Thermochemistry Review
... A. The heat required to raise the temperature of one gram of water by one Celsius degree. B. The heat required to raise the temperature of one mole of water by one Celsius degree. C. The heat required to raise the temperature of one gram of substance by one Celsius degree. D. The heat required to ra ...
... A. The heat required to raise the temperature of one gram of water by one Celsius degree. B. The heat required to raise the temperature of one mole of water by one Celsius degree. C. The heat required to raise the temperature of one gram of substance by one Celsius degree. D. The heat required to ra ...
Chapter 11.1: Describing Chemical Reactions
... Aqueous solution (dissolved in water) Indicates that heat is supplied to the reaction A formula written above or below a yield sign indicates its use as a catalyst (in tis example, Sulfuric Acid). ...
... Aqueous solution (dissolved in water) Indicates that heat is supplied to the reaction A formula written above or below a yield sign indicates its use as a catalyst (in tis example, Sulfuric Acid). ...
CST REVIEW Percent Error 1. 2. What is the formula for density?
... 23. If 85% of the isotopes of an element have a mass of 44.0 amu and 15% of the isotopes have a mass of 47 amu, what is the atomic mass of the element? Show work 24. Atoms combine to form molecules by electrons to form covalent bonds or by exchanging/transferring electrons to form bonds. 25. Are the ...
... 23. If 85% of the isotopes of an element have a mass of 44.0 amu and 15% of the isotopes have a mass of 47 amu, what is the atomic mass of the element? Show work 24. Atoms combine to form molecules by electrons to form covalent bonds or by exchanging/transferring electrons to form bonds. 25. Are the ...
CHAPTER 9 : CHEMICAL BONDING I
... 9.92 The amide ion, NH-2 , is a Bronsted base, Represent the reaction between the amide ion and water. 9.94 The triiodide ion (I-3) in which the I atoms are arranged in a straight line is stable, but the corresponding F-3 ion does not exist. Explain. 9.96 Methyl isocyanate (CH3NCO) is used to make c ...
... 9.92 The amide ion, NH-2 , is a Bronsted base, Represent the reaction between the amide ion and water. 9.94 The triiodide ion (I-3) in which the I atoms are arranged in a straight line is stable, but the corresponding F-3 ion does not exist. Explain. 9.96 Methyl isocyanate (CH3NCO) is used to make c ...
Section 1 The Nature of Chemical Reactions
... • Explain the effect a catalyst has on a chemical reaction. • Explain chemical equilibrium in terms of equal forward and reverse reaction rates. ...
... • Explain the effect a catalyst has on a chemical reaction. • Explain chemical equilibrium in terms of equal forward and reverse reaction rates. ...
PHYSICAL CHEMISTRY ERT 108 Semester II 2010
... tabulated thermodynamic data for reactants and products. However, the laws of thermodynamics only allow us to measure changes in entalpy, internal energy and entropies (ΔH, ΔU and ΔS, not the absolute values of U, H, and S, and we cannot tabulate absolute enthalpies of substances. Instead, we can ...
... tabulated thermodynamic data for reactants and products. However, the laws of thermodynamics only allow us to measure changes in entalpy, internal energy and entropies (ΔH, ΔU and ΔS, not the absolute values of U, H, and S, and we cannot tabulate absolute enthalpies of substances. Instead, we can ...
The five main types of redox reactions are combination
... are those in which the oxidation states of the reactants change. This occurs because in such reactions, electrons are always transferred between species. Redox reactions take place through either a simple process, such as the burning of carbon in oxygen to yield carbon dioxide (CO2), or a more compl ...
... are those in which the oxidation states of the reactants change. This occurs because in such reactions, electrons are always transferred between species. Redox reactions take place through either a simple process, such as the burning of carbon in oxygen to yield carbon dioxide (CO2), or a more compl ...
unit 4 practice
... 19. According to this information, as the temperature of the system increases, the equilibrium shifts A. left, and the reaction is exothermic B. left and the reaction is endothermic C. right and th ...
... 19. According to this information, as the temperature of the system increases, the equilibrium shifts A. left, and the reaction is exothermic B. left and the reaction is endothermic C. right and th ...
