Chem 1B Fa2015 FinalExam Review
... [Ni(NH3)2Cl2] is a tetrahedral complex, which is a weak-field complex, and with 3d8 electron configuration for Ni2+, the complex [Ni(NH3)2Cl2] would be paramagnetic. In addition, a tetrahedral complex [Ni(NH3)2Cl2] will not exhibit isomerism. (Show d8 configuration in tetrahedral crystal field diagr ...
... [Ni(NH3)2Cl2] is a tetrahedral complex, which is a weak-field complex, and with 3d8 electron configuration for Ni2+, the complex [Ni(NH3)2Cl2] would be paramagnetic. In addition, a tetrahedral complex [Ni(NH3)2Cl2] will not exhibit isomerism. (Show d8 configuration in tetrahedral crystal field diagr ...
Writing Chemical Formulas and Chemical Reactions
... All chemical equations must be balanced so that they are consistent with the Law of Conservation of Mass. Here are some suggestions for balancing equations: 1. When balancing equations, always start with the “ugliest” molecule first (polyatomics). 2. To balance, place the desired number (coefficient ...
... All chemical equations must be balanced so that they are consistent with the Law of Conservation of Mass. Here are some suggestions for balancing equations: 1. When balancing equations, always start with the “ugliest” molecule first (polyatomics). 2. To balance, place the desired number (coefficient ...
Condensed Phase Ethanol Conversion to Higher Alcohols Tyler L
... they incorporate the acentric (ω) factor with the critical point (Tc, Pc).2 For the PRWS, three alpha functions were tested: the standard PR alpha, Boston-Mathias, and Schwartzentruber. The PRWS and PSRK equations of state had the lowest average error in prediction of vapor pressures (2.1%) of the t ...
... they incorporate the acentric (ω) factor with the critical point (Tc, Pc).2 For the PRWS, three alpha functions were tested: the standard PR alpha, Boston-Mathias, and Schwartzentruber. The PRWS and PSRK equations of state had the lowest average error in prediction of vapor pressures (2.1%) of the t ...
1.8 M - Thierry Karsenti
... 20. Hydrocarbons: Compounds made up of carbon and hydrogen only. 21. Le Chatelier’s principle: A principle which indicates that a system at equilibrium will adjust itself in such a way as to partially offset the stress when it is subjected to an external strass. 22. Rate constant: Constant of propor ...
... 20. Hydrocarbons: Compounds made up of carbon and hydrogen only. 21. Le Chatelier’s principle: A principle which indicates that a system at equilibrium will adjust itself in such a way as to partially offset the stress when it is subjected to an external strass. 22. Rate constant: Constant of propor ...
File - Varsity Field
... Product favoured reactions – reactants are completely / largely converted into products at equilibrium, e.g. combustion reactions. • Reactant favoured – small amount of reactant converted into product, e.g. ionisation of weak acids (i.e. acetic acid). • CH3CO2H (aq) + H2O (ℓ) ...
... Product favoured reactions – reactants are completely / largely converted into products at equilibrium, e.g. combustion reactions. • Reactant favoured – small amount of reactant converted into product, e.g. ionisation of weak acids (i.e. acetic acid). • CH3CO2H (aq) + H2O (ℓ) ...
Unit 2.7: Periodic Table Group1 Group2 Li Be Na Mg K Ca Rb Sr Cs
... Add excess of a standard solution of an acid or a base Either titrate the excess or make up the solution to 250.cm3 and titrate a portion of the diluted solution 1. 1.41g of a sample of chalk, which is mostly CaCO3 with some inert impurities, was placed in a beaker and 50.0cm3 1.00mol/dm3 HCl so ...
