QUESTION 24 4 Consider the following reversible reaction: H2(g) + 12(9) 2 HI(g) K = 64.0...
Consider the reaction: H2(g) +12(9) =2HI(9) A reaction mixture in a 3.60 -L flask at 500 K initially contains 0.375 g H2 and 17.91 g 12. At equilibrium, the flask contains 17.76 g HI. Part A Calculate the equilibrium constant at this temperature. Express your answer using three significant figures. IVO AXDA O O ? K = Submit Previous Answers Request Answer X Incorrect; Try Again
At a particular temperature, K = 7.40 × 102 for the reaction H2 (g) + 12 (g) 늑 2H1(g) In an experiment, 3.30 moles of H2, 3.30 moles of I2, and 3.30 moles of HI are introduced into a 1.00-L container Calculate the concentrations of all species when equilibrium is reached Concentration of H2 = Concentration of - Concentration ofHi-M
a) H2(g) + 12 (g) = 2 HI(g) (3 points) A reaction mixture at equilibrium at 175 K contains Pue = 0.958 am, Pe=0.877 atm, and Pu=0.020 atm. A second reaction mixture, also at 175 K. contains Pie Pe=0.621 atm, and Pm 0.101 atm. Is the second reaction mixture at equilibrium? (Show all work for full credit) a IT b) (7 points) If not at equilibrium, what will be the partial pressure of HI when the reaction reaches equilibrium at...
1. At a given temperature the Kp = 4.76x10-4 for the reaction: H2(g) + 12(g) = 2 HI(g) Calculate the equilibrium partial pressure of Hl if the original reaction mixture contains H2 gas at 0.752 atm, 12 gas at 0.752 atm and Hl gas at 0.134 atm. a) 0.321 atm b) 0.810 atm c) 0.0177 atm d) 0.015 atm e) 0.192 atm
If the system: H2(g) + 12(g) = 2H1g) is initially at equilibrium, the amount of HI present in the equilibrium mixture at constant temperature could be increased by (A) (B) (C) (D) (E) increasing the pressure on the mixture. adding a catalyst increasing the concentration of H2 present. lowering the concentration of I2. increasing the volume of the reaction vessel.
Physical Chemistry Please help 4) Consider the following reaction at 298.15 K: H2(g) +12(g) = 2HI(g) a. Determine Agirn and Kp for this reaction if a mixture contains 2.82 bar HI and 0.0909 bar H2 and 12 at equilibrium. b. Determine the equilibrium concentrations if 0.0100 bar H2 and 0.0100 bar 12 are mixed together. 2. De rutand K, for thi
13. At a particular temperature the equilibrium constant for the reaction: H2(g)+F2(g) 2HF(g) is K 100.0. A reaction mixture in a 10.00-L flask contains 0.33 moles each of hydrogen and fluorine gases plus 0.40 moles of HF. What will be the concentration of H2 when this mixture reaches equilibrium? Submit Answer Tries 0/99
3. Loodeen For the reaction, H2(g) + 12(g) = 2 HI(g), K. = 54.9 at 699.0 K. at 699.0 K A system, at equilibrium contains 2.50 moles of HI and 2.12 moles of lz in a 5.00 liter vessel. How many moles of H2 should there be in the container? OOSIMHO a. 0.0537 moles OSOS Temmuz b. 0.380 moles c. 0.0215 moles d. 0.0107 moles EXIS e. 2.12 moles 4. A study of the system, 4 NH3(g) + 7 02(9)...
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.150 M CO and 0.150 M H2O. What will be the equilibrium concentration of [CO2]? What will be the equilibrium concentration of [H2]?
Given the equilibrium reaction: 2HI(g) H2(g) + I2(g) A sample mixture of HI, H2, and 12, at equilibrium, was found to have [H2]- 1.4 x 102 Mand [HI 4.0 x 102 M. If Keq 1.0 x 10, calculate the molar concentration of I2 in the equilibrium mixture, Enter your answer in the provided box. ]= м