il occur. 6. The data below refer to the following reaction: 2N0(g) + Br2(g) R 之2NOBr(g) Initial Change uilibri 1.5 5.0 1.0 Equlbrium20 Calculate Ke. 7. Consider the reaction N2(g) + 02(g)-그 2N0(g), for which K. = 0.10 at 2,000°C. Starting with initial concentrations of 0.040 M of N2 and 0.040 M of O2, which of the following would be the correct way to determine the equilibrium concentrations? 2 =0.10 2x2 D) 2

Consider the following system at equilibrium where K. 7.00x10-5 and AH° = 182 kJ/mol at 673 K. NH4I (s) = NH3 (g) + HI (g) The production of NH3 (g) is favored by: Indicate True (I) or False (F) for each of the following: 1. increasing the temperature. v 2. decreasing the pressure (by changing the volume). v 3. increasing the volume. v 4. adding NH4I . 5. removing HI .

9 q eq eq req req 1req OWLv2 | Online teaching and learning resource from Cengage Le... Submit Answer [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, Kp, for the following reaction is 0.497 at 500. K. PC15 (9) PC13 (g) + Cl₂ (g) If an equilibrium mixture of the three gases in a 12.7 L container at 500. K contains PC15 at a pressure of 0.804 atm and PC13 at a pressure of 0.911 atm, the equilibrium partial pressure of Cl₂ is l atm. b Home | bartleby Retry Entire Group 9 more group attempts remaining

Consider the following system at equilibrium where K. = 9.52x102 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CC14 (g) =2 CH,Ch (g) The production of CH,Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: |1. decreasing the temperature. | 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. v 4. adding CH,Cl . | 5. removing CCI4 .

■ 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 =

Ctrl Tab Caps Shift 58°F Sunny Esc Fn Determine the temperature of a reaction if K = 1.20 x 106 when AG° = +21.00 kJ/mol. ! 1 Q A S N FI - - 2 W S F2 X Alt # 3 E Chat D C $ 4 R TI F H O DII % 5 V F5 T G ☀ F6 ^ Question 9 of 15 6 Y B * H & 7 PrtScn U N FB J * 8 Home 1 M ( 9 K End F10 O < 1 0 L PgUp P 4 1 7 +/- : Alt PgDr

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.

ient/takeCovalentActivity.do?locator-assignment-take Consider the following system at equilibrium where AH° = 198 kJ, and K. = 2.90x102, at 1.15x10° K. 2S03(g) 2S02(g) + O2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value ofK. A. increases. B. decreases. C. remains the same. The value of Q. A. is greater than K.. B. is equal to K. C. is less than K. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of O, will: A. increase. B. decrease. C. remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Prev

q The equilibrium constant, Ke, for the following reaction is 1.80 x 104 at 298 K. [Review Topics] [References] Use the References to access important values if needed for NH4HS(9) NH3(g) + H₂S(9) Calculate the equilibrium concentration of H₂S when 0.322 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H₂S] = M Submit Answer Show Hint NOV 30 Le... The equilib tv Retry Entire Group 9 more group attempts remaining Email In M