... Add excess of a standard solution of an acid or a base Either titrate the excess or make up the solution to 250.cm3 and titrate a portion of the diluted solution 1. 1.41g of a sample of chalk, which is mostly CaCO3 with some inert impurities, was placed in a beaker and 50.0cm3 1.00mol/dm3 HCl so ...
chapter 5 - chemical reactions
... 2. Identify the reactants and products and write their chemical symbols or formulas CORRECTLY. 3. Indicate the state of substances: (g) for gas, (l) for liquid, (s) for solid, and (aq) for aqueous solution. 4. Balance the equation by introducing smallest integer (whole number) coefficients in front ...
... 2. Identify the reactants and products and write their chemical symbols or formulas CORRECTLY. 3. Indicate the state of substances: (g) for gas, (l) for liquid, (s) for solid, and (aq) for aqueous solution. 4. Balance the equation by introducing smallest integer (whole number) coefficients in front ...
No Slide Title
... that produces one mole of a single product out of elements in their standard state. Because of the way we have defined the formation reaction, we may have to use fractional stoichiometric coefficients for some or all of the reactants. The enthalpy change for this reaction is defined as the enthalpy ...
... that produces one mole of a single product out of elements in their standard state. Because of the way we have defined the formation reaction, we may have to use fractional stoichiometric coefficients for some or all of the reactants. The enthalpy change for this reaction is defined as the enthalpy ...
Solutions
... ‣ The quick story is molecules have a negative end and a positive end. ‣ The negative end of one molecule sticks to the positive end of another. ‣ We’ll discuss the rest in Chapter 11. ‣ Ionic Solids are held together by one type of intermolecular force. ‣ It’s a simpler story. ‣ The cations stick t ...
... ‣ The quick story is molecules have a negative end and a positive end. ‣ The negative end of one molecule sticks to the positive end of another. ‣ We’ll discuss the rest in Chapter 11. ‣ Ionic Solids are held together by one type of intermolecular force. ‣ It’s a simpler story. ‣ The cations stick t ...
Chapter 4: Aqueous Reactions and Solution Stoichiometry
... weighs out a known mass (and, therefore, number of moles) of the solute. The solute is added to a volumetric flask, and solvent is added to the line on the neck of the flask. ...
... weighs out a known mass (and, therefore, number of moles) of the solute. The solute is added to a volumetric flask, and solvent is added to the line on the neck of the flask. ...
full text - pdf 452 kB
... This requires a knowledge of log K at the conditions (temperature, pressure, ionic strength) of the reaction. The log K values as well as the other thermodynamic quantities such as the AH,AS and ACp values associated with reactions in aqueous solutions can change in a dramatic fashion with temperatu ...
... This requires a knowledge of log K at the conditions (temperature, pressure, ionic strength) of the reaction. The log K values as well as the other thermodynamic quantities such as the AH,AS and ACp values associated with reactions in aqueous solutions can change in a dramatic fashion with temperatu ...
Chapter 2 Geochemical Reactions
... ions in solution. While often classified as acid-base reactions, they are more than this, ranging from simple acid dissociation reactions to mineral dissolution, ion hydration and formation of complex ions. pH and dissociation of acids The most fundamental of all aqueous geochemical reactions is the ...
... ions in solution. While often classified as acid-base reactions, they are more than this, ranging from simple acid dissociation reactions to mineral dissolution, ion hydration and formation of complex ions. pH and dissociation of acids The most fundamental of all aqueous geochemical reactions is the ...
Phase Transformations Some Definitions Some Definitions, 2
... a1: Liquid is in equilibrium with its vapor (composition of vapor phase given by a1’, horizontal line is called a tie line) Composition (of liquid) same at the lower pressure, so at this pressure (p1), virtually no vapor pressure a2": Pressure is lowered to p2, new pressure is below the vapor pressu ...
... a1: Liquid is in equilibrium with its vapor (composition of vapor phase given by a1’, horizontal line is called a tie line) Composition (of liquid) same at the lower pressure, so at this pressure (p1), virtually no vapor pressure a2": Pressure is lowered to p2, new pressure is below the vapor pressu ...
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.