6. Consider the following Co(g) + H2O(g) CO2(g) + H2(g) Ko= 0.58 at 1273 K A sealed 4.00L vessel initially contains 1.00 mole CO2(g), 1.00 mole H2(g), 0.600 moles CO(g), and 0.600 moles of H20(g). Calculate the moles of H2(g) present at equilibrium.

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 5.0 L flask with 4.9 atm of ethylene gas and 1.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 4.27 atm of ethylene gas and 1.27 atm of water vapor. The engineer then adds another 2.5 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. 000 Ar [ atm x10 X S ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 0 A 1

While ethanol (CH₂CH₂OH) 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 2.0 L flask with 4.7 atm of ethylene gas and 1.6 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 3.5 atm of ethylene gas and 0.40 atm of water vapor. The engineer then adds another 2.4 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm 33 0 x10 X S 114 ype URL 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility CH151 152_lab....docx ☆ ^ W + Chapter 13- Che....doc Show

Consider the following reaction where Kc = 1.20×10-2 at 500 K:PCl5 (g)  PCl3 (g) + Cl2 (g)A reaction mixture was found to contain 0.115 moles of PCl5 (g), 4.47×10-2 moles of PCl3 (g), and 4.16×10-2 moles of Cl2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following:    1. In order to reach equilibrium PCl5(g) must be consumed .    2. In order to reach equilibrium Kc must increase .    3. In order to reach equilibrium PCl3 must be consumed .    4. Qc is less than Kc.    5. The reaction is at equilibrium. No further reaction will occur.

Consider the following reaction where Kc = 1.29×10-² at 600 K: ? COCI₂ (9) co (g) + Cl₂ (9) A reaction mixture was found to contain 0.107 moles of COCI₂ (g), 5.31×10-² moles of CO (g), and 3.63×10-² moles of Cl₂ (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: F 1. In order to reach equilibrium COCI₂(g) must be produced. 2. In order to reach equilibrium K must decrease . 3. In order to reach equilibrium CO must be produced. Ⓒ 4. Qc is less than Kc. Ⓒ 5. The reaction is at equilibrium. No further reaction will occur.

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

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 1.5 L flask with 4.8 atm of ethylene gas and 3.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 3.1 atm of ethylene gas and 2.2 atm of water vapor. The engineer then adds another 1.2 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. at atm 5

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.

Consider the following reaction where K, = 9.52×10-2 at 350 K: %3D CH4(g) + CC14(g) 2CH2C1½(g) If the three gases are mixed in a rigid container at 350 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 CH,Cl2(g) is consumed. v 2. K, will increase. • 3. A reaction will occur in which CH, is consumed. • 4. Q is less than K. v 5. The reaction is at equilibrium. No further reaction will occur.

4) Choose the reactions below where K and K are equal. 302 (g) = 203 (9) CO (g) + H2O (g) = CO2 (g) + H2 (9) N2 (g) + 3H2 (g) 2NH3 (g) N2 (g) + O2 (9) : 2ΝΟ ( g)