Final Exam Practice Problems: R = 0.0821 Latm/molK NA = 6.022
... A) Li+ (aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq) B) Li+ (aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq) C) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) ...
... A) Li+ (aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq) B) Li+ (aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq) C) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) ...
Reaction Rate Graphs C12-3
... same rate. Some reactions are very fast (eg. explosions), while others are very slow (eg. the rusting of iron). The Collision Theory states that: Chemical reactions involve collisions of reactant particles. Not all collisions lead to a chemical reaction. For molecules to react (effective colli ...
... same rate. Some reactions are very fast (eg. explosions), while others are very slow (eg. the rusting of iron). The Collision Theory states that: Chemical reactions involve collisions of reactant particles. Not all collisions lead to a chemical reaction. For molecules to react (effective colli ...
3.0 Hess`s Law
... known as Hess’s law: the overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process. • This means that the energy difference between reactants and products is independent of the route taken to get from one to the other. ...
... known as Hess’s law: the overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process. • This means that the energy difference between reactants and products is independent of the route taken to get from one to the other. ...
Chem161 Chapter 6
... to the average kinetic energy of its particles —the higher the average kinetic energy, the higher the temperature • Heat is energy (also called thermal energy) transferred between objects caused by differences in their temperatures until they reach thermal equilibrium ...
... to the average kinetic energy of its particles —the higher the average kinetic energy, the higher the temperature • Heat is energy (also called thermal energy) transferred between objects caused by differences in their temperatures until they reach thermal equilibrium ...
2009
... 2 For this section of the examination you must use an HB pencil and, where necessary, an eraser. 3 Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish Candidate Number) and Centre Name printed on it. Do not change any of these details. 4 If any of this informa ...
... 2 For this section of the examination you must use an HB pencil and, where necessary, an eraser. 3 Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish Candidate Number) and Centre Name printed on it. Do not change any of these details. 4 If any of this informa ...
第一章 绪论
... Another step in drug discovery involves further chemical modifications in order to improve the biological and physiochemical properties of a given candidate compound library. Chemical modifications can improve the pharmacophores of the candidate compounds, their pharmacokinetics, or indeed their rea ...
... Another step in drug discovery involves further chemical modifications in order to improve the biological and physiochemical properties of a given candidate compound library. Chemical modifications can improve the pharmacophores of the candidate compounds, their pharmacokinetics, or indeed their rea ...
Chemistry B1A - Bakersfield College
... Some iron wire weighing 5.6 g is placed in a beaker and covered with 15.1 g of hydrochloric acid. The acid reacts with the metal and gives off hydrogen gas, which escapes into the surrounding air. After reaction the contents of the beaker weighs 20.4 g. What is the mass of hydrogen produced? Write t ...
... Some iron wire weighing 5.6 g is placed in a beaker and covered with 15.1 g of hydrochloric acid. The acid reacts with the metal and gives off hydrogen gas, which escapes into the surrounding air. After reaction the contents of the beaker weighs 20.4 g. What is the mass of hydrogen produced? Write t ...
Equilibrium
... Often reactions are written with only ions that are actually involved in the reaction. This is why the nitrate and potassium ions have been left off of the equation. These ions that are left off the equation are called spectator ions. Write this equation and below each chemical list the solution col ...
... Often reactions are written with only ions that are actually involved in the reaction. This is why the nitrate and potassium ions have been left off of the equation. These ions that are left off the equation are called spectator ions. Write this equation and below each chemical list the solution col ...
Chemistry 12 – Unit 3 – Chapter 5 – Thermochemistry
... ∆H0reaction = Σ n∆H0f products - Σ n∆H0f reactants ∆H0rxn = [6 mol x ∆H0f of H2O(l) + 6 mol x ∆H0f of CO2(g)] – [2 mol x ∆H0f of C3H6(g) + 9 mol x ∆H0f of O2(g)] ∆H0rxn = [ 6 mol x(-285.8 kJ/mol) + 6 mol x (-393.5 kJ/mol) ] – [ 2 mol x (17.8 kJ/mol) + 9 mol x (0 kJ/mol)] ∆H0rxn = [ -1714.8 kJ + -236 ...
