A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0°C. What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol?2.85 x 104 s-1O 1.36 x 102 s1O 9.56 x 103 s1O 4.33 x 1087 s-1O 576 s1SubmitRequest Answer

Answered: Image /qna-images/answer/8f3b3e76-f64c-4e1b-a1d7-69f002e30f99.jpg

A particular first-order reaction has a rate constant of 1.35 x 102 s1 at 25.0°C. What is the magnitude of k at 95.0°C if E, = 55.5 kJ/mol? O 2.85 x 104 s1 O 1.36 x 102 s 9.56 x 103 s1 O 4.33 x 1087 s1 O 576 s1 Submit Request Answer

A particular first-order reaction has a rate constant of 1.35 x 102 s1 at 25.0°C. What is the magnitude of k at 95.0°C if E, = 55.5 kJ/mol? O 2.85 x 104 s1 O 1.36 x 102 s 9.56 x 103 s1 O 4.33 x 1087 s1 O 576 s1 Submit Request Answer

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter30: Kinetic Methods Of Analysis

Section: Chapter Questions

Problem 30.7QAP

See similar textbooks

Related questions

Q: N2O5 is used as a source of NO2 in chemical reactions. The compound decomposes in a first order…

A: Given: Initial concentration of N2O5 = 0.400 M Final concentration of N2O5 = 0.025 M Time = 120 s

Q: The reaction O2(g) + 2 NO(g) 2 NO2(g) was studied at a certain temperature with the following…

A: For any general reaction Rate law is an expression which show the relation between the concentration…

Q: The reaction C4H8(g)⟶2C2H4(g)C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol.262…

A: The Arrhenius equation is shown below: lnk2k1=-EaR1T2-1T1 Here, Ea is the activation energy, k1 is…

Q: The reaction, 2 A2X4(g) → 2 A2X3(g) + X2(g), was found to be first order. The rate law,…

A: In this question, we will see the rate law equation for the given first order reaction. You can see…

Q: 34. Given the initial rate data for the reaction A + B C, determine the rate expression for the…

A: A + B ---> C ∆C/∆t = K [A]m[B]n .............(*) K= rate constant m= order with respect to A . n=…

Q: The rate law for the reaction A2Bm2 (aq) + 2A(aq) + 2D(aq) -> D2 (aq) + 2A2Bm (aq) is rate =…

A: over all order of a reaction gives an indication of how changing the concentration of reactants will…

Q: The relative initial rates of the reaction A2 + B2 → products in vessels (a)-(d) are 1:2:4:8.…

A: Given : The relative rate of initial rates in vessels a-d = 1 : 2 : 4 : 8

Q: SO2CI2 decomposes in the gas phase by the reaction SO2Cl2(g) → SO2(g) + Cl2(g) The reaction is first…

A: The reaction taking place is given as, => SO2Cl2 (g) ------> SO2 (g) + Cl2 (g) Given :…

Q: Oxidation of thallium by cerium ion can be carried out in laboratory according to the following…

A: The order of a reaction is calculated by the slowest step of the reaction which is also known as the…

Q: The reaction; 2A + B→C From the following data collected at temperature, 25°C. Determine the rate…

Q: The activation energy for the following first-order reaction is 102 kJ/mol. N205(G) – 2NO2(9) +…

Q: (Q81) Hydrogen peroxide decomposes to water and oxygen gas is a first order reaction: 2 H202 (aq)…

Q: Consider the reaction: NO2 + O3 -->NO3 + O2 Based on the kinetic data given below, the partial order…

Q: 2. The dimerization of C4H4 was observed and yielded the data shown below. Time (s) [C.Ha] (M) 1.00…

A: The order of the reaction can be find out by graphical method. The straight line from the graph can…

Q: The reaction O2(g) + 2 NO(g) 2 NO2(g) was studied at a certain temperature with the following…

A: The rate law for the reaction can be written as: rate=kO2gxNOgy ......(1) Here, x is the order with…

Q: Do not include spaces or multiplication signs in your answer. Determine the rate law for this…

Q: A + B yields P [A] (M) [B](M) 0.763 Initial Rate (M/s) 0.247 2.83 0.247 2.289 25.47 0.494 0.763 2.83…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Initial Rate Experiment # [H;SeO3] (M) [] (M) [H*] (M) (M/s) 0.0025 0.015 0.015 9.85 x 107 0.0025…

