Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0040 M-s *: 2 HI (g) → H, (g) +I½ (g) Suppose a 250. mL flask is charged under these conditions with 300. mmol of hydrogen iodide. How much is left 80. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0040 M-s *: 2 HI (g) → H, (g) +I½ (g) Suppose a 250. mL flask is charged under these conditions with 300. mmol of hydrogen iodide. How much is left 80. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

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

- 1 Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0038 M's : 2 NH3 (g) - → N, (g) + 3 H2 (g) Suppose a 450. mL flask is charged under these conditions with 350. mmol of ammonia. How much is left 50. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Consider this reaction: NH,OH (aq) → NH, (aq) +H,0(aq) At a certain temperature it obeys this rate law. [NH, OH] rate = (1.32 M -1 •S Suppose a vessel contains NH¸OH at a concentration of 0.710 M. Calculate how long it takes for the concentration of NH¸OH to decrease by 83.0%. You may assume no other reaction is important.
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
Please don't provide handwritten solution .....
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0020 M·s 2 HI (g) → H, (g) + I, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 5.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
A chemical engineer is studying the rate of this reaction. 2N,O; (g) → 2N,O4 (g) +O, (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.8 0.6 0.4 0.2. 20 40 60 80 100 t (s) (W)['o°N]
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0044 M's : 2 HI (g) - H, (g) +I, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of hydrogen iodide. How much is left 8.0 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. x10
Consider this reaction: 2HI (g) → H, (g) +I, (g) At a certain temperature it obeys this rate law. rate =(0,465 s)[HI Suppose a vessel contains HI at a concentration of 0.540M. Calculate the concentration of HI in the vessel 2.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?
I completed the problem but for some reason, my answer is still wrong. for part a I got 5.48 x 10^-5 and for part b I got 5.61x10^-4. I substituted the concentrations in the equation but hey still seem to be wrong can someone explain?
- 1 Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0080 M's : 2 NH3 (g) → N, (g)+3 H, (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of ammonia. How much is left 2.0 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. x10 ?
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0045 M's : 2 HI (g) → H, (g)+I, (g) Suppose a 250. mL flask is charged under these conditions with 350. mmol of hydrogen iodide. How much is left 80. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10