### Chemical Equilibrium Scenario and Analysis**Consider the following reaction where \( K_c = 10.5 \) at 350 K:**\[ 2 \, \text{CH}_2\text{Cl}_2 \, (g) \leftrightarrow \text{CH}_4 \, (g) + \text{CCl}_4 \, (g) \]A reaction mixture was found to contain:- \( 1.23 \times 10^{-2} \) moles of \( \text{CH}_2\text{Cl}_2 \, (g) \)- \( 5.29 \times 10^{-2} \) moles of \( \text{CH}_4 \, (g) \)- \( 4.07 \times 10^{-2} \) moles of \( \text{CCl}_4 \, (g) \)in a \( 1.00 \) liter container.**Indicate True (T) or False (F) for each of the following:**1. \( \_\_\_\_ \) In order to reach equilibrium \( \text{CH}_2\text{Cl}_2 \, (g) \) must be **consumed**.2. \( \_\_\_\_ \) In order to reach equilibrium \( K_c \) must **decrease**.3. \( \_\_\_\_ \) In order to reach equilibrium \( \text{CH}_4 \, (g) \) must be **consumed**.4. \( \_\_\_\_ \) \( Q_c \) is **greater** than \( K_c \).5. \( \_\_\_\_ \) The reaction is at **equilibrium**. No further reaction will occur.

For a particular reaction at constant temperature, the value of equilibrium constant (Kc) always…

Consider the following reaction where K, = 10.5 at 350 K: 2 CH,Cl2 (g) CH4 (g) + CCI4 (g) A reaction mixture was found to contain 1.23×10² moles of CH,Cl, (g), 5.29×10-² moles of CH4 (g), and 4.07×10-² moles of CC, (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: O 1. In order to reach equilibrium CH,Cl½(g) must be consumed . O 2. In order to reach equilibrium K̟ must decrease. O 3. In order to reach equilibrium CH4 must be consumed . O 4. Qe is greater than Ke. 5. The reaction is at equilibrium. No further reaction will occur.

Consider the following reaction where K, = 10.5 at 350 K: 2 CH,Cl2 (g) CH4 (g) + CCI4 (g) A reaction mixture was found to contain 1.23×10² moles of CH,Cl, (g), 5.29×10-² moles of CH4 (g), and 4.07×10-² moles of CC, (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: O 1. In order to reach equilibrium CH,Cl½(g) must be consumed . O 2. In order to reach equilibrium K̟ must decrease. O 3. In order to reach equilibrium CH4 must be consumed . O 4. Qe is greater than Ke. 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...

See similar textbooks

Similar questions

While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 1.9 mol of ethylene gas and 5.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 0.97 mol of ethylene gas and 4.77 mol of water vapor. The engineer then adds another 0.95 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol x10 X
Be sure to answer all parts. The equilibrium constant K, for the reaction I(g) 5 21(g) is 3.75 x 10 at 726°C. Calculate K, and Kp for the equilibrium 21(g) S1(g) at the same temperature. K.= X 10 %3D (Enter your answer in scientific notation.) Kp = %3D
I dont know how to do these two question on reaction quotient
Consider the reaction at a particular temperature: 2NO2(g) = 2NO(g) + O2(g) K, = 8.1 x 1012 Determine the Kp in scientific notation of the following reaction at the particular temperature: 4NO2(g) = 4NO(g) + 202(g) If the answer is 2.5 x 10, express the answer as 2.5E-2.
The reaction C(s) + 2 H₂(g) = CH₂(g) has Kp = 0.263 at 1000. K. Calculate the total pressure at equilibrium when 4.305 g of H₂ and 22.06 g of C(s) are placed in a 9.08 L flask and heated to 1000. K. Ptotal = Calculate the total pressure when 4.305 g of H₂ and 7.404 g of C(s) are placed in a 9.08 L flask and heated to 1000. K. Ptotal = atm atm
Consider the following system at equilibrium at 698 K: H₂(g) + I₂(9) 2HI(g) + 2.49 kcal Indicate whether each individual change would favor the production of HI(g). Evaluate each change separately, assuming that all other conditions remain constant. Increasing the temperature. Increasing the pressure. Decreasing the volume. Removing HI. Adding I₂. .....
Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas. PCl3(g) + Cl2(g) PCl5(g). A gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibriate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.128 atm, PCl2 = 0.141 atm, and PPCl5 = 1.21 atm. (a) What is the value of Kp at this temperature? ______ (b) Does the equilibrium favor reactants or products? The equilibrium favors products. The equilibrium favors reactants. Neither reactants nor products are favored.
Determine the equilibrium partial pressure of NH3 in a reaction vessel that initially contained 0.900 atm N2 and 0.500 atm H2 at 648 K.
2. Use the following information to calculate Kp and Ke for each reaction at 1000 K. CO2(g) + C(s) = 2C0(g) Kp = 1.50 at 1000 K a. 2c0(g) = CcO2(g) + C(s) 1 b. ½ CO2(g) + ½ C(s) = CO(g) c. 4C0(g) = 2CO2(g) + 2C(s)
Consider the following reaction where K, = 6.50x10-3 at 298 K. 2NOBR(g) =2NO(g) + Br2(g) A reaction mixture was found to contain 8.79x10-2 moles of NOBR(g), 2.03x10-2 moles of NO(g), and 4.53x10 2 moles of Bro(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.