A Tutona Manu CH102 patFle| CArrDetoo002202Coy/utoral Manu Ot002 pofO Gme D Youfube MContentsV HighightQ frase6. A scientist conducts an experiment to determine the rate of NO formation in the reaction:of8ID Fage vewA d alcudV DrawN2g) + O22) → 2NOg). If the initial concentration of N2 was 0.500M and the concentration ofN2 was 0.450M after 0.100 s, what is the rate of NO formation?

6. A scientist conducts an experiment to determine the rate of NO formation in the reaction: Nzg + Ozg) → 2NO). If the initial concentration of N2 was 0.500M and the concentration of N2 was 0.450 M after 0.100 s, what is the rate of NO formation?

6. A scientist conducts an experiment to determine the rate of NO formation in the reaction: Nzg + Ozg) → 2NO). If the initial concentration of N2 was 0.500M and the concentration of N2 was 0.450 M after 0.100 s, what is the rate of NO formation?

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...

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Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 0.445M 1.30M 2.00 × 10¹ M/s 0.445M 0.597M 9.18 × 10³ M/s 1.62M 1.30M 2.65 × 105 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = x10 ロ・ロ

3. The rate equation for the decomposition of N,Os(g) (forming NO2(g)) is: A[NO2]/At = k[N;Os]. The value of k is 5.0 × 104 s-1 for the reaction at a particular temperature. a) Calculate the half-life of N2O5(g) at that temperature. b) How long does it take for [N½O5] to decrease to one tenth of its original value?
Given the following balanced equation, determine the rate of reaction with respect to Cl2]. If the rate of Cl2 loss is 4.24 x 10-2 M/s, what is the rate of NO loss? 2NO(g) + Cl2 (g) → 2NOCI(g) O 1.61 × 102 M/s O 8.48 × 10-² M/s O 1.06 × 10-1 M/s O 4.24 x 102 M/s O 2.12 x 10-² M/s
8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time
For the reaction 203(g) --> 30₂(g), the following mechanism was proposed: step 1: 03(g) --> O₂(g) + O(g) step 2: O(g) + 03(g) --> 2 O₂(g) If step 1 is the slow step, the reaction would be [Select] for 03 and [Select] for 02. If step 2 is the slow step, the reaction would be [Select] for O3 and [Select] for O₂.
For the multi-step reaction A+B → C+D the rate-limiting step is unimolecular, with A as the sole reactant. If [A] and [B] are both 0.175 M, then the rate of reaction is 0.0030 M/s. What is the rate of the reaction if [A] is doubled? rate: Starting with the original concentrations, what is the rate of the reaction if [B] is halved? rate: Starting with the original concentrations, what is the rate of the reaction if [A] and [B] are both increased by a factor of 5? rate: M/s M/s M/s
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
The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH3(g) + 302(g) → 2N2(g) + 6H₂O(A) Suppose the rate of formation of H₂O(A) is 3.0 mol/(Ls). Which of the following statements is true? The rate of consumption of NH3 is 2.0 mol/(L. s). The rate of consumption of O₂ is 2.0 mol/(L. s). The rate of formation of N₂ is 1.3 mol/(Ls). The rate of formation of N₂ is 2.0 mol/(Ls). The rate of consumption of NH3 is 0.50 mol/(L. s).
The activation energy for the following reaction is 125 kJ/mol, and AE for the reaction is -216 kJ/mol. NO₂(g) + CO(g) → NO(g) + CO₂(g) What is the activation energy for the reverse reaction NO(g) + CO₂(g) → NO₂(g) + CO(g) Please enter your answer as a real number only. (The units should be kJ/mol, but leave that off. Just enter a number like 420.3. But don't enter 420.3. Enter the correct answer.)
Last part of this question... An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 → 2NH3. Starting with a closed reactor containing 1.25 mol/L of N2 and 0.35 mol/L of H2, she finds that the H2 concentration has fallen to 0.12 mol/L after 40. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec). 0.0058 You are correct.Your receipt no. is 155-176 Previous Tries What is the average rate of NH3 production for this example? (Enter in mol/liter/sec). 0.0038 You are correct.Your receipt no. is 155-8777 Previous Tries Estimate the N2 concentration after 40 seconds? (Enter in mol/liter).
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4. Given the following balanced equation, determine the rate of reaction with respect to [NOCI]. If the rate of Cl₂ loss is 4.84 × 10-2 M/s, what is the rate of formation of NOCI? 2 NO(g) + Cl2(g) → 2 NOCI(g) A. 4.84 x 10-2 M/s B. 2.42 x 102 M/s C. 1.45 × 10-1 M/s D. 9.68 × 10-2 M/s E. 1.61 × 102 M/s