The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to HI. The rate defined below is constant at 1.20 x 10-4 mol/L-s. Au 2 HI(g) H2 (9) + I (g) A[H] = k = 1.20 x 104 mol/L ·s At Rate = a. If the initial HI concentration was 0.650 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. Concentration = M b. How long will it take for all of the 0.650 M HI to decompose? Time = min

The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to HI. The rate defined below is constant at 1.20 x 10-4 mol/L-s. Au 2 HI(g) H2 (9) + I (g) A[H] = k = 1.20 x 104 mol/L ·s At Rate = a. If the initial HI concentration was 0.650 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. Concentration = M b. How long will it take for all of the 0.650 M HI to decompose? Time = min

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The initial rate of the reaction is determined for different initial conditions, with the results listed in the table. (a) What is the overall reaction order? (b) What is the value of the rate constant, k
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) 2 H2(g) + ½ I2(g) is zero order in HI with a rate constant of 1.20x10-4 M s1. If the initial concentration of HI is 0.376 M, the concentration of HI will be | M after 2.74x103 seconds have passed.
Cyclobutane, C4H8, consisting of molecules in which four carbon atoms for a ring, decomposes when heated to give ethylene. C4H8(g) → 2C2H4(g) The reaction is first order. In an experiment, the initial concentration of cyclobutane was (3.500x10^-3) M. After heating at 450 °C, for (5.55x10^2) s, this was reduced to (2.6090x10^-3) M. What was the concentration of cyclobutane after a total of (1.008x10^3) s? Express your answer to three significant figures. Just enter the number (e.g. 2.48x10^-4) and the unit.
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H,(g) + % »(9) is zero order in HI with a rate constant of 1.20×104M s!. If the initial concentration of HI is 0.103 M, the concentration of HI will be 1.33×10-2 M after seconds have passed.
At a certain temperature the rate of this reaction is first order in HI with a rate constant of 1.13 s : 2HI (g) → H2 (g) +I, (g) Suppose a vessel contains HI at a concentration of 1.01 M. Calculate the concentration of HI in the vessel 0.730 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Ox10
For the reaction: 3 Ag + NO3– + 4 H+ –––> NO + 2 H2O + 3 Ag+ If the rate of disappearance of Ag is 0.0017 mol L–1 s–1, what is the rate of the appearance of water? For the 1st order reaction: A ––> products, assume the concentration of A falls to one-third of its original value after 150 seconds. Calculate the rate constant and the half-life.
The reaction 2 NO (g) + O2 (g) → 2 NO2 (g) occurs when automobile exhaust releases NO into the atmosphere. Use the following data to determine the order with respect to NO for this reaction. Trial [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.012 0.020 1.02 x 10-4 2 0.024 0.020 4.08 x 10-4 3 0.024 0.040 8.16 x 10-4 Enter the answer as a single digit, not the word.
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0096 M •s *: 2 HI (g) – H, (g) + I,(3) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of hydrogen iodide. How much is left 3.0 s later? 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.
Initial rate: 1.6 •10^-7mol/L•s K=6.4 •10^-9L/mol•s Rate law: k[HI]^2 Can you please show me the steps.
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H,O,(aq) → H,0M + ½ O2(g) is first order in H,02 with a rate constant of 1.10×10-3 min!. If the initial concentration of H,O2 is 5.68×10-2 M, the concentration of H,O, will be |M after 2006 min have passed.
4) The decomposition of phosphorus pentachloride (PCIS) into phosphorus trichloride (PCI3) and chlorine gas (Cl2) is a first order process with a rate constant of 0.0842 s at a certain temperature. If 40.4 s after the reaction begins, the concentration of PCIs is 0.0203 M, what was the initial concentration of PCI3? (A) 6.76 x 104 M (B) 0.609 M (C) 3.42 M (D) (E) 0.495 M ES 0.820 Mt (D)
2 3 4 =5 #1 6 7 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0040 M-s¹: 2 HI (g) → H₂(g) + 1₂ (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of hydrogen iodide. How much is left 4.0 s later? 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. S A S ? Continue Submit 00 X