### Reaction Rate Calculation ExerciseConsider the following chemical reaction:\[2\text{NH}_3 (g) \rightarrow \text{N}_2 (g) + 3\text{H}_2 (g)\]At a certain temperature, the reaction follows this rate law equation:\[\text{rate} = (0.0581 \, \text{M}^{-1} \cdot \text{s}^{-1})[\text{NH}_3]^2\]#### Problem Statement:Suppose a vessel contains NH3 at an initial concentration of 1.39 M. Calculate the concentration of NH3 in the vessel after 70.0 seconds. Assume that no other reaction is occurring in the system. Please round your answer to 2 significant digits.#### Sample Calculation:1. Given the initial concentration of \(\text{NH}_3 = 1.39 \, \text{M}\)2. Time \(\Delta t = 70.0 \, \text{s}\)3. Using the rate law to find the change in concentration over time.#### Step-by-Step Solution:(Note: The actual solution steps are not provided in the image. These can include integrating the rate law, applying initial conditions, and solving for the final concentration.)##### Instructions for Answer Submission:Enter your answer in the provided textbox; ensure it is rounded to two significant digits.\[ \boxed{ \, \text{M} \,} \]You may use the calculator tools provided to check your calculations.

The equation for the dissociation of NH3 is shown below: The second order of the reaction can be…

Consider this reaction: 2NH3 (g) → N, (g) + 3H, (g) At a certain temperature it obeys this rate law. [NH, -1 rate = (0.0581 M s. Suppose a vessel contains NH, at a concentration of 1.39M. Calculate the concentration of NH, in the vessel 70.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

Consider this reaction: 2NH3 (g) → N, (g) + 3H, (g) At a certain temperature it obeys this rate law. [NH, -1 rate = (0.0581 M s. Suppose a vessel contains NH, at a concentration of 1.39M. Calculate the concentration of NH, in the vessel 70.0 seconds later. 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

Measuring total pressure is a convenient way to monitor gas reaction: 2NOCl(g) → 2NO(g) + Cl2(g). The rate of the reaction depends on the concentration of the reactant, which is proportional to the partial pressure of the reactant. Derive a relation connecting its velocity above reaction with initial pressure, P0, and total pressure, Pt, at time t.(Hint: Assume the reaction is 2nd order. Make a table with initial (t0) and final values (t) of the moles of NOCl, NO, and Cl2, and construct the ideal gas equations for both cases. Use the ideal gas equation for t0 so that calculate the initial concentration of NOCl and substitute this value into the equation of ideal gases for t)
8 H chemPad H XX LE # Supporting Materials Periodic Table Additional Materials W 17 - Su2... → Help Greek Constants and W The reaction of fluorine and chlorine dioxide, shown below, is first order with respect to fluorine and first order with respect to chlorine dioxide. Write the rate law for this reaction. (Rate expressions take the general form: rate = k. [A]a. [B]b.) F₂(g) + 2 CIO₂ (g) → 2 FCIO₂(g) Factors G b * webassign.net 8 Supplemental Data L a ▸ G
The synthesis of ammonia obeys the following reaction: N2(g) + 3H2(g) → 2 NH3(g) N2(g) concentration measurements were taken at different times and plotted. 1) What is the average reaction rate of NH3(g) between 0 and 3 hours? (Attention, the graph is in "hour" and we want a speed in "mole/L s") 2) What is the instantaneous rate of reaction of NH3(g) at the 1st hour? 3) What is the general speed between 0 and 3 hours?
Only typed solution.
Consider the reaction below at 100oC T2U (g) ⟶⟶ 2 T (g) + U (g) When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, A. Which is the rate law of this reaction? B. which is the numerical value of the specific-rate constant, k, for this reaction? C. Which are the units for the specific rate constant, K? D. At whic rate is T generaten when [T2U] is 0. 111 M? E. if given an initial reactant concentration [T2U]o = 0.250 M, what is [T] after 15 minutes have elapsed?
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.
Answer in two significant digits, please!
The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?
Consider the mechanism. O3 + NO, – NO, + O, NO, + NO, – N,O5 slow fast O, + 2 NO, – 0, + N,O5 Identify the rate law for the overall reaction based on the mechanism. rate = k[O,||NO,? rate = k[O3] rate = k[O3][NO,1 rate = k[NO,? k[NO, ][NO3] rate =
For the simple decomposition reaction: AB(g) A(g) + B(g), the rate = k{AB}? ({ = [) and k = 0.78 1/M•s. How long (in seconds) will it take for the concentration of AB to reach one-third of its initial concentration of 1.07? Enter to 2 decimal places.