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.
The disproportionation of hydrogen iodide, 2HI(g) —> H2(g) + I2(g), is an example of first order...
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.
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?
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...
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
Consider the following reaction: H2 + I2 ➞ 2HI They react by a second-order process, first order with respect to each reactant with k = 0.63 L/(mol*sec). a) What is the initial reaction rate when we add 0.50 g H2 and 0.20 g I2 to a 800. mL vessel? b) How does the reaction rate change (by what factor/amount) when we add 0.10 g I2 to the above mixture?
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)
1a. Hydrogen iodide decomposes when heated, forming H2 (g) and I2 (g). The rate law for this reaction is -delta[HI]/delta t = k[HI]^2. At 443 °C, k=30.L/molxmin. If the initial HI (g) concentration is 5.5x10^-2 mol/L, what concentration of HI (g) will remain after 10. minutes? Concentration = ____ mol/L 1b. The decomposition of SO2Cl2 SO2Cl2 (g) ----> SO2 (g) + Cl2 (g) is first-order in SO2Cl2, and the reaction has a half-life of 245 minutes at 600 K. If...
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0096 M(s-1): 2HI(g) --> H2(g) + I2(g) Suppose a 4.0L flask is charged under these conditions with 300.0 mmol of hydrogen iodide. After how much time is there only 150.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.