Consider the following system at equi 2HI(g) =H₂(g) + I2(9) If the TEMPERATURE on the equilibr The value of KcA. Increases B. Decreases C. Remains the s

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.

Use arrows (up / down) to indicate the affect of each of these disturbances (stresses) on the concentration of the reactants and products in this equilibrium: 9 KJ + 2 S02 9) + 02 (9) = 2 S03 (9A disturbance affect on affect on affect on ISO2] [02] ISO3] decrease [SO2] increase [02] increase [SO3] increase pressure decrease temp Period 4 CHE

9) Given the following equilibrium reaction below, indicate which direction the reaction will shift when the indicated stresses are applied (à, ß, or none), AND indicate how the K value will change (increase, decrease or stays same) with the stress. P = 1 atm, unless otherwise specified. ​​CO(g) + Cl2(g) ó COCl2(g) ​ H = –107.6 kJ/mol What will happen if:​​​​​Shift​​​K value i) The pressure is quadrupled​​​​_______​_________________​ ii) The reaction temperature is decreased​​_______​__________________ iii) More COCl2 gas is added​​​​_______​__________________ iv) The volume is doubled​​​​_______​__________________

Consider the following equilibrium: N₂(g) + 3H₂(g)2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 9.24 atm of ammonia 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. rise O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this S

Consider the following system at equilibrium where AH = 268 kJ and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) NH3(g) + HCl(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: decreasing the pressure (by changing the volume): increasing the volume: adding NH4Cl: adding HCl:

▸ 69 20 E Consider the following system at equilibrium at 723 K: N₂(g) + 3H₂(g) 2NH3(g) + 26.6 kcal Indicate whether each individual change would favor the production of NH3(g). Evaluate each change separately, assuming that all other conditions remain constant. D Decreasing the temperature. Decreasing the pressure. Increasing the volume. Removing NH3. Removing H₂. C Submit Answer $ 4 R F % 5 V Retry Entire ♫ FS T G [References] the References to access important values if needed for this question. A 6 v yes no B MacBook Air F6 3 more group attempts remaining Y H & 7 B F7 U N * 8 00 D--ll FB J J ( T 1 M 9 K DD FO O O L ge A F10 P command Previous Email Instructor 4 i A AN = Next> Save and Exit ( { ? 912 option delete retu