Consider the following reaction mechanism: Step 1: A3(g) → A2(9) + A(g) Step 2: A3(g) + A(g) → 2A2(g) What is the role of A(g) and what is the overall balanced equation? Periodic Table and Datasheet O A(g) is an intermediate; 2A3(g) + A(g) → 3A2(g) + A(g) O A(g) is a catalyst; 2A3(g) + A(g).→3A2(g) + A(g) O A(g) is an intermediate; 2A3(g) → 3A2(g) O A(g) is a catalyst; 2A3(g) → 3A2(g)

Consider the following reaction mechanism: Step 1: A3(g) → A2(9) + A(g) Step 2: A3(g) + A(g) → 2A2(g) What is the role of A(g) and what is the overall balanced equation? Periodic Table and Datasheet O A(g) is an intermediate; 2A3(g) + A(g) → 3A2(g) + A(g) O A(g) is a catalyst; 2A3(g) + A(g).→3A2(g) + A(g) O A(g) is an intermediate; 2A3(g) → 3A2(g) O A(g) is a catalyst; 2A3(g) → 3A2(g)

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

2C1₂0, (g) → 2Cl₂ (g) +50₂ (g) He fills a reaction vessel with C1₂O5 and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 0.20 0.30 [C₁₂05] 0.0500M 0.0322M 0.0207 M 0.0133M 0.40 0.00858M 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 [C₁₂0₂] k = 0 x10 □・□ X
Consider the combustion of ethylene: C2H4(g)+3O2(g)→2CO2(g)+2H2O(g)C2H4(g)+3O2(g)→2CO2(g)+2H2O(g) Part A: If the concentration of C2H4C2H4 is decreasing at the rate of 3.8×10−2 M/sM/s , what is the rate of change in the concentration of CO2CO2? Express the rate in molarity per second to two significant digits Part B: What is the rate of change in the concentration of H2OH2O? Express the rate in molarity per second to two significant digits. Part C: Consider the following reaction: N2H4(g)+H2(g)→2NH3(g)N2H4(g)+H2(g)→2NH3(g) If the rate of decrease for the partial pressure of N2H4N2H4 in a closed reaction vessel is 76 torr/h, what is the rate of change for the partial pressure of NH3NH3 in the same vessel? Express the rate in torrs per hour to two significant digits. Part D: What is the rate of change of total pressure in the vessel during the reaction? Express the rate in torrs per hour to two significant digits.
A flask is charged with 0.140 mol of A and allowed to react to form B according to the following hypothetical gas-phase reaction. A(g) → B(g) The following data are collected. Os 0 40 S 0.072 80 s 0.025 120 s 0.014 (a) Calculate the number of moles of B at each time in the table. 160 s 0.013 0 - 40 s 0.0018 40 - 80 s 0.000625 80 - 120 s 0.00035 120 - 160 mol/s 0.000325 times (s) mol mol x mol x mol moles of A X mol mol/s mol/s 0 (b) Calculate the average rate of disappearance of A for each 40 s interval, in units of mol/s. mol/s 40 mol/s 80 120 0.140 0.068 0.043 0.029 160 0.016
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)
(b) Quantities of chemicals, expressed in moles, can be used to find the formula of a compound, to establish an equation and to determine reacting masses. A compound contains 72% magnesium and 28% nitrogen. What is its empirical formula? ( 2) 2. A student investigates the rate of reaction between lumps of calcium carbonate and dilute hydrochloric acid using the apparatus shown. CaCo3(s) + 2HCI (aq) CaCI 2(aq) + CO2(g) + H2O(I) The calcium carbonate was in excess. gas syringe lumps of calcium carbonate dilute hydrochloric acid
Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO₂(g)] [03(g)] Rate = k [NO₂(g)]² [03(g)] Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(g)] (b) If the rate constant for this reaction at a certain temperature is 97900, what is the reaction rate when [NO₂(g)] = 0.587 M and [03(9)] = 1.40 M? Rate = 2 NO₂(g) + 03(9) → N₂O5(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.17 M while the concentration of O3(g) is 1.40 M? M/S
Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) OO H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) +1-(aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?
If methylisonitrile is placed in a sealed quartz tube and heated in a tube furnace, it isomerizes to acetonitrile according to the reaction below: CH3NC (g) → CH3CN (g) The sealed tube initially contains 0.200 mol of methylisonitrile and zero moles of acetonitrile. After about 25 minutes of heating, there is 0.108 mol of methylisonitrile remaining in the tube. Please calculate the average rate of decomposition of methyisonitrile during this 25 min. period. Question 3 options: A) 3.7×10-3 mol/min B) 0.092 mol/min C) 4.3×10-3 mol/min D) 2.3 mol/min E) 0.54 mol/min
The following reaction occurs in your car's exhaust system catalytic converter:Heat + 2CO + O2 + Pt → 2CO2 + PtWhat is the catalyst?
Assume that the formation of nitrogen dioxide, 2 NO(g) + 02(g) – 2 NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad О Help Greek - rate=k•[NO]2.[02] rate=k*[NO]^2*[O_2] Correct. (b) A sample of air at a certain temperature is contaminated with 1.9 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. If not, repeat your answer from above. (Rate expressions take the general form: rate = k . [A]ª . [B]b. Use k' for the new rate constant as needed.) chemPad O Help Greek - rate=k':[NO]2 rate=k*[NO]^2 Correct. (c) Under the conditions described in (b), the half-life of the reaction has been estimated to be 6.7x103 min. What would the half-life be if the initial concentration of NO were 12.4 ppm? 4.0 |1030192 X min Supporting Materials Periodic Table Constants and E Supplemental Data
Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.
The following represents the effect of time on the concentration during a reaction. The upper line represents a reactant concentration and the lower line the concentration of a product. Which of the following statements is not correct? Concentration B C Time → O Between points A and D the reactant concentration is decreasing. O Between points B and C the product concentration is increasing. At point D the rate of the forward and reverse reactions are the same. O At point C the rate of product breakdown equals that of reactant consumption.