**Chemistry: Understanding Reaction Rates****Reaction:**\[ 2N_2O_5 (aq) \rightarrow 4NO_2 (aq) + O_2 (g) \]**Problem Statement:**What is the rate of disappearance of \( N_2O_5 \) from 200 to 400 seconds?**Data Table:**| Time (s) | \([N_2O_5]\) | \([NO_2]\) | \([O_2]\) ||----------|--------------|------------|-----------|| 0 | 1.00 | 0 | 0 || 200 | 0.88 | 0.24 | 0.12 || 400 | 0.78 | ? | ? || 600 | 0.69 | 0.62 | 0.16 || 800 | 0.61 | 0.78 | 0.20 |**Explanation:**The table above represents the concentration of \( N_2O_5 \), \( NO_2 \), and \( O_2 \) at various times during the reaction. **Rate Calculation:**To find the rate of disappearance of \( N_2O_5 \) from 200 to 400 seconds:\[ \text{Rate}_{N_2O_5} = -\frac{[\text{N}_2\text{O}_5]_{400} - [\text{N}_2\text{O}_5]_{200}}{400\text{s} - 200\text{s}} \]\[ \text{Rate}_{N_2O_5} = -\frac{0.78 - 0.88}{400 - 200} \]\[ \text{Rate}_{N_2O_5} = -\frac{-0.10}{200} \]\[ \text{Rate}_{N_2O_5} = 0.0005 \text{ M/s } \]Thus, the rate of disappearance of \( N_2O_5 \) is \( 0.0005 \text{ M/s } \).**Enter the Coefficient and Exponent:**\[ \text{Rate}_{N_2O_

Answered: Image /qna-images/answer/5d93aabb-ea5e-44c7-aaeb-9609537a6b70.jpg

2N₂O5 (aq) → 4NO₂(aq) + O₂(g) What is the rate of disappearance of N2O5 from 200 to 400 seconds? Time [N₂05] [NO₂] [0₂] 0 1.00 0 0 200 0.88 0.24 0.12 400 0.78 ? ? 600 0.69 0.62 0.16 800 0.61 0.78 0.20 RateN₂05 [?] × 10⁰?¹ M/s = x Coefficient (green) Exponent (yellow) Enter

2N₂O5 (aq) → 4NO₂(aq) + O₂(g) What is the rate of disappearance of N2O5 from 200 to 400 seconds? Time [N₂05] [NO₂] [0₂] 0 1.00 0 0 200 0.88 0.24 0.12 400 0.78 ? ? 600 0.69 0.62 0.16 800 0.61 0.78 0.20 RateN₂05 [?] × 10⁰?¹ M/s = x Coefficient (green) Exponent (yellow) Enter

