Part II - American Chemical Society
... iii. (1) N is more electronegative that P, so electron density is shifted from H atoms towards the N, so the H+ can be more readily removed. (2) NO3– is stabilized by resonance more than H2PO4–. (3) HNO3 has two free oxygen atoms that attract electron density from the H atom, whereas H3PO4 has only ...
... iii. (1) N is more electronegative that P, so electron density is shifted from H atoms towards the N, so the H+ can be more readily removed. (2) NO3– is stabilized by resonance more than H2PO4–. (3) HNO3 has two free oxygen atoms that attract electron density from the H atom, whereas H3PO4 has only ...
Unit 9 - Kinetics and Equilibrium
... When AgNO3 is added to a salt solution of AgCl it is described as a source of a common ion, Ag+ ion. Common ion – ion that enters the solution from 2 different sources Common ion effect can be used to make an “insoluble” salt even less soluble ...
... When AgNO3 is added to a salt solution of AgCl it is described as a source of a common ion, Ag+ ion. Common ion – ion that enters the solution from 2 different sources Common ion effect can be used to make an “insoluble” salt even less soluble ...
1 Intro / Review : Chemical Kinetics
... Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions. Enduring understanding 4.A: Reaction rates that depend on temperature and other environmental factors are determined by measuring changes in concentrations of reactants or products over time. Essential kno ...
... Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions. Enduring understanding 4.A: Reaction rates that depend on temperature and other environmental factors are determined by measuring changes in concentrations of reactants or products over time. Essential kno ...
Thermodynamics PPT
... enthalpy). Absolute value for each substance can be determined. For a chemical system: S° = nS°(products) - mS°(reactants) where n and m are the coefficients in the balanced chemical equation. Standard Molar entropy, S0, is the entropy of one mole of a substance in its standard state (298 K ...
... enthalpy). Absolute value for each substance can be determined. For a chemical system: S° = nS°(products) - mS°(reactants) where n and m are the coefficients in the balanced chemical equation. Standard Molar entropy, S0, is the entropy of one mole of a substance in its standard state (298 K ...
Reaction Rate review questions
... Predict why step one should be slower than step two. Step one involves bond breakage while step 2 is bond formation. ...
... Predict why step one should be slower than step two. Step one involves bond breakage while step 2 is bond formation. ...
Topic 5 Energetics File
... Entropy: A measure of the disorder of a system. Things causing entropy to increase: 1) increase of number of moles of gaseous molecules; 2) change of state from solid to liquid or liquid to gas; 3) increase of temperature Exothermic: A reaction in which energy is evolved. ΔH is –. Products more stab ...
... Entropy: A measure of the disorder of a system. Things causing entropy to increase: 1) increase of number of moles of gaseous molecules; 2) change of state from solid to liquid or liquid to gas; 3) increase of temperature Exothermic: A reaction in which energy is evolved. ΔH is –. Products more stab ...
Oxidation - Reduction Chemistry
... Rules for assigning oxidation numbers 1. All elements in their free state (uncombined with other elements) have an oxidation number of zero (e.g., Na, Cu, Mg, H2, O2, Cl2, etc.) 2. H is +1, except in metal hydrides, where it is -1 (e.g., NaH, CaH2) 3. O is -2, except in peroxides, where it is -1, a ...
... Rules for assigning oxidation numbers 1. All elements in their free state (uncombined with other elements) have an oxidation number of zero (e.g., Na, Cu, Mg, H2, O2, Cl2, etc.) 2. H is +1, except in metal hydrides, where it is -1 (e.g., NaH, CaH2) 3. O is -2, except in peroxides, where it is -1, a ...
Questions
... III The acidic solution in the beaker was filtered into a 250 cm3 volumetric flask. A small amount of solid impurity remained in the filter paper. The solution in the volumetric flask was carefully made up to 250 cm3 with distilled water. IV A pipette was used to transfer 25.0 cm3 portions of the ac ...
... III The acidic solution in the beaker was filtered into a 250 cm3 volumetric flask. A small amount of solid impurity remained in the filter paper. The solution in the volumetric flask was carefully made up to 250 cm3 with distilled water. IV A pipette was used to transfer 25.0 cm3 portions of the ac ...
高雄醫學大學九十二學年度學士後醫學系招生考試試題 科目:化學 考試
... 66. Calculate the temperature at which the average kinetic energy of O2 gas is twice that of He gas at 10℃. (A) 2.50℃ (B) 10.0℃ (C) 20.0℃ (D) 160℃ (E) 293℃ 67. The sodium salt, NaA, of a weak acid is dissolved in water; no other substance is added. Which of the statements (to a close approximation) ...
... 66. Calculate the temperature at which the average kinetic energy of O2 gas is twice that of He gas at 10℃. (A) 2.50℃ (B) 10.0℃ (C) 20.0℃ (D) 160℃ (E) 293℃ 67. The sodium salt, NaA, of a weak acid is dissolved in water; no other substance is added. Which of the statements (to a close approximation) ...
Topic 3 MOLE Avodagro`s number = 6.02 x 1023 things = 1 mole 1
... a) How many grams of O2 are needed to burn 1.50 mole of octane? 1.5 mole octane (25mole O2 /2mole octane) (32 g /mole O2) = 600 g 12. One of the steps in the commercial process for converting ammonia to nitric acid involves the conversion of N H3 to NO: 4NH3 (g) + 5 O2 (g) 4NO (g) + 6 H2O (g) In a ...
