Consider this reaction: 2H₂PO4 (aq) → P₂O5 (aq) + 3H₂O (aq) At a certain temperature it obeys this rate law. rate = (0.069 M¹.¹) [H₂PO₂] Suppose a vessel contains H₂PO4 at a concentration of 0.380 M. Calculate how long it takes for the concentration of H3PO4 to decrease to 5.0% of its initia value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? e 0 X S

Consider this reaction: 2H₂PO4 (aq) → P₂O5 (aq) + 3H₂O (aq) At a certain temperature it obeys this rate law. rate = (0.069 M¹.¹) [H₂PO₂] Suppose a vessel contains H₂PO4 at a concentration of 0.380 M. Calculate how long it takes for the concentration of H3PO4 to decrease to 5.0% of its initia value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? e 0 X S

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...

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Consider the hypothetical reaction: A + B + 20 → 2D + E where the rate law is Rate = -AL4 = k[AJ[B]2 At An experiment is carried out where [A]o = 7.200 x 102 M, [B]o = 2.500 M and [C], = 2.500 M. The reaction is started, and after 11.60 seconds, the concentration of A is 2.200 x 10° M. Calculate the value of k for this reaction in units of M²sª. Answer: 37.987 The correct answer is: 0.04811
When designing a consumer product, it is desirable for it to have a two-year shelf life. Often this means that the active ingredient in the product should not decrease by more than 5% in two years. If the reaction is first order, and the rate constant is: k = 2.56 × 10-2 yr 1, determine the half-life of an active ingredient that has a shelf life of 2.00 years. The half-life of an active ingredient is i yr.
2. Consider the reaction that occurs when a CIO2 solution and a solution containing hydroxide ions (OH) are mixed at 0°C, shown in the following equation. 2CIO2(aq) + 2OH (aq) → Cl03° (aq) + CIO2° (aq) + H2O (1) When solutions containing CIO2 and OH- in various concentrations were mixed at 0 oC, the following rate data were obtained: Determination Initial concentration Initial concentration of Initial rate for formation number of ClO2, mol/L OH", mol/L of CIO3¯ mol/Ls 1.25x10-2 1.30x10-3 2.33x10-4 2.50x10-2 1.30x10-3 9.34x104 3 2.50x10-2 2.60x103 1.87x10-3 a) Use the method of initial rates to find the order of the reaction with respect to CIO2 and with respect to OH. Write the rate equation for the reaction of CIO2 and OH´ at 0°C. b) Calculate the rate constant, k, for the reaction of clO2 and OH at 0°C. c) Calculate the reaction rate for the reaction CIO2 and OH at 0°C when the initial ClO2 and OH concentrations are 8.25x10-3 mol/L and 5.35x 10-² mol/L, respectively. 1.
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) +O₂ (g) At a certain temperature it obeys this rate law. rate = (0.0328 s−¹)[N₂05] S Suppose a vessel contains N₂O5 at a concentration of 0.860M. Calculate the concentration of N₂O5 in the vessel 22.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
Part A: Rate of Reaction Directions: Express the rate of the following chemical reactions in terms of the change in concentration of the reactants and products. 1) N₂(g) + 3H₂(g) → 2NH3(g) 2) 2C4H10(g) + 130₂(g) → 8CO₂(g) + 10H₂O(g)
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.
The reaction in aqueous acidic solution occurs as shown by the balanced chemical equation below: H2O2(aq) + 3 I (aq) + 2 H* (aq) 13 (aq) + 2 H20(I) In the first 40.0 seconds of the reaction, the concentration of I' changes from 1.000 M to 0.868 M. Use the information to determine the average rate of the reaction within the first 40.0 seconds of the reaction. O 3.20x103 M/s O 1.10x10-3 M/s O 4.40x10-3 M/s O 2.20x10-3 M/s
Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased
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Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A]2 where k= 1.45 ×10-2 M-1s-1 at a particular temperature. If the initial [A] = 0.300 M, what will be the concentration of A remaining after 3.00 minutes? 0.168 M 0.0221 M 0.296 M 0.287 M
Consider this reaction: 2H,PO, (ag) – P,0, (aq)+ 3H,0 (aq) At a certain temperature it obeys this rate law. rate = (0.392 M-1.s Suppose a vessel contains H, PO, at a concentration of 0.520 M. Calculate how long it takes for the concentration of H, PO, to decrease to 12.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
Questions 2A 2B and 2C please