O DOOO Consider the following reaction where K,=0.365 at 1150 K: %3D 2sO2(g) O2(g) =2s03(g) If the three gases are mixed in a rigid container at 1150 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following; v 1. A reaction will occur in which SO3(g) is produced. | 2. K, will increase. v 3. A reaction will occur in which SO, is produced. v 4. Q is less than K. v 5. The reaction is at equilibrium. No further reaction will occur.

O DOOO Consider the following reaction where K,=0.365 at 1150 K: %3D 2sO2(g) O2(g) =2s03(g) If the three gases are mixed in a rigid container at 1150 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following; v 1. A reaction will occur in which SO3(g) is produced. | 2. K, will increase. v 3. A reaction will occur in which SO, is produced. v 4. Q is less than K. v 5. The reaction is at equilibrium. No further reaction will occur.

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...

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ju sited Free Online Survey... Search Home - Academia... Submit Answer Retry Entire Group Modules [References] Use the References to access important values if needed for this question. Consider the following reaction where Kp = 0.160 at 298 K. 2NOBr(g) 2NO(g) + Br₂(g) If the three gases are mixed in a rigid container at 298 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: 1. A reaction will occur in which NOBr(g) is produced. 2. K, will increase. 3. A reaction will occur in which NO is produced. 4. Qp is greater than Kp. 5. The reaction is at equilibrium. No further reaction will occur. hp 8 Create Your Rubric -... 8 more group attempts remaining || K The Utility Experts ... E P insert » C 4x 12/ bac
Consider the following equilibrium: 2NH₂ (g)-N₂ (g) + 3H₂(g) AG-34. KJ Now suppose a reaction vessel is filled with 4.85 atm of ammonia (NH3) a system: Under these conditions, will the pressure of H, tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of H, will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of H₂ will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. and 2.40 atm of hydrogen (H₂) at 658. °C. Answer the following questions about this Ⓒrise O fall yes no atm 10 10 X S
Consider the following reaction where Ke = 10.5 at 350 K. 2CH₂Cl₂ (9) CH4 (9) + CCl4 (9) A reaction mixture was found to contain 0.0115 moles of CH₂Cl₂ (g), 0.0238 moles of CH₁ (g), and 0.0446 moles of CCl4 (g). in a 1.00 liter container. Calculate Qe ac Important values if needed for this question. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? O The reaction must run in the forward direction to reach equilibrium. The reaction must run in the reverse direction to reach equilibrium. OThe reaction is at equilibrium. Submit Answer Retry Entire Group 4 more group attempts remaining
■ W Chapter... G N. O LCG a Ⓒ BA H H The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if K, and Q are within 5% of each other.) (a) 2 NH3(g) = N₂(g) + 3 H₂(g) [NH3] = 0.485 M, [N₂]; = 0.160 M, [H₂] = 0.110 M, K = 18 What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. O It will not shift. (b) 2 NH3(9) N₂(g) + 3 H₂(g) What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. P (NH3) = 1.90 atm, P(N₂) = 11.65 atm, P(H₂) = 11.65 atm, K = 6.6x104 O To the right, i.e. the product-side. O It will not shift. (c) 2 SO 3(g) 2 SO₂(g) + O₂(9) What is the reaction quotient? webassign.net [SO3] = 1.65 M, [SO₂), = 1.65 M, [0₂], =…
For the reaction 2CH,(g) =C,H2(g) + 3H2(g) Ke = 0.155 at 1611 °C. What is K, for the reaction at this temperature? Express your answer numerically. • View Available Hint(s) ? Kp =
As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
2H20(g) + 3N2(g) 2 2N20(g) + N2H4(g) If K, for the above reaction is 781.8 at 200.9 K, what is Kp for the same reaction? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 12.3 and 120. and -123)
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if Kc and Qc are within 5% of each other.) (a.) 2 SO3(g) 2 SO2(g) + O2(g) Pi(SO3) = 0.100 atm, Pi(SO2) = 1.10 atm, Pi(O2) = 1.20 atm, Kp = 5.5 atm What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT? (b.) 2 NO(g) + Cl2(g) 2 NOCl(g) Pi(NO) = 1.25 atm, Pi(Cl2) = 1.25 atm, Pi(NOCl) = 0 atm, Kp = 3.1 ✕ 103 What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT? (c.) N2(g) + O2(g) 2 NO(g) [N2]i = 0.120 M, [O2]i = 0.240 M, [NO]i = 1.20 M, Kc = 0.050 What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT?
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
In the gas-phase reaction A + B=C+ 2 D, it was found that, when 2.00 mol A, 1.00 mol B and 3.00 mol D were mixed and allowed to come to equilibrium at 25°C, the resulting mixture contained 0.79 mol C at a total pressure of 1.00 bar. Calculate Kp. [.960]
3. Phosphoryl chloride, POCI3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCI3(8)and NO(g) according to the following equation: PCI3 (g) + NO2 (g) = POCI3 (g) + NO (g) The Keg for this reaction at 800 K is 6.90. If 1.25 mol PCI3 (g) and 1.94 mol NO2 (g) are placed into a 2.0 L container, what is the concentration of each gas at equilibrium at 800 K? PCI3 (g) NO2 (g) POCI3 (g) NO(g) Keq = 6.90 + + E
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