1. Metal A has a higher specific heat than metal B. If the two metals are independently applied with equal heat, it is expected that metal A will have a higher change in temperature. 2. The units for the rate constant of an over-all 1" order reaction is s, when the reaction time is measured in seconds. If K is much greater than 1 (that is, K>>1), the equilibrium will favor the formation of reactants. 3. 4. In the iron-thiocyanate system, increasing the pH would produce a dark orange solution. 5. For a weak acid HA, the equilibrium concentration of H3O* is equal to [HA]i- 6. The buffer region is the pH range where a buffer effectively neutralizes added acids and bases, while maintaining a relatively constant pH. A buffer can be expressed by the Henderson-Hasselbaich equation. Diluting a concentrated weak base, results to an increase in pH. 7. 8. 9. The plot of absorbance versus concentration of an absorbing species will be linear at all concentrations. 10. For a system at equilibrium, the rate of the forward and reverse reactions is the same. 11. Using a wider beaker in a single run increases the reaction rate between persulfate and iodide. 12. The entire experiment is under adiabatic and isothermal conditions.
Basics in Organic Reactions Mechanisms
In organic chemistry, the mechanism of an organic reaction is defined as a complete step-by-step explanation of how a reaction of organic compounds happens. A completely detailed mechanism would relate the first structure of the reactants with the last structure of the products and would represent changes in structure and energy all through the reaction step.
Heterolytic Bond Breaking
Heterolytic bond breaking is also known as heterolysis or heterolytic fission or ionic fission. It is defined as breaking of a covalent bond between two different atoms in which one atom gains both of the shared pair of electrons. The atom that gains both electrons is more electronegative than the other atom in covalent bond. The energy needed for heterolytic fission is called as heterolytic bond dissociation energy.
Polar Aprotic Solvent
Solvents that are chemically polar in nature and are not capable of hydrogen bonding (implying that a hydrogen atom directly linked with an electronegative atom is not found) are referred to as polar aprotic solvents. Some commonly used polar aprotic solvents are acetone, DMF, acetonitrile, DMSO, etc.
Oxygen Nucleophiles
Oxygen being an electron rich species with a lone pair electron, can act as a good nucleophile. Typically, oxygen nucleophiles can be found in these compounds- water, hydroxides and alcohols.
Carbon Nucleophiles
We are aware that carbon belongs to group IV and hence does not possess any lone pair of electrons. Implying that neutral carbon is not a nucleophile then how is carbon going to be nucleophilic? The answer to this is that when a carbon atom is attached to a metal (can be seen in the case of organometallic compounds), the metal atom develops a partial positive charge and carbon develops a partial negative charge, hence making carbon nucleophilic.
Please answer 6-12
![Write true if the statement is true,
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1. Metal A has a higher specific heat than metal B. If the two metals are independently applied with equal
heat, it is expected that metal A will have a higher change in temperature.
2. The units for the rate constant of an over-all 1st order reaction is s', when the reaction time is measured in
seconds.
3.
If K is much greater than 1 (that is, K>>1), the equilibrium will favor the formation of reactants.
4.
In the iron-thiocyanate system, increasing the pH would produce a dark orange solution.
5.
For a weak acid HA, the equilibrium concentration of H3O* is equal to [HA]i.
6. The buffer region is the pH range where a buffer effectively neutralizes added acids and bases, while
maintaining a relatively constant pH.
A buffer can be expressed by the Henderson-Hasselbaich equation.
7.
8. Diluting a concentrated weak base, results to an increase in pH.
9. The plot of absorbance versus concentration of an absorbing, species will be linear at all concentrations.
10. For a system at equilibrium, the rate of the forward and reverse reactions is the same.
11. Using a wider beaker in a single run increases the reaction rate between persulfate and iodide.
12. The entire experiment is under adiabatic and isothermal conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fec9523be-5f6c-46bc-84ca-9af77089f748%2F0cc47dc2-333c-48a4-ba8a-bae1a4e53dcc%2F4wyak5i_processed.jpeg&w=3840&q=75)
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