At a certain temperature the rate of this reaction is first order in H₂CO3 with a rate constant of 4.73 s H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 1.01 M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.212M. You may assume no other reaction is important. olo Round your answer to 2 significant digits. Ar s ? @ EH

At a certain temperature the rate of this reaction is first order in H₂CO3 with a rate constant of 4.73 s H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 1.01 M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.212M. You may assume no other reaction is important. olo Round your answer to 2 significant digits. Ar s ? @ EH

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

O A B с D a b C STEP 1: STEP 2: STEP 3: rate k rate k [OCI-][H₂O] [H] rate k [OCI-] [-][OH-] [OCI-][I] rate =k. [OH-] Oct (aq) + H₂O(l) → HOCI(aq) + OH(aq) l(aq) + HOCK(aq) → HOI(aq) + Cl(aq) OH(aq) + HOl(aq) → H₂O(l) + Ol(aq) [OCI-][I][H₂O] [OH-] FAST SLOW FAST
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0099 M's 2 NH3(g) N2(g)+ 3H,(g) Suppose a 4.0L flask is charged under these conditions with 450. mmol of ammonia. After how much time is there only 225. mmol left? 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 ammonia with a rate constant of 0.0078 M·s: 2 NH; (g) → N, (g) +3 H, (g) Suppose a 400. mL flask is charged under these conditions with 150. mmol of ammonia. How much is left 10. 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.
Subject-advance chemistry
At a certain temperature the rate of this reaction is second order in NH4OH with a rate constant of 0.0412M I 'S: NH4OH(aq) → NH3 (aq) + H2O (aq) Suppose a vessel contains NH4OH at a concentration of 1.36M. Calculate how long it takes for the concentration of NH4OH to decrease to 21.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ☐ Х
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0015 M's : 2 NH, (g) - N, (g)+3 H, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of ammonia. After how much time is there only 75.0 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. x10
At a certain temperature the rate of this reaction is first order in HI with a rate constant of 0.00183 s 2HI (g) → H₂(g) + 1₂ (g) Suppose a vessel contains HI at a concentration of 1.34M. Calculate the concentration of HI in the vessel 570. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 21/39 x10 X Ś 2. ?
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0085 M ·s 2 HI (g) – H, (g) + I,(3) Suppose a 2.0 L flask is charged under these conditions with 350. 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 2 significant digits. O
The balanced chemical equation for the reaction between iodine vapour and fluorine gas is: 3I2(g) + 6F2(g) → 2IF5(g) + I 4F 2(g) A chemist measures the rate at which iodine vapour is consumed to be 4.5 × 10–4 mol/(L•s). At what rate is F2(g) consumed?
At a certain temperature the rate of this reaction is first order in NH, with a rate constant of 7.43 s 3. 2NH3 (g) - N2 (g)+3H, (g) Suppose a vessel contains NH, at a concentration of 0.910M. Calculate how long it takes for the concentration of NH, to decrease to 0.0910M. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10
Aa.104.
The general rate law for the reaction is given by rate = k[NH4+]x[NO2-]y. Determine the order with respect to each reactant (i.e. solve for x and y). X = Y = Then determine the value of the rate constant, k (provide your answer to two significant figures). Rate constant, k = x 10 --