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

Please answer I really need help
From the data given in the table below, determine the rate law for the following chemical equation. NH4+(aq) + NO2-(aq) → N2(g) + 2 H2O(l) Experiment [NH4+]o [NO2-]o Initial Rate (consumption of NH4+) 1 0.24 0.10 7.2 x 10-6 M/s 2 0.12 0.10 3.6 x 10-6 M/s 3 0.12 0.15 5.4 x 10-6 M/s Select one: a. Rate = k[NH4+][NO2-]2 b. Rate = k[NH4+]2[NO2-] c. Rate = k[NH4+]2 d. Rate =k[NH4+]2[NO2-]2 e. Rate = k[NO2-] f. Rate = k[NO2-]2 g. Rate = k[NH4+] h. Rate = k[NH4+][NO2-]
REIFUNG DISTING Pressure (atm) 1.6 1.4 1.2 1 0.8 0.6 0.4 0.2 0 0 A B 5 10 15 ● · ● 20 25 Time (minutes) 30 35 C D 40 45 00 50
The reaction I (ag) + OCI (ag) → IO¯(aq) + Cl¯(ag) was studied, and the following data were obtained: [I], (mol/L) [OCI¯], (mol/L) Initial Rate (mol/L · s) 0.080 0.18 7.80 x 10- 0.040 0.18 3.90 × 10–2 0.020 0.090 9.80 x 10 -3 0.16 0.090 7.80 x 10–2 What is the rate law? (Use k for the rate constant.) Rate = Calculate the value of the rate constant. k = L/mol · s Calculate the initial rate for an experiment where both I and OCI are initially present at 0.16 mol/L. Rate = mol/L · •S
TIA
Consider the reaction: H2 (g) +I2 (g) → 2 HI (g) A chemist performed an experiment and monitored the concentration of I2 during the course of the reaction. The red line in the graph below represents the results obtained. Which line in the plot would best represent how the concentration of HI changes during the course of the reaction? Time (s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a a b b d d е е Concentration (M)
A gas, AB, decomposes and the volume of B2 produced is measured as a function of time. The data obtained are as follows: time(min) 0 8.3 15.4 19.0 vol(L) 0 4.2 8.6 11.5 What is the average rate of production of B2 for the first 19 min?
2. Suggest method(s) that can be used to measure the rate of reaction of the following reactions. Explain your choices. (There may be more than one method in each of the following reaction.) 5H,O,(aq) + 2MNO, (aq) + 6H¨(aq) → 2Mn²*(aq) + 8H2O(1) + 502(g)
Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, fınd the rate law. 0–H [RCOOH], M [R'OH], M (HA], M Initial Rate, Ml·min' || R-c-o–H 0.35 0.35 0.50 4.60 0.50 + HA - R-Ć+ k2 0.62 0.35 8.14 A- 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 0–H Group 1 Rate = k[RCOOH][R'OH] 0–H 0–H k3 O Rate = k[RCOOH][R'OH][HA] R-C+ A + R -0–H R—С—0—Н Rate = k[RCOOR']/{[RCOOH][R'OH]} k4 0–H R'-o+ A- Rate = k[R'OH] Group 2 H Rate = k[RCOOH] 0–H k5 R—С—0—н R-C-0–R' + H2O + HA R-o+ A- Group 3 H. Step 2 or Step 3 Step 1 or Step 2 Step 1 or Step 3 Step 2 Step 1
Help with the question on the right Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, find the rate law. 0–H (RCOOH), M [R'OHJ, M (HAJ, M Initial Rate, M-min"' - R-C+ k2 R С—0—Н + HA A- 0.35 0.35 0.50 4.60 0.50 0.62 0.35 0.35 8.14 0.81 0.50 10.6 0.35 0.50 0.75 0–H 9.84 Group 1 0–H 0–H k3 Rate = k[RCOOH][R'OH] R-Ć+ A- R 0–H R—С—0—Н + Rate = k[RCOOH][R'OH][HA] k4 0–H R-ó+ A- Group 2 Rate = k[RCOOR']/{[RCOOH][R'OH]} H Rate = k[R'OH] 0–H Rate = k[RCOOH] k5 R- C-0–R' R-C-0–H + H,о + НА R-o+ A- Group 3 Step 2 or Step 3 O Step 1 or Step 2 Step 1 Step 3 Step 2 Step 1
60 QUESTION 13 The following graphs can be used for the questions that follow: 00 B0 00 Seris 1 02 time(min) D2 -D4 y = -0.0358x + 0.1058 Liner (Serive t) -18 time(min) The decomposition reaction of NO 2 is important in atmospheric chemistry. The reaction 2NO 2(g) → 2NO(g) + O 2(g) is second order with respect to NO 2. How can the rate constant be determined? A plot of 1/[NO2] versus time will be linear with a slope of -k. A plot of 1/[NO2] versus time will be linear with a slope of k. A plot of [NO2] versus time will be linear with a slope of -k. A plot of In[NO2] versus time will be linear with a slope of -k. Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air DD F8 F3 F4 F5 F1 %23 24 2 4. 7.
For the reaction: IO3 (aq) + 5 I (aq) + 6 H* (aq) + 3I2 (aq) + 3 H2O (l) the reaction rate of I° (aq) is 2.6 x 10-3 M/s Calculate the rate at which (ac) is formed.