Inorganic Chemistry
... quantities, A and G as criteria for thermodynamic equilibrium and spontaneity, their advantage over entropy change. Variation of G and A with P, V and T. Gibbs-Helmoltz equation, Clapeyron equation, Clausius-Clapeyron equation, reaction isotherm and reaction isochore. 2. Chemical Equilibrium 06 hrs ...
... quantities, A and G as criteria for thermodynamic equilibrium and spontaneity, their advantage over entropy change. Variation of G and A with P, V and T. Gibbs-Helmoltz equation, Clapeyron equation, Clausius-Clapeyron equation, reaction isotherm and reaction isochore. 2. Chemical Equilibrium 06 hrs ...
Year 9 Chemical Sciences Program Term 3 Course 2 2017
... recognising that the conservation of mass in a chemical reaction can be demonstrated by simple chemical equations ...
... recognising that the conservation of mass in a chemical reaction can be demonstrated by simple chemical equations ...
CHEMICAL REACTIONS
... ________ 20. The complete combustion of octane (C8H18) would: a. require 25 O2(g). c. produce 18 H2O(g). b. produce 16 CO2(g). d. all of the above ________ 21. Double-replacement reactions are generally driven by the formation of: a. a precipitate. c. water. b. a gaseous product. d. all of the above ...
... ________ 20. The complete combustion of octane (C8H18) would: a. require 25 O2(g). c. produce 18 H2O(g). b. produce 16 CO2(g). d. all of the above ________ 21. Double-replacement reactions are generally driven by the formation of: a. a precipitate. c. water. b. a gaseous product. d. all of the above ...
Yr-11-Chem-ATAR-unit-2
... solutions. They learn how rates of reaction can be measured and altered to meet particular needs, and use models of energy transfer and the structure of matter to explain and predi ...
... solutions. They learn how rates of reaction can be measured and altered to meet particular needs, and use models of energy transfer and the structure of matter to explain and predi ...
Double-Replacement Reactions - Fort Thomas Independent Schools
... • The classification scheme described in this section provides an introduction to five basic types of reactions: • Synthesis (Combination) • Decomposition • Single-displacement (replacement) • Double-displacement (replacement) • Combustion reactions ...
... • The classification scheme described in this section provides an introduction to five basic types of reactions: • Synthesis (Combination) • Decomposition • Single-displacement (replacement) • Double-displacement (replacement) • Combustion reactions ...
Teacher Background - Online Learning Exchange
... balanced chemical equations as a basis for calculating how much reactant is needed or how much product will be formed in a reaction. When you know the quantity of one substance in a reaction, you can calculate the quantity of any other substance consumed or produced in the reaction. Quantity usually ...
... balanced chemical equations as a basis for calculating how much reactant is needed or how much product will be formed in a reaction. When you know the quantity of one substance in a reaction, you can calculate the quantity of any other substance consumed or produced in the reaction. Quantity usually ...
Summer Work
... First Exercise: Fe3+(aq) + SCN-(aq) FeSCN2+(aq) If at equilibrium and 25°C, you have [FeSCN2+] = 0.25 mol/L, [Fe3+] = 0.046 mol/L, and [SCN-] = 0.046 mol/L, what is the equilibrium constant, Keq? ...
... First Exercise: Fe3+(aq) + SCN-(aq) FeSCN2+(aq) If at equilibrium and 25°C, you have [FeSCN2+] = 0.25 mol/L, [Fe3+] = 0.046 mol/L, and [SCN-] = 0.046 mol/L, what is the equilibrium constant, Keq? ...
Notes on kinetic and potential energy
... just rearranged. We can be even more explicit and say that the number of atoms, and the mass of each atom, are not changed in a chemical reaction. Thus there is overall conservation of mass during chemical reactions. This conservation concept is rather easy to grasp and was verified experimentally i ...
... just rearranged. We can be even more explicit and say that the number of atoms, and the mass of each atom, are not changed in a chemical reaction. Thus there is overall conservation of mass during chemical reactions. This conservation concept is rather easy to grasp and was verified experimentally i ...
2 - My CCSD
... Ag1+ + NO31- + Na1+ + Cl1- AgCl + Na1+ + NO31Note that the AgCl did not ionize, because it is a “precipitate” ...
... Ag1+ + NO31- + Na1+ + Cl1- AgCl + Na1+ + NO31Note that the AgCl did not ionize, because it is a “precipitate” ...
Document
... 93. The coefficients are missing from the skeleton equation below. Cr (s) + Fe(NO3)2 (aq) Fe(s) + Cr(NO3)3 (aq) The correct order for the missing coefficients is_________. 94. The equation 2 C3H7OH + 9 O2 6 CO2 + 8 H2O is an example of which type of ...
