion cubic meters of air at 25 °C and 720 mm Hg pressure?364viewsHas a video solution.
Open QuestionWhich statement correctly describes a reaction in dynamic equilibrium? At dynamic equilibrium, the reactions stop and the amounts of reactants and products do not change. At dynamic equilibrium, the reactions continue but the amounts of reactants and products do not change. At dynamic equilibrium, the reactions stop but the amounts of reactants and products are changing. At dynamic equilibrium, the reactions continue and the amounts of reactants and products are changing.210viewsHas a video solution.