... ∆H0reaction = Σ n∆H0f products - Σ n∆H0f reactants ∆H0rxn = [6 mol x ∆H0f of H2O(l) + 6 mol x ∆H0f of CO2(g)] – [2 mol x ∆H0f of C3H6(g) + 9 mol x ∆H0f of O2(g)] ∆H0rxn = [ 6 mol x(-285.8 kJ/mol) + 6 mol x (-393.5 kJ/mol) ] – [ 2 mol x (17.8 kJ/mol) + 9 mol x (0 kJ/mol)] ∆H0rxn = [ -1714.8 kJ + -236 ...
SAMPLE PAPER -9 Time Allowed: 3 Hrs
... chains are arranged side by side in Zig – Zag with alternate R on same side. Two neighbouring chains are held by H bond . Sheets are stacked one above the other like pages of book. ...
... chains are arranged side by side in Zig – Zag with alternate R on same side. Two neighbouring chains are held by H bond . Sheets are stacked one above the other like pages of book. ...
PHYSICAL SETTING CHEMISTRY
... 58 Determine the total number of electrons in the bonds between the nitrogen atom and the three hydrogen atoms represented in diagram 2. [1] 59 Explain, in terms of distribution of charge, why a molecule of the substance represented in diagram 3 is nonpolar. [1] 60 Draw a Lewis electron-dot diagram ...
... 58 Determine the total number of electrons in the bonds between the nitrogen atom and the three hydrogen atoms represented in diagram 2. [1] 59 Explain, in terms of distribution of charge, why a molecule of the substance represented in diagram 3 is nonpolar. [1] 60 Draw a Lewis electron-dot diagram ...
Spring 2001 Key
... heat. -----------------------------------------------------------------------------------------------------------(d) is a false statement: production of 6 moles of CO2 will produce 4440 kJ of heat. The reaction is exothermic. Energy would be required if the reaction was endothermic. (a) is true sinc ...
... heat. -----------------------------------------------------------------------------------------------------------(d) is a false statement: production of 6 moles of CO2 will produce 4440 kJ of heat. The reaction is exothermic. Energy would be required if the reaction was endothermic. (a) is true sinc ...
Document
... of the system, regardless of how that condition was achieved. energy, pressure, volume, temperature ...
... of the system, regardless of how that condition was achieved. energy, pressure, volume, temperature ...
Stoichiometry
... cation of another compound. AX + BZ AZ + BX These reactions proceed if one of the ff. is satisfied: 1. An insoluble/slightly soluble product is formed (PRECIPITATE formation) 2. A weakly ionized species is produced. The most common species of this type is water. 3. A gas is produced as a product. ...
... cation of another compound. AX + BZ AZ + BX These reactions proceed if one of the ff. is satisfied: 1. An insoluble/slightly soluble product is formed (PRECIPITATE formation) 2. A weakly ionized species is produced. The most common species of this type is water. 3. A gas is produced as a product. ...
Bioorthogonal chemistry
The term bioorthogonal chemistry refers to any chemical reaction that can occur inside of living systems without interfering with native biochemical processes. The term was coined by Carolyn R. Bertozzi in 2003. Since its introduction, the concept of the bioorthogonal reaction has enabled the study of biomolecules such as glycans, proteins, and lipids in real time in living systems without cellular toxicity. A number of chemical ligation strategies have been developed that fulfill the requirements of bioorthogonality, including the 1,3-dipolar cycloaddition between azides and cyclooctynes (also termed copper-free click chemistry), between nitrones and cyclooctynes, oxime/hydrazone formation from aldehydes and ketones, the tetrazine ligation, the isocyanide-based click reaction, and most recently, the quadricyclane ligation.The use of bioorthogonal chemistry typically proceeds in two steps. First, a cellular substrate is modified with a bioorthogonal functional group (chemical reporter) and introduced to the cell; substrates include metabolites, enzyme inhibitors, etc. The chemical reporter must not alter the structure of the substrate dramatically to avoid affecting its bioactivity. Secondly, a probe containing the complementary functional group is introduced to react and label the substrate.Although effective bioorthogonal reactions such as copper-free click chemistry have been developed, development of new reactions continues to generate orthogonal methods for labeling to allow multiple methods of labeling to be used in the same biosystems.