### General Chemistry 4th Edition ### McQuarrie • Rock • Gallogly ### University Science Books presented by Macmillan Learning---### Reaction AnalysisThe reaction:\[ \text{C}_4\text{H}_8 (g) \longrightarrow 2\text{C}_2\text{H}_4 (g) \]is characterized by an activation energy of 262 kJ/mol. At a temperature of 600.0 K, the rate constant, \( k \), is \( 6.1 \times 10^{-8} \, \text{s}^{-1} \). The question posed is to determine the value of the rate constant at 750.0 K.A student attempted to solve the problem and submitted the following answer for the rate constant (\( k \)):\[ k = 1.34 \times 10^3 \, \text{s}^{-1} \]However, this answer is marked as incorrect.---To solve this problem correctly, one could use the Arrhenius equation:\[ k = A e^{-\frac{E_a}{RT}} \]where:- \( k \) is the rate constant,- \( A \) is the pre-exponential factor or frequency factor,- \( E_a \) is the activation energy,- \( R \) is the universal gas constant (8.314 J/mol·K),- \( T \) is the temperature in Kelvin.By substituting the given values of activation energy (\( E_a = 262 \, \text{kJ/mol} \)), and the temperatures (initial \( T_1 = 600.0 \, \text{K} \) and final \( T_2 = 750.0 \, \text{K} \)), we can apply the two-point form of Arrhenius equation:\[ \ln \left(\frac{k_2}{k_1}\right) = \frac{E_a}{R} \left(\frac{1}{T_1} - \frac{1}{T_2}\right) \]Given:- \( k_1 = 6.1 \times 10^{-8} \, \text{s}^{-1} \)- \( E_a = 262 \, \text{kJ/mol} = 262000 \, \text{J/mol} \)After solving for

Answered: Image /qna-images/answer/c4ab7cbb-53e5-4210-8377-3b9ab41f6b2b.jpg

The reaction C,H;(g) → 2 C,H, (g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-1. What is the value of the rate constant at 750.0 K? k = 1.34 х103 s-1 Incorrect

The reaction C,H;(g) → 2 C,H, (g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-1. What is the value of the rate constant at 750.0 K? k = 1.34 х103 s-1 Incorrect

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

A certain reaction has a ΔH = -75 kJ and an activation energy of 40 kJ. A catalyst is found that lowers the activation energy of the forward reaction by 15 kJ. What is the activation energy of the reverse reaction in the presence of this same catalyst?
The reaction CHg (g)2C₂H₂(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 x 10-8 s-¹. What is the value of the rate constant 790.0 K? k = 2.81 Incorrect S-1
A certain reaction has an activation energy of 49.24 kJ/mol. At what Kelvin temperature will the reaction proceed 6.50 times faster than it did at 299 K? 379 T = K Incorrect
A certain reaction has an activation energy of 39.57 kJ/mol. At what Kelvin temperature will the reaction proceed 5.50 times faster than it did at 337 K? T = K
Consider the reaction below at 100oC T2U (g) ⟶⟶ 2 T (g) + U (g) When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, which is the numerical value of the specific-rate constant, k, for this reaction?
A certain reaction has an activation energy of 60.65 kJ/mol. At what Kelvin temperature will the reaction proceed 3.50 times faster than it did at 357 K? T = K
20
1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. (i) H2(g) + NO(g) → H20(g) + N(g) (ii) N(g) + NO(g) → N2(g) + O(g) (iii) O(g) + H2(g) → H20(g) Ea = 436 kJ AH = -491 kJ Ea = 625 kJ AH = -312 kJ Ea = 1690 kJ AH = +131 kJ a. What is the AH for the overall reaction? Overall, is it endothermic or exothermic? b. Draw the potential energy diagram for the reaction. Assume the potential energy of the reactants was 1400 kJ1) 2600 2400 2200 2000 1800 1600 1400 1200 1000 800 600 400 200 Reaction Progress c. What is Ea for the overall reaction? You must calculate this from the potential energy diagram. Potential Energy (kJ)
Will the rate constant (usually symbolized by k) for a particular reaction change when concentrations of reactants are changed? How about when the temperature is changed?
The reaction C,H,(g) → 2C,H¸(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant,k, is 6.1 x 10s. What is the value of the rate constant S at 850.0 K? 1.9 x102 k = Incorrect
Consider the reaction below at 100°C. T2U (g) -> 2T (g) + U (g) When [T2U], is 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U], is 0.144 M, the reaction rate is 3.09 x 10-3 M/s. What are the units for the specific-rate constant, k? What are the units of the specific-rate constant, k A. L2 mol1 s-1 B. s-1 C. mol L-1 s-1 D. L mol-1 s-1
11. The elementary steps for the catalyzed decomposition of dinitrogen monoxide are shown below. Step 1: N20(g) + NO(g) → N2(g) + NO2(g) (slow) Step 2: NO2(g) → NO(g) + 1/2 O2(g) (fast) Which of the following statements is/are CORRECT? The overall balanced reaction is N20(g) → N2(g) + 1/2 O2(g). 2. NO2(g) is a catalyst for the reaction. 3. NO(g) is a reaction intermediate. 1. a) 1 only c) 3 only d) 1 and 3 e) 1, 2, and 3 f) none of the above b) 2 only