2. Consider the following equilibrium system: _NO2(g) → _N2₂04 (g) Two sets of equilibrium data are listed for the same temperature. Container 1 2.00 L 0.12 moles NO2 0.16 moles N204 ? moles N204 0.26 moles NO2 Container 2 5.00 L Determine the number of moles N204 in the second container. 3. A student places 2.00 moles SO3 in a 1.00 L flask. At equilibrium [0₂] = 0.10 M at 130 °C. Calculate the keq. _SO2(g) + O2(g) ⇒ _SO3(g) 4. At equilibrium the 4.0L flask contains the indicated amounts of the three chemicals. PCI5.012 mol H20.016 mol HCI .120 mol Calculate [POCI3]. _PCIs (s) + _H₂O(g)_HCI (g) +_POCI3 (g) Keq=11

2. Consider the following equilibrium system: _NO2(g) → _N2₂04 (g) Two sets of equilibrium data are listed for the same temperature. Container 1 2.00 L 0.12 moles NO2 0.16 moles N204 ? moles N204 0.26 moles NO2 Container 2 5.00 L Determine the number of moles N204 in the second container. 3. A student places 2.00 moles SO3 in a 1.00 L flask. At equilibrium [0₂] = 0.10 M at 130 °C. Calculate the keq. _SO2(g) + O2(g) ⇒ _SO3(g) 4. At equilibrium the 4.0L flask contains the indicated amounts of the three chemicals. PCI5.012 mol H20.016 mol HCI .120 mol Calculate [POCI3]. _PCIs (s) + _H₂O(g)_HCI (g) +_POCI3 (g) Keq=11

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

The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be? H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?
MAI Van JL.cas-Cudo Lab Assignment #3 E.mheducation.com Saved # 3 6 Be sure to answer all parts. Consider the following equilibrium system involving SO2, Cl2, and SO,Cl, (sulfuryl dichloride): SO2(g) + Cl2(g) = SO,C(g) Predict how the equilibrium position would change if the following changes were to occur. The temperature remains constant in each case. (a) Cl, gas is added to the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. ((More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (b) SO,Cl, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (c) SO, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More…
Consider the following exothermic reaction: C (s) + 2 Cl2 (g) ⇋⇋ CCl4 (g) How would the equilibrium shift if the reaction mixture is heated? Select one: a. The reaction would shift towards the products. b. The reaction would shift towards the reactants. c. The equilibrium would not be affected.
4. For the reaction CH4(g) + 2 H2S(g) = CS2(g) + 4 H₂(g) Kc = 3.59 at 900 °C. For each of the following measured concentrations determine whether the reaction is at equilibrium. If not, in which direction will the reaction proceed to get to equilibrium? [CH] [H₂S] [CS₂] [H2] Expt 1 Expt 2 Expt 3 1.15 1.07 1.10 1.20 1.20 1.49 1.51 0.90 1.10 1.08 1.78 1.68
Use the following information to answer the next question Factors that can affect equilibrium I and II III only I, II, and III I. O II only II. III. The factors from the list above that would increase the equilibrium concentration of NO(g) in the system; 4NH3(g) +502 (g) 4NO(g) + 6H₂O(g) AH = -905 kJ while all other variables are held constant are Decreasing the volume Increasing the temperature Adding NH3(g)
A sample of H,S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium. What is the total pressure of all gases in the container? 2H2S(g) = 2H2(g) + S2(g) K, = 3.85 x 10-7 0.497 atm 0.215 atm 0.793 atm 0.624 atm 0.387 atm O O O
Consider the following reaction at equilibrium. Which of the following changes will shift the equilibrium to the left? CH4(g) + Cl2(g) ⇌ CCl4(l) + HCl(g) ΔH°= –398 kJ I. Increasing the temperature II. Decreasing the temperature III. Increasing the volume IV. Decreasing the volume V. Removing some Cl2 VI. Adding some Cl2 VII. Removing some HCl VIII. Adding some HCl A. I, IV, VI, VII B. II, III, VI, VIII C. I, VI, VIII D. I, III, V, VIII E. II, IV, VI, VII
Consider the reaction: Heat + CaSO3(s) <----> CaO(s) + SO2(g) What change will cause an increase in the pressure of SO2 when equilibrium is reestablished? increasing the reaction temperature decreasing the volume of the container adding more CaSO3 removing CaO
see image
For the following reaction, K, = 0.262 at 1000°C: C(s) + 2 H2(g) = CH4(g) At equilibrium, Pa, is 1.22 atm and 1.35 g of carbon is present. What is the equilibrium partial pressure of CH4(g)? 0.390 atm 5.68 atm 0.997 atm 0.320 atm 0.624 atm None of these
Consider the following exothermic reaction: C (s) + 2 Cl2 (g) ⇋⇋ CCl4 (g) How would the equilibrium shift if the reaction mixture is heated? Select one: a. The reaction would shift towards the products. b. The reaction would shift towards the reactants. c. The equilibrium would not be affected.