lodine, k, is reacted with cyclohexanone, CeHi00, and the chemical equation is as following: The reaction rate can be expressed as following: A(I,1 At • K[H*I[cyclohexanone) [I, T rate Chemicals HCI Cyclohexanone Distilled water Triodide, Initial concentration, M 5x 101 3x 101 4x 102 Determine the concentrations of HCI, cyclohexanone, and triiodide in this solution. Chemicals Volume added, mL Concentration in solution, M HCI Cyclohexanone Water Triiodide, Total volume, mL 16 18 12 4 50 The rate orders for H", CaH100, and I, are 1, 1 and 0, respectively. The kinetic studies of the prepared solution are analyzed in two different temperatures, which are 30°C and 40°C. Triodide decolorized at 16 minutes and 10 minutes at reaction temperatures of 30°C and 40'C, respectively. Calculate the concentrations of HCI, cyclohexanone, and triodide in the prepared solution. a b Calculate the rates of reaction at 30"C and 40°C, respectively. Calculate the rate constants for reactions at 30°C and 40'C, respectively. d Calculate the activation energy with Arrhenius equation. O°C = 273 K; gas constant, R = 8.314 J/mol-K.
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 help me with question c and d only
![lodine, k, is reacted with cyclohexanone, CeH100, and the chemical equation is as
following:
The reaction rate can be expressed as following:
A[L,]
K[H*][cyclohexanonejLT
Δι
rate -
Chemicals
HCI
Cyclohexanone
Distilled water
Triiodide,
Initial concentration, M
5x 101
3x 101
4 x 102
Determine the concentrations of HCI, cyclohexanone, and triodide in this solution.
Chemicals
Volume added,
mL
16
Concentration in solution,
M
HCI
Cyclohexanone
Water
Triiodide,
Total volume,
mL
18
12
4
50
The rate orders for H", CaH100, and , are 1, 1 and 0, respectively. The kinetic studies of
the prepared solution are analyzed in two different temperatures, which are 30°C and
40°C. Triiodide decolorized at 16 minutes and 10 minutes at reaction temperatures of
30°C and 40°C, respectively.
Calculate the concentrations of HCI, cyclohexanone, and triodide in the prepared solution.
a
Calculate the rates of reaction at 30°C and 40°C, respectively.
Calculate the rate constants for reactions at 30°C and 40°C, respectively.
Calculate the activation energy with Arrhenius equation. O°C = 273 K; gas constant, R = 8.314
J/mol-K.
d
k, E, T, - T,
In
R( T,T,
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