4. Consider the system described by the following reaction: C₂H6(g) + O2(9) CO2(g) + H₂O AH-2847.6 kJ What effect would the following changes have on the concentration of all substances at equilibrium? State whether the amount of each chemical will increase or decrease after each change. Use Le Châtelier's principle to support your answers. a. The temperature of the container used for the reaction increases. b. The pressure increases. c. A catalyst is added. d. The volume of the container increases. e. [0₂] increases.

4. A. An important reaction in the commercial production of hydrogen is  CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift").  a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.

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

The chemical equation represents a reversible reaction. 3H2(9) + N2(9) # 2NH3(g) At equilibrium, 1 liter of a mixture of gases at 450°C contains 1.83 mol of hydrogen (H2), 0.793 mol of nitrogen (N2), and 1.72 mol of ammonia (NH3).What is the equilibrium constant for the reaction under these conditions? O A. 0.718 B. 0.609 O C. 1.39 O D. 0.159 96 5 6

Consider the following system at equilibrium: N2(g) + 3H2(g)  2NH3(g) + 92.94 kJWhich of the following changes will shift the equilibrium to the right? I. increasing the temperature II. decreasing the temperature III. increasing the volume IV. decreasing the volume V. removing some NH3 VI. adding some NH3 VII. removing some N2 VIII. adding some N2 ​ Group of answer choices I, IV, VI, VII II, III, V, VIII I, VI, VIII I, III, V, VII II, IV, V, VIII

In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC.  In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first.  This mixture is also heated to 350 oC.  After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?

Heating HI(g) at 425 °C causes some of this compound to decompose, forming H2 (g) and I2 (g). Eventually, the amounts of the three species do not change further, the system has reached equilibrium. (At this point, approximately 22% of the HI has decomposed.) What is happening in this system at the molecular level? O H2(g) reacts with I2 (g) to produce HI(g) at the same rate as it decomposes. H2 (g) and I2 (g) molecules collide with HI(g) making the reaction stop. Only part of the HI(g) molecules has enough energy to decompose at this temperature. 5:55 PM FLV 2/22/2020 Type here to search hp ins prt sc delete home f12 f8 f9 f10 f5 f6 f7 14 10 num & backspace lock 23 8. 3 %24

Answer the following questions

Consider the following endothermic reaction: 4 PCl5 (g)   ⇋⇋   P4 (s)   +   10 Cl2 (g) How will the amount of Cl2 be affected if the total pressure of the system is increased? Select one: a. The concentration of Cl2 will increase. b. The concentration of Cl2 will decrease. c. The amount of Cl2 will not change.

Consider the following equilibrium: 2NH3(g) → N₂(g) + 3H₂(g) AG = 34. kJ Now suppose a reaction vessel is filled with 6.39 atm of ammonia (NH3) and 0.200 atm of hydrogen (H₂) at 206. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 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. OO U rise fall yes no atm x10 X Ś