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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Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of ·0.0011Ms−1:2NH3(g)→N2(g)+3H2(g) Suppose a 5.0L ⁢ 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 2 significant digits.
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0041 M-s 2NH₂(g) → N₂(g) + 3 H₂ (g) Suppose a 450. mL flask is charged under these conditions with 100. mmol of ammonia. 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. 0 X S
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. = (0.291 M¹s¹) [N₂0₂] rate Suppose a vessel contains N₂O, at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O to decrease to 23.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Subm Continue Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cente 80°F Partly sunny ^ pe here to search B X G
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.0317 M¹-s¯¹) [₂0₂] S Suppose a vessel contains N₂O5 at a concentration of 0.440 M. Calculate the concentration of N₂O5 in the vessel 480. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ? X S
For this reaction: 2A (g) + 3B (g) → 3C (g) + 4E (g), а. Express the rate of the reaction in terms of the change in concentration of each reactant and product with time. b. When [E] is increasing at 0.22 mol/L.s, show how fast is [A] decreasing. [A] is decreasing by + unit is
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.
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
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.
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O₂(g) + NO(g) →→→ O₂(g) + NO₂ (g) -> The rate law for this reaction is rate of reaction = k [0₂] [NO] Given that k = 4.78 × 106 M-¹.s¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03] = 7.59 × 10-6 M and [NO]。 = 6.45 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h-¹.L-1
Consider a reaction A → B with activation energy 50.7 kJ/mol. At 19.5 °C, the rate constant, k, for this reaction is 0.095 s−1. Calculate the temperature, T (in °C), at which k = 0.329 s−1. Assume the pre-exponential factor (A) is constant with temperature. �=0.08206 L⋅atmmol⋅K=8.314 Jmol⋅K �K=�∘C+273.15 1 kJ = 1000 J Report your answer to three significant figures without the unit. Example: 20.0. Be sure that your answer is in °C and not Kelvin!
Consider the reaction described by the equation С,Н, Вr, (aq) + 3Г (аq) — С,н,(8) + 2 Br (aq) + I5 (aq) The rate law is rate = k[C,H,Br,][I¯] where k = 0.00594 M-1. s-!. What are the missing entries in the table? Run [C,H,Br, lo (M) [I-], (M) Initial rate of formation of C,H, (M-s -) 1 0.245 0.00143 0.245 y 0.000713 3 0.245 0.245