A chemistry graduate student is studying the rate of this reaction:2N₂O5 (g) → 2N₂O4 (g) + O₂(g)She fills a reaction vessel with N₂O5 and measures its concentration as the reaction proceeds:time(seconds)01.02.03.04.0[N₂O5]0.500 M0.311 M0.193 M0.120M0.0744 MUse this data to answer the following questions.Write the rate law for this reaction.Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also besure your answer has the correct unit symbol.rate= k0x10ロ･ロX00S

Answered: Image /qna-images/answer/fb2cbb90-111f-4970-b7de-6fe60e455084.jpg

A chemistry graduate student is studying the rate of this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) She fills a reaction vessel with N₂O5 and measures its concentration as the reaction proceeds: time (seconds) [₂05] 0 1.0 2.0 3.0 0.500M 0.311 M 0.193 M 0.120M 4.0 0.0744 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k= 0 ロ･ロ X 5

A chemistry graduate student is studying the rate of this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) She fills a reaction vessel with N₂O5 and measures its concentration as the reaction proceeds: time (seconds) [₂05] 0 1.0 2.0 3.0 0.500M 0.311 M 0.193 M 0.120M 4.0 0.0744 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k= 0 ロ･ロ X 5

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

Consider the same reaction carried out two more times, both at the same condition(including concentration and temperature), but where the volume of the reaction is doubled in the second reaction. Since the concentrations are the same in both cases, the 2nd has twice the quantity of gases. How do those two rates of reaction compare to each other? Please compare using units of moles/(L•min) and separately using units of moles/min.
Study the reactions. I. N2 (g) + O2(g) → 2NO(g) II. CO(g) + 02(g) → 2CO2 (g) III. Na(s) + HCI(1) → 2NACI(aq) + H2(g) What factor would only affect the rate of the third reaction? the pressure of the reactants the temperature of the reactants the concentration of the reactants the surface area of the reactants
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
22. The rate of a reaction depends on many factors such as the concentration of the reactants. Which of the following explains why an increase in the concentration of reactants affects the rate of reaction? The reactants move faster. The collisions increase between the reactants. There are fewer molecules present. The activation energy is lowered.
The synthesis of ammonia obeys the following reaction: N2(g) + 3H2(g) → 2 NH3(g) What is the average reaction rate of H2(g) between the 2nd and the 9th hour. (Attention, the graph is in "hour" and we want a speed in "mole/L·s".) What is the instantaneous reaction rate of H2(g) at the 3rd hour. What is the reaction rate between the 2nd and the 9th hour.
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)
1a
Can someone please help with question 7
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
A general reaction written as 2A + 2B → C + 2D is studied and yields the following data. [A]0 [B]0 Initial Δ[C]/Δt 0.100 M 0.100 M 4.00 × 10–5 mol/L • s 0.200 M 0.100 M 4.00 × 10–5 mol/L • s 0.100 M 0.200 M 8.00 × 10–5 mol/L • s What is the overall order of the reaction? Question 8 options: A) 0 B) 2 C) 3 D) 4 E) 1
Given the following balanced equation, determine the rate of reaction with respect to [NOCI]. If the rate of Cl₂ loss is 4.84 x 10-2 M/s, what is the rate of loss of NO? 2 NO(g) + Cl2(g) 2 NOCI(g) 4.84 x 10-² M/s 2.42 x 10-² M/s 1.45 x 10-1 M/s 9.68 x 10-2 M/s 1.61 x 10-² M/s