CHAPTER 4: AQUEOUS REACTIONS AND SOLUTION
... called the solvent. Water is considered the universal solvent because of its ability to dissolve many substances. The other dissolved substances are called the solutes. A solvent dissolves a solute. ...
... called the solvent. Water is considered the universal solvent because of its ability to dissolve many substances. The other dissolved substances are called the solutes. A solvent dissolves a solute. ...
THERMOCHEMISTRY
... Conversions of different forms of energy are governed by : The Law of Conservation of Energy: · Energy may be converted from one form to another, but the total quantity of energy remains constant. ...
... Conversions of different forms of energy are governed by : The Law of Conservation of Energy: · Energy may be converted from one form to another, but the total quantity of energy remains constant. ...
C E E ln − =
... H2N-CH2-COOH ↔ +H3N-CH2-COOWe can imagine that the formation of a zwitterion occurs as a series of steps: H2N-CH2-COOH + H2O ↔ H2N-CH2-COO- + H3O+ Ka = 4.3 × 10-3 H2N-CH2-COO- + H2O ↔ +H3N-CH2-COO- + OHKb = 6.0 × 10-5 H3O+ + OH- ↔ 2 H2O 1/Kw = 1.0 × 1014 H2N-CH2-COOH ↔ +H3N-CH2-COOKa × Kb / Kw = 2.6 ...
... H2N-CH2-COOH ↔ +H3N-CH2-COOWe can imagine that the formation of a zwitterion occurs as a series of steps: H2N-CH2-COOH + H2O ↔ H2N-CH2-COO- + H3O+ Ka = 4.3 × 10-3 H2N-CH2-COO- + H2O ↔ +H3N-CH2-COO- + OHKb = 6.0 × 10-5 H3O+ + OH- ↔ 2 H2O 1/Kw = 1.0 × 1014 H2N-CH2-COOH ↔ +H3N-CH2-COOKa × Kb / Kw = 2.6 ...
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... • 3. All common sulfides are insoluble except those of Group1A(1), Group 2A(2), and NH4+ ...
... • 3. All common sulfides are insoluble except those of Group1A(1), Group 2A(2), and NH4+ ...
Chapter 4. Aqueous Reactions and Solution Stoichiometry
... We often do not see that the net ionic equation for the reaction between strong acids and strong bases is always H+(aq) + OH–(aq) H2O(l). Weaknesses in recollection of ionic nomenclature and the structure of common ions often make it difficult for us to write molecular, complete ionic, and net ion ...
... We often do not see that the net ionic equation for the reaction between strong acids and strong bases is always H+(aq) + OH–(aq) H2O(l). Weaknesses in recollection of ionic nomenclature and the structure of common ions often make it difficult for us to write molecular, complete ionic, and net ion ...
Section – B - About iTutoring
... (18). Under which conditions Kp and Kc will be equal? When ∆n = np – nr = 0, then Kp = Kc. (19). When Kp > Kc? When ∆ng > 0, then Kp > Kc. (20). Write le- Chatelier’s principle. If from the factors determining the equilibrium state, any one factor is changed, there will be such a change in the syst ...
... (18). Under which conditions Kp and Kc will be equal? When ∆n = np – nr = 0, then Kp = Kc. (19). When Kp > Kc? When ∆ng > 0, then Kp > Kc. (20). Write le- Chatelier’s principle. If from the factors determining the equilibrium state, any one factor is changed, there will be such a change in the syst ...
1. Naturally occurring boron consists of two isotopes, boron–10 and
... 800. torr and 27.0ºC. what would its volume be if the pressure was increased to 1200. torr and it was cooled to –73.0ºC. A) 1.35 L C) 2.70 L E) 1.2 L ...
... 800. torr and 27.0ºC. what would its volume be if the pressure was increased to 1200. torr and it was cooled to –73.0ºC. A) 1.35 L C) 2.70 L E) 1.2 L ...
Chapter 5
... reaction: C8H18(l) + 25/2 O2(g) 8 CO2(g) + 9H2O(l) A 1.00 g sample of octane is burned in a bomb calorimeter that contains 1.20 kg of water surrounding the bomb. The temperature of the water rises to 33.20 °C from 25.00 °C when the octane is reacted. If the heat capacity of the bomb is 837 J/°C, c ...
... reaction: C8H18(l) + 25/2 O2(g) 8 CO2(g) + 9H2O(l) A 1.00 g sample of octane is burned in a bomb calorimeter that contains 1.20 kg of water surrounding the bomb. The temperature of the water rises to 33.20 °C from 25.00 °C when the octane is reacted. If the heat capacity of the bomb is 837 J/°C, c ...
Chemical Kinetics – Reaction Orders
... It would have been patently impossible, by merely looking at the chemical equation for this reaction, to have come up with this rate law for the reaction between H2 and Br2. Note that as far as the order of this reaction is concerned, one can only say that it is first order in H2; it is impossible t ...
... It would have been patently impossible, by merely looking at the chemical equation for this reaction, to have come up with this rate law for the reaction between H2 and Br2. Note that as far as the order of this reaction is concerned, one can only say that it is first order in H2; it is impossible t ...
Chemical equilibrium
In a chemical reaction, chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. Usually, this state results when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and backward reactions are generally not zero, but equal. Thus, there are no net changes in the concentrations of the reactant(s) and product(s). Such a state is known as dynamic equilibrium.