None The rate of decomposition of N2O5 in CCl4 at 323 K has been studied by monitoring the concentration of N2O5 in the solution.-2 N2O5(9) 4 NO2(g) + O2(g)Initially the concentration of N2O5 is 2.35 M. At 173 minutes, the concentration of N2O5 is reduced to 2.17 M. Calculate the average rate of this reaction in M/min.0.00104X M/minTutorialDid you recall that the average rate of change of a substance is the change in concentration of the substance divided by the time required for that concentration change? Did you recall how to account for theaverage rate of change of reactants versus products? Did you recall how to account for the coefficients of the reactants and products when calculating rates?Submit Answer

Answer: The given balanced chemical equation is:2N2O5(g)→4NO2(g)+O2(g)The rate of reaction is…

Answered: The rate of decomposition of N2O5 in…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 96QRT

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The rate constant, k, at 25 C is 0.27/h for the reaction Pt(NH3)2Cl2(aq) + H2O() [Pt(NH3)2(H2O)Cl]+(aq) + Cl(aq) and the rate equation is Reaction rate = k[Pt(NH3)2C12] Calculate the rate of reaction when the concentration of Pt(NH3)2Cl2 is 0.020 M.
Write a rate law for NO3(g) + O2(g) NO2(g) + O3(g) if measurements show the reaction is first order in nitrogen trioxide and second order in oxygen.
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
A reaction has the following experimental rate equation: Rate = k[A]2[B]. If the concentration of A is doubled and the concentration of B is halved, what happens to the reaction rate?
The reaction between ozone and nitrogen dioxide at 231 K is first-order in both [NO2] and [O3]. 2 NO2(g) + O3(g) N2O5(g) + O2(g) (a) Write the rate equation for the reaction. (b) If the concentration of NO2 is tripled (and [O3] is not changed), what is the change in the reaction rate? (c) What is the effect on reaction rate if the concentration of O3 is halved (with no change in [NO2])?
The rate of a certain reaction is given by the following rate law: = K[N₂]³[03] Use this information to answer the questions below. rate = k What is the eaction order in N₂? What is the reaction order in 03? What is overall reaction order? At a certain concentration of N₂ and O3, the initial rate of reaction is 45.0 M/s. What would the initial rate of the reaction be if the concentration of N₂ were doubled? Round your answer to 3 significant digits. The rate of the reaction is measured to be 8.0 x 103 M/s when [N₂] = 1.5 M and [03] = 0.42 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. k= -3 0 0 0 WO -1 'S S 0
In a reversible reaction between A and B, k1 is the rate constant for the formation of B from A, and k–1 is the rate constant for the formation of A from B. What is the rate equation if both reactions are first order with respect to the reactant? Rate of disappearance of A = k1 [A] – k–1 [B] Rate of disappearance of A = k1 [A] + k–1 [B] Rate of disappearance of A = k–1 [A] + k1 [B] Rate of disappearance of A = (k–1/k1) [A][B] Rate of disappearance of A = k–1 [A] – k1 [B]
Considering the reaction below, which of the following statements is false: 4 NO2(g) + 2 Kl(aq) → 2 KNO3(aq) + 12(g) + 2 NO(g) Rate = K[NO₂]²[KI] Doubling the concentration of NO2 will increase the reaction rate by eight (8) times. The order of the reaction is 1st order with respect to Kl. Doubling the concentration of KI will decrease the reaction time. The order of the reaction is third overall.
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy - 1 E=74.0 kJ/mol. If the rate constant of this reaction is 61. M 387.0 °C? Round your answer to 2 significant digits. - 1 -1 k = M²¹ ₁5² ¹ О •S x10 X - 1 S at 349.0 °C, what will the rate constant be at olo Ar
Given the following balanced equation, determine the rate of reaction with respect to N2. N2(9) + 3H2 (g) → 2NH3 (g) Rate = - 2 1 A[N2] At 1 ΔΗ] Rate = 3 At 2A[N2] Rate = + At A[N2] Rate = At O It is not possible to determine without more information.
The reaction rate for the decomposition of N2O5 to form NO2 and O2 was studied as a function of temperature. The first order reaction rate constants were found to be: T (K) k(s*) 273 7.9 x 107 298 3.5 x 105 308 1.4 x 104 318 5.0 x 104 328 1.5 x 10 3 338 4.9 x 103 What is the Ea for this reaction in kJ/mol? Use Excel to plot the pertinent data and use linear regression to calculate the slope of the line connecting your data. Round your answer to 2 decimal places.
Consider the following reaction: (a) The rate law for this reaction is first order in HBr(g) and first order in O₂(g). What is the rate law for this reaction? Rate = k [HBr(g)] [O₂(g)] O Rate = k [HBr(g)]² [O₂(g)] O Rate = k [HBr(g)] [O₂(g)]² O Rate = k [HBr(g)]² [0₂(g)]² O Rate = k [HBr(g)] [O₂(g)]³ O Rate = k [HBr(g)]4 [0₂(g)] (b) If the rate constant for this reaction at a certain temperature is 11500, what is the reaction rate when [HBr(g)] = 0.00379 M and [O₂(g)] = 0.00876 M? Rate = 4 HBr(g) + O₂(g) → 2 H₂O(g) + 2 Br₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00758 M while the concentration of O₂(g) is 0.00876 M? M/S

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