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) H2(g) +12(g) Suppose a 350. mL flask is charged under these conditions with 100. mmol of hydrogen iodide. How much is left 20. 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. X ☐ x10

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) H2(g) +12(g) Suppose a 350. mL flask is charged under these conditions with 100. mmol of hydrogen iodide. How much is left 20. 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. X ☐ x10

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

Suppose a 350. mL flask is charged under these conditions with 100. mmol of hydrogen iodide. After how much time is there only 50.0 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.
Consider this reaction: 2H,PO, (aq)→ P,0, (aq) + 3H,0 (aq) At a certain temperature it obeys this rate law. rate = (14,5 M)[H,PO.] Suppose a vessel contains H,PO at a concentration of 1.17 M. Calculate how long it takes for the concentration of H,PO to decrease by 84.0%. You may 4 assume no other reaction is important. Round your answer to 2 significant digits.
I need help with this problem. I don't know how to start it.
At a certain temperature the rate of this reaction is first order in HI with a rate constant of 0.0263 s : 2HI (g) - H, (g)+I, (g) Suppose a vessel contains HI at a concentration of 0.130 M. Calculate the concentration of HI in the vessel 35.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. ) M x10
Consider this reaction: 2N,03 (g) → 2N,04(g) +O2 (g) At a certain temperature it obeys this rate law. rate =(167. Ms")[N,0, Suppose a vessel contains N,O, at a concentration of 0.220M. Calculate the concentration of N,0, in the vessel 0.200 seconds later. You may assume no 12 other reaction is important. Round your answer to 2 significant digits. () M x10
Consider this reaction: H,CO, (ag) – H,0 (aq) + CO, (ag) At a certain temperature it obeys this rate law. rate = (9.70 x 10-4s)H,co,] Suppose a vessel contains H,CO, at a concentration of 0.470 M. Calculate the concentration of H,CO, in the vessel 680. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x10
Consider this reaction: 2HI (g) → H₂ (g) + 1₂ (g) At a certain temperature it obeys this rate law. rate = (0.00315 M¹-s¯¹) [HI] ² S olo Suppose a vessel contains HI at a concentration of 1.16M. Calculate the concentration of HI in the vessel 970. seconds later. You may assume no other reaction is important. Ar Round your answer to 2 significant digits. M x10 X Ś ?
Mechanism
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0032 M's : 2 NH, (g) → N2 (g) +3 H, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of ammonia. How much is left 10. s later? You may assume no other reaction is important. olo Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. Ar
A reaction proceeds according to the following equation: A + 3B → 2C + 2D At an early stage of the reaction, conc. A = 1.191 M and 6.06 minutes later, conc. A= 0.949 M. What is the average rate of the reaction during this time period, expressed in units of M·s-1?
Measuring total pressure is a convenient way to monitor gas reaction: 2NOCl(g) → 2NO(g) + Cl2(g). The rate of the reaction depends on the concentration of the reactant, which is proportional to the partial pressure of the reactant. Derive a relation connecting its velocity above reaction with initial pressure, P0, and total pressure, Pt, at time t.(Hint: Assume the reaction is 2nd order. Make a table with initial (t0) and final values (t) of the moles of NOCl, NO, and Cl2, and construct the ideal gas equations for both cases. Use the ideal gas equation for t0 so that calculate the initial concentration of NOCl and substitute this value into the equation of ideal gases for t)
Consider this reaction: 2NH, (g) → N, (g) +3H, (g) At a certain temperature it obeys this rate law. 2 rate = (0.0581 Ms)[NH,1 Suppose a vessel contains NH, at a concentration of 1.39M. Calculate the concentration of NH, in the vessel 70.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ?