Three students are preparing alkoxides in the lab by mixing sodium metal with a suitable alcohol. Student A uses ethanol and adds the sodium in a single piece. Student B uses ethanol and cuts the sodium into several smaller pieces. Student C also adds the sodium in a single piece, but is using propanol as the alcohol. All other reaction conditions are identical. Student B's reaction was the fastest, Students A and C find that their reactions take the same amount of time to reach completion. Which factor(s) affecting the rates of reactions is/are most likely to account for the observed differences in rate? O State of the reactants O Nature of the reaction O Both the nature of the reaction AND the states of the reactants Temperature.

Three students are preparing alkoxides in the lab by mixing sodium metal with a suitable alcohol. Student A uses ethanol and adds the sodium in a single piece. Student B uses ethanol and cuts the sodium into several smaller pieces. Student C also adds the sodium in a single piece, but is using propanol as the alcohol. All other reaction conditions are identical. Student B's reaction was the fastest, Students A and C find that their reactions take the same amount of time to reach completion. Which factor(s) affecting the rates of reactions is/are most likely to account for the observed differences in rate? O State of the reactants O Nature of the reaction O Both the nature of the reaction AND the states of the reactants Temperature.

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

An increase in temperature will Group of answer choices decrease the rate of a reaction. decrease the activation energy for a reaction. increase the amount of collisions in the system. increase the number of elementary steps in the reaction. none of the above.
The higher the rate constant, the (faster or slower) the reaction.
In general as a reaction proceeds, what happens to the rate of the reaction? Select one: a. Generally as a reaction proceeds the reaction rate will increase with time. b. Generally as a reaction proceeds the reaction rate will remain constant with time. c. Generally as a reaction proceeds the reaction rate will decrease with time.
In an all gas phase reaction, the size of the reaction flask was increased. What happens to the rate of reaction? a) rate will increase b) rate will decrease c) rate will stay the same
What is one of the key complications in producing ammonia? O The reaction is too fast to be curolled. The hydrogen reactant is very difficult to acquire. Nitrogen, a reactant, is stable and unreactive. The ammonia product is unstable and does not store well over long perfods.of.time. The necessary catalyst is very rare.
Comment how the temperature affects the rate. a. Temperature definitely has an affect on the rate. When there is an increase in temperature, the rate at which the reaction occurs also increases. This is proved through my data. As each experiment had an increasing temperature, here are my rates that go from lowest to highest temperature: 3.25*10 M/s, 4.15*10 M/s, 6.85*10 M/s, 9.17*10* M/s. With this increase in temperature, there is therefore an increase in the energy of molecules in the solution. With this increase in energy, there is an increase in collisions with enough energy, and this ultimately leads to the rate increasing.
Answer the questions for the following potential energy dia Mi ANSWER ALL QUESTIONS WITHIN THE TEST AND NOT ON THE SCRATCH PAPER. a. How many elementary steps are in this mechanism? b. Is the overall reaction exothermic or endothermic? c. Which step is the slowest? d. Which step is the fastest? e. Which steps are exothermic? f. Which steps are endothermic?
Consider the following mechanism: Cl2 → Cl+ + Cl- Cl- + H2S → HCl + HS- Cl+ + HS- → HCl + S What is the role of Cl+? A. product B. intermediate C. catalyst D. reactant
The rate of a reaction increases when a catalyst has been added to the reaction mixture. The catalyst _____ A) increases the kinetic energy of the reactants. B) decreases the rate of the reverse reaction. C) increases the number of collisions between reactants. D) alters the enthalpy of reaction. E) provides a new mechanism for the reaction to proceed by.
Answer the attached photo.