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 |
Be sure to answer all parts. Kc for the reaction of hydrogen and iodine to produce...
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] =
1- Be sure to answer all parts Kc for the reaction of hydrogen and iodine to produce hydrogen iodide, H2(g) +12(g) = 2H1(e) is 54.3 at 430°C. Determine the initial and equilibrium concentration of Hi ir initial concentrations of H2 and 12 are both 0.11 M and their equilibrium concentrations are both 0.048 M at 430°C. [HI]i = [HI]e = 2-Be sure to answer all parts. Kc for the reaction of hydrogen and lodine to produce hydrogen iodide. H2(g) +1218)...
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
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.)
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2 (g) + I_2 (g) 2HI (g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of HI if initial concentrations of H_2 and I_2 are both 0.10 M and their equilibrium concentrations are both 0.043 M at 430 degree C. [HI]_i = M [HI]_e = M
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2(g)+I_2(g) doubleheadarrow 2HI(g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of H_2and I_2 are both 0.11 M and their equilibrium concentrations are both 0.048 M at 430 degree
Given the following information calculate the equilibrium concentrations of all species. H2 + I2 = 2HI Kc=54.3 Initial [H2]=[I2]=.500 M, [HI]=0
consider the equilibrium reaction of H2 (g) + I2 (g) <-----> 2 HI (g) it has an equilibrium constant Kc = 54.3 at 430°C. if the initial concentration of [HI]0 = 2.000 M. what are the equilibrium concentrations?
If a 2L reaction vessel initially contains 2 mols of Hydrogen and 2 mols of Iodine, what will be the molar concentrations at equilibrium of all species? H2 (g) + I2 (g) --> 2HI (g) Kc = 50.5