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.

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.

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

The rate equation for a reaction between substances M and N is : rate = K[M]2 [N]2 The initial rate is found to be 7.5 × 10–3 mol dm-3 s-1 when the initial concentration of M is of 0.25 mol dm-3 and the initial concentration of N is 0.50 mol dm-3. Determine the value of k. Select one: O a. 0.24 s-1 O b. 0.12 s-1 O c. 0.96 s-1 d. 0.48 s-1
None
General Chemistry 4th Edition McQuarrie • Rock • Gallogly dUniversity Science Books presented by Macmillan Learning The reaction C,H¿ (g) → 2 C,H¿(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-!. What is the value of the rate constant at 840.0 K? k =
The reaction C,H,(g) → 2 C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-'. What is the value of the rate constant : 775.0 K? k = ?
The reaction described by the equation 0,(g) + NO(g) - O2(g) + NO, (g) > has, at 310 K, the rate law rate of reaction k[O,][NO] k = 3.0 x 106 M-1.s-1 Given that [O,] = 2.0 × 10-4 M and [NO] = 4.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. rate: M/s What is the overall order of this reaction? 2 3 1
8 OKONETICS AND EQUILIBRIUM Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2N₂O, (g) → 2N₂O, (g) + O₂(g) He fills a reaction vessel with N₂O, and measures its concentration as the reaction proceeds: time (minutes) 0 10. [N₂O,] Explanation 0.300M 0.121 M 20. 0.0762 M 30. 0.0555 M 40. 0.0436M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. Check rate & D www-awa.aleks.com k= D.D X
: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9
The following reaction has a rate constant of 0.892 M-¹s-¹. Reaction: Y → Z If the reaction is initiated with [Y] = 0.521 M, before [Y] =0.305 M. seconds must pass Please write your answer with 3 significant figures, i.e. 1.23 s.
The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?
59.)
Consider the reaction: A + B --> products. From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant: [A] (M) [B] (M) Rate (M/s) 1.50 1.50 3.15 X 10-1 1.50 2.50 2.98 X 10 –1 3.00 1.50 5.50 X 10-1
Given below is the data for the reaction. Calculate the value of the rate constant "k" with proper units. A + B → C Set [A] (M) [B] (M) Init, rate M-sec 1 0.050 0.200 5.0 x 10-5 2. 0.100 0.200 5.0 x 10-5 0.050 0.600 4.5 x 10-4 Determine the order in "A" Determine the order in "B" Substitute the order for A and B in the rate law equation below. Rate = k [A]' [B]