Chemical kinetics Questions and Answers

A certain reaction has an activation energy of 35.30 kJ/mol.
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A certain reaction has an activation energy of 35.30 kJ/mol. At what Kelvin temperature will the reaction proceed 3.00 times faster than it did at 343 K?
The rate constant for this second-order reaction is 0.820
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The rate constant for this second-order reaction is 0.820 M-¹. s-¹ at 300 °C. A --> products How long, in seconds, would it take for the concentration of A to decrease from 0.950 M to 0.220 M?
The rate constant for this zero-order reaction is 0.0400 M
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The rate constant for this zero-order reaction is 0.0400 M s¹ at 300 °C. A --> products How long (in seconds) would it take for the concentration of A to decrease from 0.890 M to 0.220 M?
After 44.0 min, 41.0% of a compound has decomposed. What is
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After 44.0 min, 41.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics?
The activation energy for a particular reaction is 102
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The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 x 10s¹ at 308 K, what is the rate constant at 273 K?
For the reaction A + B -> C the rate law is determined to be
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For the reaction A + B -> C the rate law is determined to be rate = (0.25 M.s)[A][B]. Which of the following will increase the rate of the reaction? Please mark all that apply, and only those that
Under certain conditions the rate of this reaction is zero
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Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.010 M-s‾¹: 2NH₃(g) → N₂(g) + 3H₂(g) Suppose a 250. mL flask is charged under these conditions with
The graph below is a potential energy diagram for the
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The graph below is a potential energy diagram for the hypothetical reaction: A + B - C + D a. Is the forward reaction endothermic or exothermic? Calculate the value of AH for this reaction. b. What is
For the decomposition of nitrous oxide at 565 °C 2 N₂0 2 N₂
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For the decomposition of nitrous oxide at 565 °C 2 N₂0 2 N₂ + 0₂ the average rate of disappearance of N₂O over the time period from t = 0 s to t= 522 s is found to be 1.54x10-³ M s¹_ The average rate
Use the information to answer the following question.
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Use the information to answer the following question. Several groups of Chemistry students are tasked with producing aluminum chloride using solid aluminum as a reactant. The teacher provides the
Describe and explain the possible effect on your results
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Describe and explain the possible effect on your results (yield and purity) of the following experimental errors or variations: a. The reaction flask you used for the preparation of m-toluoyl chloride
Reaction intermediates are never actually observed in the
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Chemical kinetics Solutions
Reaction intermediates are never actually observed in the products because They are produced in one step and then used up in a later step They disappear before we can see them They turn back into