Figure 1. Nitrite concentration versus time for the reaction of ammonium ion with nitrite. Tangent lines at t=0 and 75,000 s indicated in red. nitrite concentration (M) NH4 (aq) + NO₂ (aq) N2(g) + 2 H₂O(l) [NO₂ ]0=0.0050 M [NH4*]0=0.100 M 0.005+ 0.004 0.003 0.002- 0.001 0 t=0 s 50000 100000 Time (s) t = 75,000 s 150000 200000 Critical Thinking Questions 1. What is the instantaneous reaction rate at t=0 seconds? 2. What is the instantaneous reaction rate at = 75,000 seconds? 3. What is the average reaction rate over the first 30,000 second time interval?

Figure 1. Nitrite concentration versus time for the reaction of ammonium ion with nitrite. Tangent lines at t=0 and 75,000 s indicated in red. nitrite concentration (M) NH4 (aq) + NO₂ (aq) N2(g) + 2 H₂O(l) [NO₂ ]0=0.0050 M [NH4*]0=0.100 M 0.005+ 0.004 0.003 0.002- 0.001 0 t=0 s 50000 100000 Time (s) t = 75,000 s 150000 200000 Critical Thinking Questions 1. What is the instantaneous reaction rate at t=0 seconds? 2. What is the instantaneous reaction rate at = 75,000 seconds? 3. What is the average reaction rate over the first 30,000 second time interval?

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

Figure 1. Nitrite concentration versus time for the reaction of ammonium ion with nitrite ion (NO₂) = 0.00500 M nitrite concentration (M) 0.005 0.004- 0.003 0.002- 0.0011 0.000- 0 at t=0 s: d(NO₂) dt 50000 at t= 75,000 s: (NH). Critical Thinking Questions 10. What is the rate of reaction at r = 0 s? d(NO₂) di time (s) 1.35 x 10-7 M/s 100000 = 0.100 M 11. What is the rate of reaction at t = 75,000 s? 1.80 × 108 M/s 150000 12. How does the rate of reaction change as (NO₂) decreases? 13. Estimate the value of the rate of reaction at /= 175,000 s. Explain your reasoning.
At 40^0c, H202 (aq) will decompose according to the foll. reaction: 2 H202 (aq) ----2H20(l) +02 (g) The foll. data were collected for the concentration of h202 at various times. Time. [H202] (mol/L) 0. 1.600 3.10*10^4 0.592 6.20*10^4. 0.219 (a) Calculate the average rate of decomposition in H202 between0 and 3.10 * 10^4 s. use this rate to calculate the average rate of production 02 (g) over the same time period. (b) What are these rates for the time period 3.10*10^4 s. to 6.20 *10^4 s.? Rate of H202 decomposition Rate of O2 Production
Consider the reaction in aqueous solution: 3r+ S20g? - 15 + 2 so,2 Under a given set of conditions, the concentration of 13 changes from 0.0 M to 9.3 10 Min 30 seconds Calculate A(SOyat (in molil-s) for this time interval O 97 104 moUL s O 93- 105 molLs O 8.6 10-5 mol/L s O 97x10 mol/L s O 62- 104 molL s
I PREFER TYPEWRITTEN SINCE I HAVE A HARD TIME READING HANDWRITTEN SOLUTIONS. YOU CAN DO IT HANDWRITTEN, AND HOWEVER, IF I DON'T UNDERSTAND YOUR WRITING, I WILL GIVE A DOWNVOTE THANK YOU. PLEASE SKIP TOO IF YOU ALREADY DID THIS.
3. Draw a reaction energy diagram, and label the product (P), reactant (R), transition states (TS1, TS2, etc.), intermediates (INT1, INT2, etc.) and activation energies (AG‡₁, AG 2, etc.) for a reaction with the following criteria: i. A three-step, endothermic reaction; ii. AG3 > 0 but AG₁ AG‡₁ >> AG‡₂. Which species does the structure of the transition state of the rate-determining step resemble?
True or False (6 - 7) 6. It is found for the reaction A + B → C that doubling A while keeping B constant makes the reaction go 8 times faster and doubling B while keeping A constant makes the reaction go 2 times faster. The rate law for this reaction is: rate= k (A][B]* 7. Suppose you were dissolving a metal such as zinc with hydrochloric acid. Particle size of zinc has no effect on the rate of reaction.
Write the balanced reaction that corresponds to the data in graph.
I PREFER TYPEWRITTEN SINCE I HAVE A HARD TIME READING HANDWRITTEN SOLUTIONS. YOU CAN DO IT HANDWRITTEN, AND HOWEVER, IF I DON'T UNDERSTAND YOUR WRITING, I WILL GIVE A DOWNVOTE THANK YOU. PLEASE SKIP TOO IF YOU ALREADY DID THIS.
Consider a reaction taking place at two different temperatures, T₁= 50 K and T₂- 150 K. What is the mathematical expression showing at which temperature the reaction will be faster?
3) Which of the following is NOT true about a catalyst? A.It may be homogeneous B. It speeds up the reverse reaction C. It is consumed D. It speeds up the forward reaction E. it may be heterogeneous
Help, please answer my chemistry question ASAP! It is attached below
Subject-advance chemistry