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 when [H2] = 1.49×10-2 M and [I2] = 1.61×10-2 M. From this experiment, the rate constant is _________M-1s-1.
The gas phase reaction of hydrogen with iodine H2 + I2 ---------->2 HI is first order...
The reaction H2(g) + I2(g) → 2 HI (g) is first order in both hydrogen and iodine. It is therefore referred to as second order overall. Its rate constant for the formation of HI (g) at 400 ◦C is 2.34 × 10−2 · lit · mol−1 · sec−1 and its activation energy is 150 KJ/mol. Use the rate law to estimate how long it takes to form 0.1 mole of HI(g) if I start by putting 2 moles 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.)
The reduction of nitric oxide with hydrogen 2 NO + 2 H2—+N2 + 2 H20 is second order in NO and first order in H Complete the rate law for this reaction in the box below. Use the form k[A]”[B]"..., where 'l' is understood for m. n ... (don't enter l) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.82 M-5....
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 reaction 2HI → H2 + I2 is second order in [HI] and second order overall. The rate constant of the reaction at 700°C is 1.57 × 10−5 M −1s−1. Suppose you have a sample in which the concentration of HI is 0.75 M. What was the concentration of HI 8 hours earlier? A) 0.45 M B) 0.75 M C) 2.3 M D) 1.9 M
For the gas phase decomposition of hydrogen iodide at 700 K 2 HI H2+ I2 the following data have been obtained: 1.77 0.452 0.720 0.329 [HI], M 11.5 23.0 34.5 time, s Ms. The age rate of disappearance of HI over the time period from t =11.5 s to t = 23.0 s is
The gas phase decomposition of HI into H2 and I2 is found to have an activation energy of 198 kJ/mol. The rate constant at 775 oC is 1.54 x 10-4 M-1s-1. What is the value of the rate constant at 977 oC?
2 ICl + H2----->I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.129 8.70×10-2 1.67×10-3 2 0.258 8.70×10-2 3.34×10-3 3 0.129 0.174 6.68×10-3 4 0.258 0.174 1.34×10-2 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 or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = ____________ From these data,...
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.