The rate constant for the reaction of nitrogen with oxygen was determined at four temperatures.N2(g) + O2(g)T(K)2NO(g)k (cm3/molecule⚫s)2507.18 x 10-82751.36 x 10-73002.31 x 10-73253.46 x 10-73rd attemptPart 1 (1 point)Plot these data to calculate the activation energy of the reaction.kJ/molPart 2 (1 point)Plot these data to calculate the frequency factor A for the reaction.cm3/molecules

Step 1: For the given reaction, we are given rate constants at different temperatures. Using that we…

Answered: The rate constant for the reaction of…

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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At 10oC and 50oC the first-order rate constants of a reaction are 9.88 x 10-4 and 9.45 x 10-2 s-1 respectively. What is the activation energy (kJ/mole)? (R = 8.31 J/mole oK). 87.2 78.2 27.8 28.7
но HO HO HO 0 + ½ O, → + H,0 H H но OH ascorbic acid dehydroascorbic acid Vitamin C is oxidized slowly to dehydroascorbic acid by the oxygen in air. It is catalyzed by ions such as Cu*2 and Fe*3. The reaction can be followed by measuring the ultraviolet absorbance at 243 nm. Time (hours) Absorbance (A) 1/A In A - In A 0.75 1.3 -0.29 0.29 1 0.38 2.6 -0.97 0.97 2 0.19 5.3 - 1.7 1.7 3 0.095 11 - 2.4 2.4 29. What is the hybridization of carbon 1 (far left) and carbon 2 (middle) in this hydrocarbon: CH3CH=CH2? (A) sp³, sp (B) sp?, sp? (C) sp³, sp? (D) sp, sp?
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 122.0 °C |1.0 × 108 45.0 °C 1.0 × 10 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E a mol
The variation of the rate constant with temperature for the decomposition of HI(g) to H2(g) and I2(g) is given here. What is the activation energy for the reaction? 2HI(g) ⟶ H2(g) + I2(g)
Consider the following complex reaction: P + 2Q → Products whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [P](M) [Q](M) Rate(M/s) 1 0.100 0.050 2.25 × 10−3 2 0.100 0.150 6.75 × 10−3 3 0.200 0.050 9.00 × 10−3 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law (express your answer to three significant figures), and select the units for k.
Write rate law for the chemical reaction ?
An energy diagram showing two peaks suggests that there are two steps and three transition states in the reaction mechanism. Select one: O True O False Given a reaction with an activation energy of 2.3 x 104 J/mol. The rate constant will increase by a factor of when the reaction temperature is increased from 200 °C to 250 °C. O 2.42 O 2.81 O 1.58 O 1.75 For the complete neutralization reaction between a 1 M strong acid and a 1 M strong base of equal initial volumes that is marked by a temperature rise, the entropy of neutralization is positive (ASn > 0) whereas the Gibbs free energy is negative (AGxn < 0). Select one: O True O False
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 59.0 °C 6.5 x 101 14 163.0 °C |4.2 × 10 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E x10 mol
The following data were collected for a certain reaction of the type A +B → products. Determine the specific rate constant for this reaction. [A]o, mol L-1 [B]o, mol L-1 Initial rate, mol L-1 s-1 Run i 0.200 0.300 2.44 x 10-2 ii 0.200 0.450 2.44 x 10-2 i 0.300 0.450 5.49 x 10-2 O A. 0.610 L mol s-1 B. 0.960 L mol1 s-1 C. 0.271 L mol-1 s-1 D. 0.407 L mol-1 s-1 O E. 0.120 L mol-1 s-1
What amount of time is required for the concentration of A to decrease from 0.800 M to 0.185 M in the zero-order reaction A → B? (k = 0.0567 M*s⁻¹)
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 253.0 °C 7.6×10 ¹0 354.0 °C 5.8 × 10¹1 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. kJ E x10 mol X ? a II Ś

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