Consider the following system at equilibrium at 500 K: PCI5 (9) +21.0 kcalPCl3 (9) + Cl₂ (9) Indicate whether each individual change would favor the production of PC13 (9). Evaluate each change separately, assuming that all other conditions remain constant. Increasing the temperature. [ Decreasing the pressure. Decreasing the volume. Adding PCls. Adding Cl₂. ences] eferences to access important values if needed for this question. Submit Answer Retry Entire Group 3 more group attempts remaining Previous Next

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. .....

12.) A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g) = N2(g) + 3H2(g) At equilibrium, the mixture contained to following concentrations: [H2] = 0.0283 M, [N2] = 0.00944 M,[NH3] = 0.101 M. What is Kp at this temperature?

Methanol is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g) + 2 H­2(g) <-> CH3OH(g). At equilibrium mixture in a 1.05 L vessel is found to contain 0.652 mol CH3OH, 0.386 mol CO, and 0.209 mol H2.  Calculate the value of Kc.

Type the word True or False in the provided space for the following. Consider the following system at equilibrium where Kc = 9.52x10-2 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CCl4 (g) → 2 CH₂Cl₂ (g) The production of CH₂Cl2 (g) is favored by: decreasing the temperature. increasing the pressure. increasing the volume. removing CH₂Cl2. removing CCl4. I. II. III.____ IV. V.

Consider the following reaction where Kc PC15 (9) PC13 (g) + Cl₂ (9) A reaction mixture was found to contain 0.117 moles of PC15 (g), 0.0259 moles of PC13 (g), and 0.0368 moles of C1₂ (g), in a 1.00 liter container. Calculate c Qc² = = 0.0120 at 500 K. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? O The reaction must run in the forward direction to reach equilibrium. O The reaction must run in the reverse direction to reach equilibrium. O The reaction is at equilibrium.

Write the expression for the equilibrium constant K, for the following reaction. (Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH)2 as (P NH3)². If either the numerator or denominator is 1, please enter 1.) PCI5(g) + PCI3(g) + Cl2(g) K ||

6. Write the equilibrium constant expression for the following reactions. a. CHa (8) + 20; (B) → CO; (B) + 2H;0 (g) b. 4 NH3 (g) + 302 (g) → 2N2 (g) + 6H;0 (g) c. C (s) + 2H2 (g) CH4 (g)