Iodine fluoride gas (IF) decomposes to gaseous iodide (I2) and fluoride (F2) at a high temperature. If Kp at this high temperature is 19.7, determine the equilibrium partial pressure of IF gas if its initial concentration was 0.306 atm? Hint: You should write a balanced chemical equation for the reaction described.
Question 6 options:
0.153 atm |
|
0.0689 atm |
|
0.168 atm |
|
0.0310 atm |
|
0.138 atm |
Iodine fluoride gas (IF) decomposes to gaseous iodide (I2) and fluoride (F2) at a high temperature....
Iodine fluoride gas (IF) decomposes to gaseous iodide (I2) and fluoride (F2) at a high temperature. If Kp at this high temperature is 19.7, determine the equilibrium partial pressure of IF gas if its initial concentration was 0.306 atm? Hint: You should write a balanced chemical equation for the reaction described. Question 6 options: 0.153 atm 0.0689 atm 0.168 atm 0.0310 atm 0.138 atm
lodine fluoride gas (IF) decomposes to gaseous iodide (12) and fluoride (F2) at a high temperature. If Kp at this high temperature is 19.7, determine the equilibrium partial pressure of IF gas if its initial concentration was 0.306 atm? Hint: You should write a balanced chemical equation for the reaction described. 0.138 atm 0.0310 atm 0.168 atm 0.0689 atm 0.153 atm
Phosphorous pentafluoride (PF5) gas decomposes into phosphorous (P4) gas and fluorine (F2) gas at a certain temperature. Determine the equilibrium constant for this reaction at this temperature if the measured equilibrium concentrations ([ ](eq)) are: [PF 5)(eq) = 0.0198 M, [P4(eq) = 0.317 M, [F2](eq) = 0.744 M. Hint: You should write a balanced chemical equation for the reaction described. 2.37 x 107 1.07 x 105 8.41 x 10-2 1.85 x 10-7 11.9 lodine fluoride gas (IF) decomposes to gaseous...
When gaseous F2 and I2 are heated to high temperatures, the I2 sublimes and gaseous iodine heptafluoride forms.? 310 torr of F2 and 3.60 g of solid iodine are put into a a 2.50 L container at 250 K and the container is heated to 550 K. What is the final pressure? What is the partial pressure of I2 gas?
When gaseous F2 and solid I2 are heated to high temperatures, the I2 sublimes and gaseous iodine heptafluoride forms. 280 torr of F2 and 4.00g of I2 are put into a 2.50L container at 250K and the container is heated to 550K. a) what is the final pressure in atm? b) what is the partial pressure of I2 gas in atm?
Hydrogen iodide gas decomposes into hydrogen gas and iodine gas at 453°C. If a 2.00 L flask is filled with 0.200 mol of hydrogen iodide gas, 0.156 mol hydrogen iodide remains at equilibrium. What is the equilibrium constant, Kc. for the reaction at this temperature? 2 HI (g) ⇌ H2 (g)+ I2 (8) 0.020 0.0062
Diatomic iodine [I2] decomposes at high temperature to form I atoms according to the reaction: I2(g)⇌2I(g), Kc=0.011 at 1200∘C In an equilibrium mixture, the concentration of I2 is 0.10 M. What is the equilibrium concentration of I?
Diatomic iodine (I2) decomposes at high temperature to form I atoms according to the reaction: I2(g)⇌2I(g),Kc=0.011 at 1200∘C In an equilibrium mixture, the concentration of I2 is 0.25 M. What is the equilibrium concentration of I?
Phosphorous pentafluoride (PF5) gas decomposes into phosphorous (P4) gas and fluorine (F2) gas at a certain temperature. Determine the equilibrium constant for this reaction at this temperature if the measured equilibrium concentrations ([ ](eq)) are: [PF5](eq) = 0.0198 M, [P4](eg) = 0.317 M, [F2](eq) = 0.744 M. Hint: You should write a balanced chemical equation for the reaction described. 11.9 1.07 x 105 8.41 x 10-2 1.85 x 10-7 2.37 x 107
18. Pure carbon dioxide (Pco2 = 1 atm) decomposes at high temperature. For the reaction system 2 CO2(9) #2 CO(g) + O2(9) the percentage of carbon dioxide that undergoes the decomposition reaction is as follows: Temperature Decomposition (K) 1500 0.048 2500 17.6 3000 54.8 Is this reaction endothermic? Calculate the value of K, at each temperature. 19. Elements of Group 16 form hydrides with the generic formula H.X. When gaseous H,X is bubbled through a solution that is strongly acidic,...