Hydrogen gas, iodine vapor, hydrogen iodine are mixed in a flask and heated to 642°C.
H2(g) + I2(g) ⇋ 2 HI(g) Kc = 53 at 642°C
If the initial concentrations of hydrogen gas and iodine vapor are both 0.054 mol/L and the concentration of hydrogen iodine is 0.130 mol/L what is the equilibrium concentration of hydrogen gas? Enter a number to 4 decimal places.
Hydrogen gas, iodine vapor, hydrogen iodine are mixed in a flask and heated to 642°C. H2(g)...
Hydrogen gas, iodine vapor and hydrogen iodide gas are added to an evacuated flask until the concentrations of H2 and I2 are both 2.0 M and that of HI equals 8.0M K=9.00 at 423C The reaction vessel is heated to 675 where the equilibrium concentration of the HI is determined to be 6.0M What is the K value at 675C
Kc for the reaction of hydrogen and iodine to produce hydrogen iodide, H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Determine the initial and equilibrium concentration of HI if initial concentrations of H2 and I2 are both 0.10 M and their equilibrium concentrations are both 0.052 M at 430°C
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
c for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) <-> 2HI(g) is 54.3 at 430 degrees Celsius. Calculate the equilibrium concentrations of H2, I2, and HI at 430 degrees Celsius if the initial concentrations are (H2) = (I2) = 0 M, and (HI)= 0.393 M. (H2) = _______ M (I2) = _________ M (HI) = _________ M (Please explain with an ICE chart if possible.)
c for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) <-> 2HI(g) is 54.3 at 430 degrees Celsius. Calculate the equilibrium concentrations of H2, I2, and HI at 430 degrees Celsius if the initial concentrations are (H2) = (I2) = 0 M, and (HI)= 0.393 M. (H2) = _______ M (I2) = _________ M (HI) = _________ M (Please explain with an ICE chart if possible.)
Suppose that 0.1000 mole each of H2 and I2 are placed in 1.000-L flask, stoppered, and the mixture is heated to 425oC. At equilibrium, the concentration of I2 is found to be 0.0210 M. a) What are the equilibrium concentrations of H2 and HI, respectively? Calculate Kc for the following reaction at 425oC. H2(g) + I2(g) ⇄ 2 HI(g) b) If the initial concentrations of H2 and I2 are 1.000 M each, and the initial concentration of HI is 0.000,...
a) In order to study hydrogen halide decomposition, a researcher fills an evacuated 1.79 L flask with 0.452 mol of HI gas and allows the reaction to proceed at 428°C: 2HI (g) ⇋ H2(g) + I2(g) At equilibrium, the concentration of HI = 0.055 M. Calculate Kc. Enter to 4 decimal places. HINT: Look at sample problem 17.6 in the 8th ed Silberberg book. Write a Kc expression. Find the initial concentration. Fill in the ICE chart. Put the E (equilibrium) values...
1. In order to study hydrogen halide decomposition, a researcher fills an evacuated 1.79 L flask with 0.222 mol of HI gas and allows the reaction to proceed at 436°C: 2HI (g) ⇋ H2(g) + I2(g) At equilibrium, the concentration of HI = 0.09 M. Calculate Kc. Enter to 4 decimal places. HINT: Look at sample problem 17.6 in the 8th ed Silberberg book. Write a Kc expression. Find the initial concentration. Fill in the ICE chart. Put the E (equilibrium) values...
Be sure to answer all parts. Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H2, I2, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.419 M. [H2] = [I2] = [HI] =
Be sure to answer all parts. Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H2, I2, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.349 M. [H2] = M [I2] = M [HI] = M