The disproportionation of hydrogen iodide, 2HI(g)-->H2(g)+I2(g), is an example of first order kinetics.
(i) Write the rate law for this reaction.
(ii) what are the units of k, the rate constant? Show how you determined the units
(iii) Prepare a plot (sketch) of the [HI] versus time.
The disproportionation of hydrogen iodide, 2HI(g)-->H2(g)+I2(g), is an example of first order kinetics. (i) Write the...
The disproportionation of hydrogen iodide, 2HI(g) —> H2(g) + I2(g), is an example of first order kinetics. 1) write the rate law for this reaction 2) what are the units of k, the rate law constant? Show how you determined the units.
Hydrogen iodide undergoes decomposition according to the equation 2HI (g) yields H2(g) + I2 (g) The equilibrium constant Kp at 500 K for this equilibrium is 0.060. Suppose 0.176 mol of HI is placed in a 5.00- L container at 500 K. What is the equilibrium concentration of H2?
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.)
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
In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)½ H2(g) + ½ I2(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.68×10-3 M-1 s-1 and a y-intercept of 2.66 M-1. Based on this plot, the reaction is ______ (zero/first/second) order in HI and the rate constant for the reaction is _____...
The gas phase decomposition of hydrogen iodide at 700 K
HI(g)½
H2(g) + ½ I2(g)
is second order in HI with a
rate constant of 1.20×10-3
M-1 s-1.
If the initial concentration of HI is
2.22 M, the concentration of HI
will be _____________________M after
2.21×103 seconds have
passed.
he rate constant for the formation of hydrogen iodide from the elements H2(g) + I2(g) → 2HI(g) is 2.7 × 10–4 L/(mol∙s) at 600 K and 3.5 × 10–3 L/(mol∙s) at 650 K. Find the activation energy Ea. J/mol Then calculate the rate constant at 684 K. L/(mol•s)
The gas phase reaction of hydrogen with iodine H2 + I2 ---------->2 HI is first order in H2 and first order in I2. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate=__________ In an experiment to determine the rate law, the rate of the reaction was determined to be 5.37×10-22 Ms-1...
Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. What will be the concentration of HI after t = 5.92×1010 s ([HI]t) for a reaction starting under the condition in the simulation?