### Reaction Rate and Concentration CalculationAt a certain temperature, the rate of this reaction is first order in \( \text{NH}_3 \) with a rate constant of \( 1.22 \ s^{-1} \):\[2\text{NH}_3 \ (g) \rightarrow \text{N}_2 \ (g) + 3\text{H}_2 \ (g)\]Suppose a vessel contains \( \text{NH}_3 \) at a concentration of \( 0.450 \ M \). Calculate the concentration of \( \text{NH}_3 \) in the vessel \( 0.860 \) seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.____\(\boxed{\phantom{0}M}\) \[\checkmark_{x10}\]**Explanation:**1. **Identify the Reaction Order and Rate Constant:** - The reaction is first order in \( \text{NH}_3 \) (ammonia). - The rate constant \( k \) is \( 1.22 \ s^{-1} \).2. **Initial Concentration:** - Initial concentration of \( \text{NH}_3 \) is \( [\text{NH}_3]_0 = 0.450 \ M \).3. **Use the First Order Reaction Formula:** - The formula for first-order reactions is: \[ [\text{NH}_3] = [\text{NH}_3]_0 e^{-kt} \]4. **Substitute the Given Values:** - Time \( t \) is \( 0.860 \) seconds. - Substitute into the formula: \[ [\text{NH}_3] = 0.450 \ M \times e^{-1.22 \times 0.860} \]5. **Calculate:** - Calculate the exponent: \[ -1.22 \times 0.860 \approx -1.0492 \] - Calculate \( e^{-1.0492} \): \[ e^{-1.0492} \approx 0.350 \] - Final concentration: \[ [\text{NH}_3] \approx 0.450 \ M

Given: The rate constant of the reaction, (K)=1.22S-1. The initial concentration of NH3, [A0]=0.450…

At a certain temperature the rate of this reaction is first order in NH, with a rate constant of 1.22 s : 2NH; (g) → N, (3) + 3H, (2) Suppose a vessel contains NH, at a concentration of 0.450M. Calculate the concentration of NH, in the vessel 0.860 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. ?

At a certain temperature the rate of this reaction is first order in NH, with a rate constant of 1.22 s : 2NH; (g) → N, (3) + 3H, (2) Suppose a vessel contains NH, at a concentration of 0.450M. Calculate the concentration of NH, in the vessel 0.860 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

At a certain temperature the rate of this reaction is second order in SO, with a rate constant of 4.02 M 's': 2S0, (g) → 2S0, (g) +0,(g) Suppose a vessel contains SO , at a concentration of 0.790 M. Calculate how long it takes for the concentration of SO, to decrease to 0.103 M. You may assume no other reaction is important. Round your answer to 2 significant digits.
-1 At a certain temperature the rate of this reaction is second order in SO, with a rate constant of 74.4M - 1 S. : 280; (g) →2S0, (g) + 02 (g) Suppose a vessel contains SO, at a concentration of 0.340M. Calculate how long it takes for the concentration of SO, to decrease to 0.0408M. You may assume no other reaction is important. Round your answer to 2 significant digits.
Consider this reaction: 2H, РО, (ад) — Р,0; (аq)+3н,0 (ад) At a certain temperature it obeys this rate law. = (0.749 M ¿PO, •S Suppose a vessel contains H,PO, at a concentration of 0.660M. Calculate how long it takes for the concentration of H,PO, to decrease by 83.0%. You may 4 assume no other reaction is important. Round your answer to 2 significant digits. S ?
At a certain temperature the rate of this reaction is first order in NH3 with a rate constant of 0.354 s : 2NH3(g) → N₂ (g) + 3H₂(g) Suppose a vessel contains NH3 at a concentration of 0.380M. Calculate the concentration of NH3 in the vessel 2.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X
At a certain temperature the rate of this reaction is second order in HI with a rate constant of 0.22M¹s¹: 2 HI(g) → H₂(g) + 1₂ (8) Suppose a vessel contains HI at a concentration of 0.910M. Calculate how long it takes for the concentration of HI to decrease to 0.064 M. You may assume no other reaction is important. Round your answer to 2 significant digits. 0.9 X 圖图

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0021 M-s 2NH, (g) - N, (g) + 3H₂(g) Suppose a 5.0 L 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 the correct number of significant digits.
Consider this reaction: →H2CO3aq+H2OaqCO2aq At a certain temperature it obeys this rate law.rate =·0.0579M−1s−1H2CO32 Suppose a vessel contains H2CO3 at a concentration of 0.820M. Calculate the concentration of H2CO3 in the vessel 280.seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M
At a certain temperature the rate of this reaction is second order in SO, with a rate constant of 0.0151 M .s ': 2S0, (g) → 2S0, (g) +0, (g) Suppose a vessel contains SO, at a concentration of 0.430M. Calculate the concentration of SO, in the vessel 580. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. ?
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0096 M's: 2 NH, (g) N, (g) +3 H, (e) Suppose a 2.0 L flask is charged under these conditions with 150, mmol of ammonia. How much is left 2.0 s later? 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. 8 D.P Consider this reaction: 250, ) - 2S0, (g)+0, (g) At a certain temperature it obeys this rate rate - (0.067 M)[so, Suppose a vessel contains SO, at a concentration of 0.28OM. Calculate how long it takes for the concentration of SO, to decrease to 0.025M. You may assume no other reaction is important. Round your answer to 2 significant digits. Djo X
At a certain temperature the rate of this reaction is first order in H,CO, with a rate constant of 0.394 s H,CO, (aq) – HyO(@q) +D, lạy) Suppose a vessel contains H,CO, at a concentration of 0.780M. Calculate the concentration of H₂CO, in the vessel 3.30 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X
At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.75Ms H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.130M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.0286 M. You may assume no other reaction is important. Round your answer to 2 significant digits. X ? S
23 II. An experiment followed the decomposition. of nitregen dioxide to nitregen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |[NO₂] (M) 0.0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M G 2 XX 6.5 Hoa X019 201 2(x) = 2 (1.86) (3 (9)