Q: 1. For the reaction between hydrogen gas and fluorine gas the following data was collected H2(g) +…

Q: What graph will demonstrate that experimental concentration data fit a second-order reaction?…

A: Note: As per our guidelines, we are supposed to answer only one question when multiple questions are…

Q: A particular first-order reaction has a rate constant of 1.35 × 102 s−1 at 25.0 ∘C. What is the…

A: Arrhenius equation is a mathematical expression containing various rate dependent terms such as…

Q: The rate constant of a first-order reaction is 4.60 x 104/s at 350°C. If the activation energy is…

A: Given that: Rate constant (k1) = 4.60×10-4 s-1 Temperature (T1) = 350°C = 623K Activation energy…

Q: Acids are common catalysts for many biochemical reactions. The following 3-step mechanism has been…

A: Slow step is always at the rate determining step in a multi step mechanism. Rate law and the Order…

Q: The reaction A (g) + (B) g → C(g) has a rate law that is rate = 5.43 x 10-2 (A][B]. The reaction…

A: Order of the reaction is defined as the sum of the exponential power of all the concentration terms…

Q: II. Rate Law The following data were collected experimentally from the following reaction. 2 NO + 2…

Q: Determine the rate law for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H20(g) Using the method of…

A: Determination of rate law for an reaction

Q: Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A]2 where k=2.90 ×10-2…

A: For the given reaction, Rate law has been defined as : Rate = k [A]2 From…

Q: The half-life for a first order reaction A P at 600 K is 24 seconds. How many seconds are needed for…

Q: The following data were obtained for the reaction of NO with O2. Concentrations are in molecules/cm…

Q: 15.) The rate constant for the following second-order reaction is 0.80/(M·s) at 10°C.…

A: The reaction given is => 2 NOBr (g) → 2 NO (g) + Br2(g) Given ; Order of reaction = 2 Initial…

Q: The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the…

Q: What is the rate for the second order reaction A → Products when [A] = 0.451 M? (k = 0.761 M⁻¹s⁻¹)?

A: For any reaction, the rate of reaction depends on the concentration of reactants only And since the…

Q: The following data were measured for the reaction 2 NO(g) + Br2(g) ---> 2 NOBr(g) Experiment [NO]…

Q: ee Periodic Table Order of the reaction with respect to NO2: Order of the reaction with…

A: Order of reaction is defined as the sum of power of concentration of reactants in the rate law…

Q: A certain reaction is second order in N₂ and second order in H₂. Use this information to complete…

A: Reaction is of second order with respect to N2 and second order with respect to H2.

Q: For the following reaction A → B P0 (A)= 360…

A: The question is based on the concept of chemical kinetics. we have to calculate order of the…

Q: A particular first-order reaction has a rate constant of 1.35 × 102 s−1 at 25.0 ∘C. What is the…

A: According to the clausius clapeyron equation, ln(K2 / K1) = (-Ea /R) X (1/T2 - 1/T1) where K2 =…

Q: A particular first order reaction has a rate constant of 7.35X 10E4 s-1 at 25.0 degrees Celsius what…

Q: The rate constant for this first-order reaction is 0.0125 s−10.0125⁢ s−1 at 300 °C.…

A: We know that, the first order rate expression as follows --- ln a(a-x) = kt ............(i) Where,…

Q: The reaction 2 NO(g) + O₂(g)-> 2 NO₂(g) proceeds through the following mechanism: (a) The second…

A: The relation between the concentration of the reactants and the rate of reaction is expressed by the…

Q: 13. The rate of the reaction NO2(8) + CO(g) NO(8) + CO2(g) depends only on the concentration of NO2…

A: we need to find the value of k according to the given data

Q: A + B → products Initial concentration (mol/L) Initial rate Experiment A B (mol L-¹ min¹¹) 1 1.50…

A: Rate of reaction is change in concentration with respect to time. aA + bB →cC For above reaction…

Q: The reaction described by the equation 0,(g) + NO(g) - 0,(g) + NO,(g) has, at 310 K, the rate law…

Q: The data in the table below were obtained for the reaction: 2 CIO2 (aq) + 2 OH (aq) → CIO3 (aq) +…

A: The given reaction is as follows: 2ClO2(aq) +2OH-(aq) → ClO3-(aq) +ClO2-(aq) + H2O(l) Let the order…

Q: A proposed mechanism for the reaction is: - Step 1: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) Step 2: N₂O(g)…

A: Rate Law :- The rate law of a chemical reaction is an expression that provides a relationship…

Q: At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 10-3 min…

Q: What is the value of the Arrhenius activation energy (E) for a chemical reaction if the rate…

A: The details solution for this is provided below in attach image.

