Esters
... used (usually sulphuric acid) A condensation reaction The condensation reaction between the hydroxyl group and the carboxylic acid known as esterification. Reverse reaction = ester hydrolysis ...
... used (usually sulphuric acid) A condensation reaction The condensation reaction between the hydroxyl group and the carboxylic acid known as esterification. Reverse reaction = ester hydrolysis ...
unit 4 revision checklist - A
... a) Derive an expression for the equilibrium constant Kc of a chemical reaction, and deduce its units b) Calculate the equilibrium constant of a reaction from equilibrium concentration data and vice versa c) Calculate the equilibrium constant of a reaction from initial concentration data and some inf ...
... a) Derive an expression for the equilibrium constant Kc of a chemical reaction, and deduce its units b) Calculate the equilibrium constant of a reaction from equilibrium concentration data and vice versa c) Calculate the equilibrium constant of a reaction from initial concentration data and some inf ...
KEY - Practice Qs
... (b) Explain, in terms of electron configuration, why oxygen atoms and sulfur atoms form compounds with similar molecular structures. Oxygen and sulfur atoms have the same number (six) of valence electrons. OR Atoms of both elements need two more valence electrons to complete their outer shells. (c) ...
... (b) Explain, in terms of electron configuration, why oxygen atoms and sulfur atoms form compounds with similar molecular structures. Oxygen and sulfur atoms have the same number (six) of valence electrons. OR Atoms of both elements need two more valence electrons to complete their outer shells. (c) ...
Unit 6 Interactive Reading Packet File - District 196 e
... 17. Which of the following is/are true concerning enthalpy? a) ∆H for a reaction depends upon the states of the reactants and products. b) ∆H (forward reaction) = -∆H (reverse reaction) c) The enthalpy of a system is independent of the way the system achieved its current state. d) Changes in enthalp ...
... 17. Which of the following is/are true concerning enthalpy? a) ∆H for a reaction depends upon the states of the reactants and products. b) ∆H (forward reaction) = -∆H (reverse reaction) c) The enthalpy of a system is independent of the way the system achieved its current state. d) Changes in enthalp ...
Alkene/Alkyne Addition Reactions
... Alcohols are named in the exact same manner as alkanes, alkenes, and alkynes except: To find the base name, drop the “e” from the name of the corresponding alkane and add “ol” Use the carbon number to identify the position of the alcohol. CH3CH2CHCH3 CH3CH2CH2OH ...
... Alcohols are named in the exact same manner as alkanes, alkenes, and alkynes except: To find the base name, drop the “e” from the name of the corresponding alkane and add “ol” Use the carbon number to identify the position of the alcohol. CH3CH2CHCH3 CH3CH2CH2OH ...
aldehydes and ketones
... • Ketones have greater steric crowding in their transition states, so they have less stable transition states. ...
... • Ketones have greater steric crowding in their transition states, so they have less stable transition states. ...
thermdyn - chemmybear.com
... The entropy increases (S>0) since solid reactants (b) 2 C + 2 O2 2 CO2 are converted to gases and liquids, which have a H = 2(-393.5) = -787.0 kJ much higher degree of disorder. 2 H2 + O2 2 H2O The free energy decreases (G<0) as is shown by H = 2(-285.8) = -571.6 kJ the fact that the react ...
... The entropy increases (S>0) since solid reactants (b) 2 C + 2 O2 2 CO2 are converted to gases and liquids, which have a H = 2(-393.5) = -787.0 kJ much higher degree of disorder. 2 H2 + O2 2 H2O The free energy decreases (G<0) as is shown by H = 2(-285.8) = -571.6 kJ the fact that the react ...
Part II - American Chemical Society
... iii. An increase in temperature will cause the relative amount of reactants to increase and products to decrease. This can be explained by noting that the value of ∆Hrxn is negative, which means that adding heat will shift the reaction to the left. Another argument is that as the temperature increas ...
... iii. An increase in temperature will cause the relative amount of reactants to increase and products to decrease. This can be explained by noting that the value of ∆Hrxn is negative, which means that adding heat will shift the reaction to the left. Another argument is that as the temperature increas ...
a ΔG - KFUPM Resources v3
... In other words, what is the situation when enthalpy and entropy compete with each other? Gibbs free energy (or simply free energy) is another thermodynamic quantity that reflects the balance between enthalpy and entropy of a system. Gibbs free energy is defined as: G = H – TS The change in Gibbs f ...
... In other words, what is the situation when enthalpy and entropy compete with each other? Gibbs free energy (or simply free energy) is another thermodynamic quantity that reflects the balance between enthalpy and entropy of a system. Gibbs free energy is defined as: G = H – TS The change in Gibbs f ...
AP Chemistry - cloudfront.net
... mixture: (a) distilled water; (b) gasoline; (c) beach sand; (d) wine; (e) air. 2.109 name the technique(s) and briefly describe the procedure you would use to separate the following mixture into two components: (table salt and pepper; (b) table sugar and ...
... mixture: (a) distilled water; (b) gasoline; (c) beach sand; (d) wine; (e) air. 2.109 name the technique(s) and briefly describe the procedure you would use to separate the following mixture into two components: (table salt and pepper; (b) table sugar and ...