... 93. The coefficients are missing from the skeleton equation below. Cr (s) + Fe(NO3)2 (aq) Fe(s) + Cr(NO3)3 (aq) The correct order for the missing coefficients is_________. 94. The equation 2 C3H7OH + 9 O2 6 CO2 + 8 H2O is an example of which type of ...
SUMMER WORK AP Chemistry
... (a) Write a net ionic equation for the reaction that occurs in each of the experiments. (b) Identify the precipitate formed, if any, in each of the experiments. 14. Calculate ΔE and determine whether the process is endothermic or exothermic for the following cases: (a) q = 0.763 kJ and w = –840 J; ( ...
... (a) Write a net ionic equation for the reaction that occurs in each of the experiments. (b) Identify the precipitate formed, if any, in each of the experiments. 14. Calculate ΔE and determine whether the process is endothermic or exothermic for the following cases: (a) q = 0.763 kJ and w = –840 J; ( ...
Class Notes
... - salts with alkali metals (Li+1, Na+1, K+1, etc) - salts with ammonium (NH4+1) - Sulfates (SO4-2) (except in salts with Pb+2, Ag+1, Hg+2, Ba+2, Sr+2, and Ca+2) - Chlorides (Cl-1), Bromides (Br-1), and Iodides (I-1) (except in salts with Ag+1, ...
... - salts with alkali metals (Li+1, Na+1, K+1, etc) - salts with ammonium (NH4+1) - Sulfates (SO4-2) (except in salts with Pb+2, Ag+1, Hg+2, Ba+2, Sr+2, and Ca+2) - Chlorides (Cl-1), Bromides (Br-1), and Iodides (I-1) (except in salts with Ag+1, ...
Chemical theory for mixtures containing any number of alcohols
... Finally, the model xs compared with statistical assocmtmg fluid theory (SAFT) and the two approaches are found to be strikingly similar ...
... Finally, the model xs compared with statistical assocmtmg fluid theory (SAFT) and the two approaches are found to be strikingly similar ...
KUT 101/2 – General Chemistry Practical I
... • Differentiate the primary and secondary standards. • Differentiate the equivalence and end-points. • Choose suitable indicators for acid-base titration. • Determine the amount of acid in an unknown. • Know a quantitative technique of volumetric analysis. • Understand the definition of BOD (Biochem ...
... • Differentiate the primary and secondary standards. • Differentiate the equivalence and end-points. • Choose suitable indicators for acid-base titration. • Determine the amount of acid in an unknown. • Know a quantitative technique of volumetric analysis. • Understand the definition of BOD (Biochem ...
Chemistry 1A Final Exam December 12, 2001 Page 1 of 16 (Closed
... increase the partial pressure of NH3 (g) at equilibrium decrease the partial pressure of H2 (g) at equilibrium increase the value of the equilibrium constant cause the reaction to shift to the right increase the reaction temperature ...
... increase the partial pressure of NH3 (g) at equilibrium decrease the partial pressure of H2 (g) at equilibrium increase the value of the equilibrium constant cause the reaction to shift to the right increase the reaction temperature ...
Solution
... d) Calculate the equilibrium constant for this reaction at 25°C. Are products or reactants favored at equilibrium under standard conditions? Is this consistent with part (c)? Explain your answer. dG = -RT*lnK K = e-dG/RT = e-(-4.75 x 105 J/(8.31J/(K*mol)*298 K) = 1.83 x 1083, this is a very large K ...
... d) Calculate the equilibrium constant for this reaction at 25°C. Are products or reactants favored at equilibrium under standard conditions? Is this consistent with part (c)? Explain your answer. dG = -RT*lnK K = e-dG/RT = e-(-4.75 x 105 J/(8.31J/(K*mol)*298 K) = 1.83 x 1083, this is a very large K ...
File
... (b) Evaporation of water. (c) Distribution of solute throughout the solvent. (d) Expansion of gases. (e) Flow of water from a hill to the ground. (f) Mixing of gases. In all the above cases, the system reaches a state of greater disorder. Eventhough the energy of the system increases (endothermic) d ...
... (b) Evaporation of water. (c) Distribution of solute throughout the solvent. (d) Expansion of gases. (e) Flow of water from a hill to the ground. (f) Mixing of gases. In all the above cases, the system reaches a state of greater disorder. Eventhough the energy of the system increases (endothermic) d ...
Chemical thermodynamics
Chemical thermodynamics is the study of the interrelation of heat and work with chemical reactions or with physical changes of state within the confines of the laws of thermodynamics. Chemical thermodynamics involves not only laboratory measurements of various thermodynamic properties, but also the application of mathematical methods to the study of chemical questions and the spontaneity of processes.The structure of chemical thermodynamics is based on the first two laws of thermodynamics. Starting from the first and second laws of thermodynamics, four equations called the ""fundamental equations of Gibbs"" can be derived. From these four, a multitude of equations, relating the thermodynamic properties of the thermodynamic system can be derived using relatively simple mathematics. This outlines the mathematical framework of chemical thermodynamics.