Carbonyl fluoride, COF,, is a chemical reagent useful in the synthesis of fluorinated organic compounds. The decomposition of COF, occurs at high temperature and with a catalyst according to the • Part A following reaction: 2 COF2(g) = CO2(g) + CFa(g) Determine the equilibrium constant at 651 K. Given that A,H° = -48.4 kJ mol-1 and the equilibrium constant at 821 Kis K= 9,17: O 69.5 O 1.44 O 9.19 O 9.15 O 58.4

FaceboOK [Review Topics] [References) Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° 268 kJ, and K. 5.10x106, at 548 K. %3D NH,CI(s) NH3(g) + HCI(g) When some moles of NH,CI(s) are removed from the equilibrium system at constant temperature: The value of K The value of Q. The reaction must O run in the forward direction to restablish equilibrium. O run in the reverse direction to restablish equilibrium. O remain the same. It is already at cquilibrium. The concentration of NH, will Retry Entire Group 1 more group attempt remaining Submit Answer

3. Consider the following reaction: Co(g) + 2H2(g) S CH;OH(g); Kp = 2.26x10ª at 25 °C Calculate AG for the reaction at 25 °C for each of the following conditions: (a) standard conditions (b) at equilibrium (c) P (CH3OH) = 1.0 atm, P (CO) = P (H2) = 0.010 atm

Consider the following system at equilibrium where K, = 154 and AH° = -16.1 kJ/mol at 298 K. 2 NO (g) + Brz (g) =2 NOB (g) The production of NOB (g) is favored by: Indicate True (T) or False (F) for each of the following; | 1. increasing the temperature. 2. increasing the pressure (by changing the volume). | 3. increasing the volume. V 4. removing NOB . 5. adding Br2.

A2(g) + 3B2(g) -> 2AB3(g) where the ΔGorxn is -140 kJ and equilibrium constant at standard conditions is 3.5x1024. a) If we place 0.100 atm of AB3, 0.050 atm of B2, and 0.500 atm of A2 in a container at 25oC, which direction will the reaction go (if any) to reach equilibrium? b) What is the value of ΔGrxn assuming the temperature is maintained at 25oC?

Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.

A] HgS occurs in two crystalline forms called "red" and "black". For the conversion of 8. L- the red form to the black form at 525 °C, 4Gº = -0.157 kJ mol-¹ and AH = 4.184 kJ mol-¹. Assuming the AH is temperature independent, find the temperature at which the two forms can coexist at equilibrium at 1.000 bar. Which is more stable above this temperature?

Consider the following system at equilibrium where Ho = 18.8 kJ, and Kc = 9.52E-2, at 350 K: CH4(g) + CCl4(g) 2 CH2Cl2(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature:   whats the value of Kc   The value of Q   The reaction must

[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH=-108 kJ, and K. 77.5, at 600 K. CO(g) + C,(g) COCI,(g) When 0.22 moles of Cl,(g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish cquilibrium. O remain the same. It is already at cquilibrium. The concentration of CO will Submit Answer Retry Entire Group 1 more group attempt remaining

Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical species that would be present in this solution are written in the second column of the table. Use the checkboxes to classify each compound. compound HCI W Ba (OH), HC,H,O, KCI Explanation patric(most common) 1 Other place . с important species present when dissolved in water E н,о, ст. н.о Ba, OH, H₂O но, с.н,о.. нс.н, о,, H,о K, CI, H₂O Check $ 4 R type of compound (check all that apply) ionic molecular strong weak strong weak acid acid base base Speciation is happening because the two groups split and live in other places 0 % 5 0 0 0 0 0 T 0 0 0 G Search or type URL 0 0 0 0 X Y 0 0 0 0 S & 0 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Access 0.5 U * 00 8 9