Q: Determine the rate law for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H20(g) Using the method of…

Q: Nitrite ion reacts with ozone in aqueous solution, producing nitrate ion and oxygen: NO−2 (aq)+O3…

A: ReactionNO2-(aq) + O3(g) → NO3-(aq) + O2 (g)Average rate (0-100μs)r = -dcadt = -(9.93 x10-3-1.13…

Question

A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0°C. What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol?
2.85 x 104 s-1
O 1.36 x 102 s1
O 9.56 x 103 s1
O 4.33 x 1087 s-1
O 576 s1
Submit
Request Answer

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Ammonium cyanate, NH4NCO, rearranges in water to give urea, (NH2)2CO. NH4NCO(aq) (NH2)2CO(aq) Using the data in the table: (a) Decide whether the reaction is first-order or second-order. (b) Calculate k for this reaction. (c) Calculate the half-life of ammonium cyanate under these conditions. (d) Calculate the concentration of NH4NCO after 12.0 hours.
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
Ammonium cyanate, NH4NCO, in water rearranges to produce urea, a common fertilizer, (NH2)2CO: NH4NCO(aq)(NH2)2CO(aq) The rearrangement is a second-order reaction. It takes 11.6 h for the concentration of NH4NCO to go from 0.250 M to 0.0841 M. (a) What is k for the reaction? (b) What is the half-life of the reaction when NH4NCO is 0.100 M? (c) How long will it take to rearrange 39% of a 0.450 M solution? (d) How fast is a 0.839 M solution being changed to urea?
11.51 Peroxyacetyl nitrate (PAN) has the chemical formula CtHjNOj and is an important lung irritant in photochemical smog. An experiment to determine the decomposition kinetics of PAN gave the data below. Determine the order of reaction and calculate the rate constant for the decomposition of PAN. Time, t (min) Partial Pressure of PAN (torr) 0.0 2.00 X 10~’ 10.0 1.61 X 10~} 20.0 1.30 X 10_J 30.0 1.04 X 10"’ 40.0 8.41 X 10-4 50.0 6.77 x 10-4 60.0 5.45 X 10-4
Consider the following representation of the reaction 2NO2(g) 2NO(g) + O2(g). Determine the time for the final representation above if the reaction is a. first order b. second order c. zero order
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.
Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2) by reaction in the gas phase. The following pressure data were obtained when a sample containing 5.00 102 mol sulfuryl chloride was heated to 600. K in a 5.00 101-L container. Time (hours): 0.00 1.00 2.00 4.00 8.00 16.00 PSO2Cl2(atm): 4.93 4.26 3.52 2.53 1.30 0.34 Defining the rate as [SO2Cl2]t, a. determine the value of the rate constant for the decomposition of sulfuryl chloride at 600. K. b. what is the half-life of the reaction? c. what fraction of the sulfuryl chloride remains after 20.0 h?
The rate of the reaction NO2(g)+CO(g)NO(g)+CO2(g) depends only on the concentration of nitrogen dioxide below 225C. At a temperature below 225C, the following data were collected: Time(s) [NO2](mol/L) 0 0.500 1.20 103 0.444 3.00 103 0.381 4.50 103 0.340 9.00 103 0.250 1.80 104 0.174 Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO2] at 2.70 104 s after the start of the reaction.
11.34 Rate data were obtained at 25°C for the following reaction. What is the rate law expression for this reaction? A + 2B — C + 2D Expt Initial [A] (mol L-’) Initial [B] (mol L_1) Initial Rate ofFormation of C (mol L-1 min-1) 1 0.10 0.10 3.0 X 10~4 2 0.30 0.30 9.0 X 10"4 3 0.10 0.30 3.0 X 10~4 4 0.20 0.40 6.0 X 10"4
For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (a) Rate = k [X][Y][Zl, (b) Rate = k [X]-[Y]1/2[Z], (c) Rate = k [X]L5[Y]-1, (d) Rate = k [X]/[Y]2
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.