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?
consider the equilibrium reaction of H2 (g) + I2 (g) <-----> 2 HI (g) it has...
Consider the equilibrium reaction. H2(g) + I2(g) equilibrium reaction arrow 2 HI(g) In this case, 1.000 M H2 reacts with 2.000 M of I2 at a temperature of 414°C. The value of Kc = 72. Determine the equilibrium concentrations of H2, I2, and HI. [H2] [I2] [HI]
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
The following reaction: H2 (g) + I2 (g) ⇋ 2 HI (g) Has an equilibrium constant of 30.5 under certain conditions. If initial concentrations of reactants and product are: [H2] = 0.100 M; [I2] = 0.100 M; and [HI] = 0.250 M, what will be the equilibrium concentration of HI?
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.)
Consider the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T(∘C) [H2] [I2] [HI] [Kc] 25 0.0355 0.0388 0.922 − 340 − 4.55×10−2 M 0.384 M 90.6 445 4.90×10−2 M 4.74×10−2 M − 50.2 Find Kc at 25 ∘C. Find [H2] at 340 ∘C. Find [HI] at 445 ∘C.
Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations are [H2] = 0.200 M and [I2] = 0.400 M. The equilibrium constant Kc for the reaction following reaction is 57.0 at 700 K. (Show Work) H2(g)+I2(g)<--- ---->2HI(g)
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
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)...