2016 - Specimen Paper 4 - Cambridge International Examinations
... number of moles of HCl used = ………………………………………………...…..……. number of moles of CoCl2 formed = ……………………………………………..….…… number of moles of CoCl2.6H2O formed = ………………………………………..…..… mass of one mole of CoCl2.6H2O = 238 g maximum yield of CoCl2.6H2O = …………………………………………………..…..… g to show that cobalt(II) ca ...
... number of moles of HCl used = ………………………………………………...…..……. number of moles of CoCl2 formed = ……………………………………………..….…… number of moles of CoCl2.6H2O formed = ………………………………………..…..… mass of one mole of CoCl2.6H2O = 238 g maximum yield of CoCl2.6H2O = …………………………………………………..…..… g to show that cobalt(II) ca ...
Final competitions (29.03.2008) Competing equilibria Complex
... b. A precipitate of iron(III) hydroxide is probably obtained in solution of higher pH (solution B), what can be checked after calculation of free Fe3+ ions concentration. Total concentration of soluble Fe(III) forms, cFe, is: cFe = [Fe3+] + [FeC2O4+] + [Fe(C2O4)2-] + [Fe(C2O4)33-] Using equations de ...
... b. A precipitate of iron(III) hydroxide is probably obtained in solution of higher pH (solution B), what can be checked after calculation of free Fe3+ ions concentration. Total concentration of soluble Fe(III) forms, cFe, is: cFe = [Fe3+] + [FeC2O4+] + [Fe(C2O4)2-] + [Fe(C2O4)33-] Using equations de ...
4-아미노피리딘 – HCl, –HBr 복합체에 대한 양자화학적 연구 : 즈비터
... 3-N site in an “inverted” fashion with the Br atom, rather than the hydrogen atom, interacting with 3-N. The conformer (a), in which HBr bonds to 1-N, is now calculated to be ~2 kcal/mol higher than (d). It would be useful to examine the structural features of (d) to elucidate this stability of the ...
... 3-N site in an “inverted” fashion with the Br atom, rather than the hydrogen atom, interacting with 3-N. The conformer (a), in which HBr bonds to 1-N, is now calculated to be ~2 kcal/mol higher than (d). It would be useful to examine the structural features of (d) to elucidate this stability of the ...
Review #7: Solutions, Acids and Bases 1. Definitions: a) Solution: a
... sodium chloride), or a solution that contains these ions in equal concentrations (for example, water). Its pH is 7.0. ...
... sodium chloride), or a solution that contains these ions in equal concentrations (for example, water). Its pH is 7.0. ...
Chapter 4,5,6
... 9. Suppose that nitrosyl chloride gas (NOCl) is produced by reacting 6.00 g of chlorine gas with 5.00 g of nitric oxide gas (NO). (a) If the reaction is carried out in a 15.0 L container at a constant temperature of 35.00C, calculate the total pressure in the container after the reaction is complete ...
... 9. Suppose that nitrosyl chloride gas (NOCl) is produced by reacting 6.00 g of chlorine gas with 5.00 g of nitric oxide gas (NO). (a) If the reaction is carried out in a 15.0 L container at a constant temperature of 35.00C, calculate the total pressure in the container after the reaction is complete ...
Lesson 2: Electrolytes
... ions are found in ionic compounds 2. These charges must be mobile when dissolved in water, the ions are pulled apart and are free to conduct electricity 3. The charges must move in a particular direction the electrodes on the electrical conductivity meter direct the charges ...
... ions are found in ionic compounds 2. These charges must be mobile when dissolved in water, the ions are pulled apart and are free to conduct electricity 3. The charges must move in a particular direction the electrodes on the electrical conductivity meter direct the charges ...
Exames anteriores a 1994
... d) M forms a complex ML with the acid H2L with the formation constant K1. The solution contains an other metal ion N that forms a complex NHL with the acid H2L. Determine the conditional equilibrium constant, K’1 for the complex ML in terms of [H+] and K values. [M’] = total concentration of M not b ...
... d) M forms a complex ML with the acid H2L with the formation constant K1. The solution contains an other metal ion N that forms a complex NHL with the acid H2L. Determine the conditional equilibrium constant, K’1 for the complex ML in terms of [H+] and K values. [M’] = total concentration of M not b ...
