The vacancy concentration for a metal A with an activation energy Q is 2x10-5. Calculate the vacancy concentration for a second metal B with activation energy 1.2Q. (This question has only one correct answer) O a. 2.3 x 10-6 O b. 4.3 x 10:5 1.3 x 10-6 Od. 3.3 x 10-4

At a certain temperature, the equilibrium constant, K., for this reaction is 53.3. H,(g) + L, (g) = 2 HI(g) K. = 53.3 At this temperature, 0.400 mol H, and 0.400 mol I, were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI] = o DDI prt s delete home end 8. backspace num lock home K enter pause ↑ shift

(i) energy does not change,(ii) always absorbed energy,(iii) energy is always released,(iv) reactants may be formed.Which statement is true about the decomposition of an activated complex? A. (iii) and (iv)B. (i), (iii) and (iv)C. (ii) and (iii)D. (i), (ii) and (iv)E. (i) and (ii)

Determine the direction of the equilibrium will shift to as a result of the following changes

Which of the following statements is true? a. The concentration of a catalysts steadily decreases as a reaction proceeds b. A catalyst functions by selectively retarding the reverse directions c. A catalyst functions by lowering the activation energy for a reaction. d. A catalyst changes the ∆H for the reaction.

Ctrl Tab Caps Shift 58°F Sunny Esc Fn Determine the temperature of a reaction if K = 1.20 x 106 when AG° = +21.00 kJ/mol. ! 1 Q A S N FI - - 2 W S F2 X Alt # 3 E Chat D C $ 4 R TI F H O DII % 5 V F5 T G ☀ F6 ^ Question 9 of 15 6 Y B * H & 7 PrtScn U N FB J * 8 Home 1 M ( 9 K End F10 O < 1 0 L PgUp P 4 1 7 +/- : Alt PgDr

The answer is D but I'm not sure why. Please explain

The elementary reaction 101 4 2H₂O(g) = 2H₂(g) + O₂(g) proceeds at a certain temperature until the partial pressures of H₂O, H₂, and O₂ reach 0.0700 atm, 0.00350 atm, and 0.00300 atm, respectively. What is the value of the equilibrium constant at this temperature? Kp = O R 01 F % 5 1 T a G 6 24 1 & Y H 7 U 8 J 144 ( 9 K BO O O ☐ L Resources DDI P { 2. ✈ ? 59°F [ insert pause prt sc Hint 10/1/2022 backspace delete home enter pg ur T shift in er

Chapter 16 (Due 06/10, 23:00) O Saved 3 attempts left Check my work Be sure to answer all parts. Consider the following equilibrium process at 686°C: So CO;(g) + H2(g) = CO(g)+ H2O(g) Guidec The equilibrium concentrations of the reacting species are [CO] = 0.0500 M, [H2] = 0.0420 M, [CO2] = 0.0900 M, and [H,O] = 0.0350 M. ok (a) Calculate K, for the reaction at 686°C. int (b) If we add CO, to increase its concentration to 0.480 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? ences CO2: M H,: M CO: M H,O: M МaсВook Pro Thank We @ #3 $ 4. 5. 8. CO 3. 2.

A. Consider the endothermic reaction at 25oC: FeSCN+2(aq) --><-- Fe+3(aq) + SCN-(aq) What direction will the reaction shift in response to the following stresses? (Use arrows or write "right" , "left" , or "no shift").  a. More SCN- is added.  b. Solid sodium hydroxide is added. (iron (III) hydroxide is insoluble). c. The reaction container is set into ice water to cool. d. The pressure of the air around the reaction is doubled. e. Solid iron (III) chloride (FeCl3) is added. B. At 25oC, Kc for thr above reaction is 9.1 x 10-6. Determine the equilibrium concentration of Fe+3 in the solution if 0.50 mol of FeSCN+2 is dissolved to make 2.50 liters of solution.