At a certain temperature this reaction follows first-order kinetics with a rate constant of 2.98 s¹: 2H₂PO4 (aq) → P₂O5 (aq) + 3H₂O (ag) Suppose a vessel contains H₂PO4 at a concentration of 0.490 M. Calculate the concentration of H₂PO4 in the vessel 0.250 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X D

At a certain temperature this reaction follows first-order kinetics with a rate constant of 2.98 s¹: 2H₂PO4 (aq) → P₂O5 (aq) + 3H₂O (ag) Suppose a vessel contains H₂PO4 at a concentration of 0.490 M. Calculate the concentration of H₂PO4 in the vessel 0.250 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X D

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

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.657 s ': 2HI (g) → H, (g) + I, (g) Suppose a vessel contains HI at a concentration of 0.570M. Calculate the concentration of HI in the vessel 1.10 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x10
The first-order reaction: S02CI2 → SO2 + Cl2 has a rate constant equal to 2.20 x 10-5 s-1 at 593 K. What percentage of the initial amount of SO,Cl2 will remain after 22.3 hours? 92.8 % 85.4 % O 1.00 % 17.1 % 14.7 %
At a given temperature, a first-order reaction has a rate constant of 1.5 × 10–3 s–1. What is the time required for the reaction to be 32% completed?
Using the above data, determine the order of the reaction with respect to A and B, and the rate law.
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0188 s NH,OH (aq) → NH, (aq)+H,0 (aq) Suppose a vessel contains NH,OH at a concentration of 0.590M. Calculate the concentration of NH,OH in the vessel 49.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Under certain conditions the rate of this reaction zero order in dinitrogen monoxide with a rate constant of 0.0064 M · s: 2N,0 (g) – 2N, (g) +0, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. 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 2 significant digits.
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0066 s 2HI (g) → H, (g) + 12 (g): Suppose a vessel contains HI at a concentration of 0.220M. Calculate how long it takes for the concentration of HI to decrease to 6.0% of its initial may assume no other reaction is important. Round your answer to 2 significant digits.
At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.75Ms H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.130M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.0286 M. You may assume no other reaction is important. Round your answer to 2 significant digits. X ? S
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.00717 s : CICH,CH,CI (g) → CH,CHCI (g) + HCI (g) Suppose a vessel contains CICH,CH,Cl at a concentration of 1.00M. Calculate the concentration of CICH,CH,Cl in the vessel 89.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. |M Ox10 ?
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0424 s¯¹: S 2NH3(g) → N₂(g) + 3H₂(g) Suppose a vessel contains NH3 at a concentration of 0.460M. Calculate the concentration of NH3 in the vessel 17.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X 5
The reaction 2 NO(g) + Cl2(g) → 2 NOCl(g) is 2nd order in NO and 1st order in Cl2. 5 mol of nitric oxide and 2 mol of chlorine were brought together in a volume of 2 dm3 and the initial rate was 2.4× 10–3 mol dm3 s–1. What will be the rate when half of the chlorine has reacted?
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0022 M⚫s 1: 2 HI (g) →H₂ (g) +12(g) Suppose a 4.0 L flask is charged under these conditions with 250. mmol of hydrogen iodide. How much is left 7.0 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. X x10