Chemistry - Onslow College
... as metals, C, CO, H2, Fe2+, Br-, I-, SO2, HSO3-, H2S, SO32-, H2O2 5. Carry out redox reactions use the properties of oxidants and reductants to identify the product of redox reactions Properties are limited to appearance ie colour and state identify the oxidant and/or reductant from reaction ...
... as metals, C, CO, H2, Fe2+, Br-, I-, SO2, HSO3-, H2S, SO32-, H2O2 5. Carry out redox reactions use the properties of oxidants and reductants to identify the product of redox reactions Properties are limited to appearance ie colour and state identify the oxidant and/or reductant from reaction ...
Fall 2012
... 62. While working in the lab you accidentally spill about 10 mL of 1 M H2SO4 on the benchtop. You make a quick check of yourself and find no evidence of splashes. What should you do next? a. ...
... 62. While working in the lab you accidentally spill about 10 mL of 1 M H2SO4 on the benchtop. You make a quick check of yourself and find no evidence of splashes. What should you do next? a. ...
Donnan phenomena in membranes with charge due to ion
... In Eqs. (2) and (3)) the ,V”S refer to the standard-state chemical potentials while q?D=e(c$2-$l)/kT is the Donnan potential in kT/e units established between the two phases, while k is the Boltzmann constant, T, the temperature, and e, the absolute value of the electronic charge. The NaCl and HCl c ...
... In Eqs. (2) and (3)) the ,V”S refer to the standard-state chemical potentials while q?D=e(c$2-$l)/kT is the Donnan potential in kT/e units established between the two phases, while k is the Boltzmann constant, T, the temperature, and e, the absolute value of the electronic charge. The NaCl and HCl c ...
Department of Chemistry, IIT-Delhi CY110N Tutorial
... 3. The standard reaction Gibbs energy of K4 [Fe(CN)6 ]·3H2 O→ 4K+ (aq) + [Fe(CN)6 ]4− (aq) +3H2 O(l) is 26.12 kJ/mol. The enthalpy of solution of the trihydrate is +55.0 kJ/mol. Calculate the standard molar entropy of solution of the hexacyanoferrate (II) ion in water given that the standard molar e ...
... 3. The standard reaction Gibbs energy of K4 [Fe(CN)6 ]·3H2 O→ 4K+ (aq) + [Fe(CN)6 ]4− (aq) +3H2 O(l) is 26.12 kJ/mol. The enthalpy of solution of the trihydrate is +55.0 kJ/mol. Calculate the standard molar entropy of solution of the hexacyanoferrate (II) ion in water given that the standard molar e ...
summer fun - West Windsor-Plainsboro Regional School District
... to go to completion. Unionized or partially ionized molecules give solutions that are known as nonelectrolytes or weak electrolytes. The best know nonelectrolyte is water formed in acid-base neutralization reactions. Acetic acid is an example of an acid that is primarily molecular (weak electrolyte) ...
... to go to completion. Unionized or partially ionized molecules give solutions that are known as nonelectrolytes or weak electrolytes. The best know nonelectrolyte is water formed in acid-base neutralization reactions. Acetic acid is an example of an acid that is primarily molecular (weak electrolyte) ...
Differential Equations of Gas-Phase Chemical Kinetics
... chemistry. The program uses thermodynamic data and chemical reactions that have the CHEMKIN-II description. The information is collected in databases that are stored in files of the Microsoft Access type. The data are displayed in the tables and can be easily handled. Chemked has the multipledocumen ...
... chemistry. The program uses thermodynamic data and chemical reactions that have the CHEMKIN-II description. The information is collected in databases that are stored in files of the Microsoft Access type. The data are displayed in the tables and can be easily handled. Chemked has the multipledocumen ...
Equilibrium chemistry
Equilibrium chemistry is a concerned with systems in chemical equilibrium. The unifying principle is that the free energy of a system at equilibrium is the minimum possible, so that the slope of the free energy with respect to the reaction coordinate is zero. This principle, applied to mixtures at equilibrium provides a definition of an equilibrium constant. Applications include acid-base, host-guest, metal-complex, solubility, partition, chromatography and redox equilibria.