... a) How many grams of O2 are needed to burn 1.50 mole of octane? 1.5 mole octane (25mole O2 /2mole octane) (32 g /mole O2) = 600 g 12. One of the steps in the commercial process for converting ammonia to nitric acid involves the conversion of N H3 to NO: 4NH3 (g) + 5 O2 (g) 4NO (g) + 6 H2O (g) In a ...
The effect of confinement on chemical reactions
... interaction between the reacting molecules and the adsorbent, causing the adsorbed phase to have a significantly higher density than the bulk phase. The combination of these two factors naturally causes an enhancement of the equilibrium yield, as the increased density of the adsorbed phase displaces ...
... interaction between the reacting molecules and the adsorbent, causing the adsorbed phase to have a significantly higher density than the bulk phase. The combination of these two factors naturally causes an enhancement of the equilibrium yield, as the increased density of the adsorbed phase displaces ...
CHAPTER I
... Copper, in Group IB, will also have one electron assigned to the 4s orbital, plus 28 other electrons assigned to other orbitals. The configuration of Be 1s2 2s2.All elements of Group 2A have electron configurations [electrons of preceding rare gas + ns2], where n is the period in which the element ...
... Copper, in Group IB, will also have one electron assigned to the 4s orbital, plus 28 other electrons assigned to other orbitals. The configuration of Be 1s2 2s2.All elements of Group 2A have electron configurations [electrons of preceding rare gas + ns2], where n is the period in which the element ...
CHAPTER 16
... numbers of molecules. They can be fractions when necessary. 2. The physical state of the product or reactant involved in a reaction is an important factor and, therefore, must be included in the thermochemical equation. 3. The change in enthalpy represented by a thermochemical equation is directly p ...
... numbers of molecules. They can be fractions when necessary. 2. The physical state of the product or reactant involved in a reaction is an important factor and, therefore, must be included in the thermochemical equation. 3. The change in enthalpy represented by a thermochemical equation is directly p ...
Reaction Energy
... • example: the Hf0 of carbon dioxide is –393.5 kJ per mol of gas produced. • Elements in their standard states are defined as having Hf0 = 0. • This indicates that carbon dioxide is more stable than the elements from which it was formed. ...
... • example: the Hf0 of carbon dioxide is –393.5 kJ per mol of gas produced. • Elements in their standard states are defined as having Hf0 = 0. • This indicates that carbon dioxide is more stable than the elements from which it was formed. ...
Chemistry Entrance Material for Grade 10 to 11 Answer Key
... 9. Which one of the following is TRUE when a liquid is cooled? [-A-] A plot of temperature versus distance can be drawn. [-B-] A plot of temperature versus time can be drawn. [-C-] Energy is released at an increasing rate. [-D-] Energy is released at a constant rate. Comparing cooling curves of 2 sa ...
... 9. Which one of the following is TRUE when a liquid is cooled? [-A-] A plot of temperature versus distance can be drawn. [-B-] A plot of temperature versus time can be drawn. [-C-] Energy is released at an increasing rate. [-D-] Energy is released at a constant rate. Comparing cooling curves of 2 sa ...
Chapter 4 Chemical Quantities and Aqueous Reactions
... - acids ionize in water to form H+ ions. More precisely, the H from the acid molecule is donated to a water molecule to form hydronium ion, H3O+. Most chemists use H+ and H3O+ interchangeably. - bases dissociate in water to form OH ions. Bases, like NH3, that do not contain OH ions, produce O ...
... - acids ionize in water to form H+ ions. More precisely, the H from the acid molecule is donated to a water molecule to form hydronium ion, H3O+. Most chemists use H+ and H3O+ interchangeably. - bases dissociate in water to form OH ions. Bases, like NH3, that do not contain OH ions, produce O ...
chem equation Pkt Student2
... 1) Which side of the yields arrow do you find reactants? ______________________________ 2) Which side of the yields arrow do you find products? _______________________________ 3) In a chemical equation, what do the coefficients represent? ______________________________ 4) In a chemical equation, wha ...
... 1) Which side of the yields arrow do you find reactants? ______________________________ 2) Which side of the yields arrow do you find products? _______________________________ 3) In a chemical equation, what do the coefficients represent? ______________________________ 4) In a chemical equation, wha ...
Topic 6 Kinetics File
... 6. It has been found that the rates of many reactions are doubled by a 10-degree C rise in temperature. The main reason for this is that A. the energy of activation decreases with temperature. B. the energy of activation increases with temperature. C. the speed of molecules is dramatically increase ...
... 6. It has been found that the rates of many reactions are doubled by a 10-degree C rise in temperature. The main reason for this is that A. the energy of activation decreases with temperature. B. the energy of activation increases with temperature. C. the speed of molecules is dramatically increase ...
0922085
... The mass of 180 litres of UN No. 1092 ACROLEINE is 144 kg. What is the relative density of the substance? A ...
... The mass of 180 litres of UN No. 1092 ACROLEINE is 144 kg. What is the relative density of the substance? A ...
QUESTION BANK CHEMISTRY-XII THE SOLID STATE CHAPTER
... 12. How fluoride can be converted to fluorine? 13. Suggest two materials other than hydrogen that can be used as fuels in fuel cells. 14. Rusting of iron is quicker in saline water than in ordinary water. Why is it so? 15. Express mathematically relationship among the resistance specifi ...
... 12. How fluoride can be converted to fluorine? 13. Suggest two materials other than hydrogen that can be used as fuels in fuel cells. 14. Rusting of iron is quicker in saline water than in ordinary water. Why is it so? 15. Express mathematically relationship among the resistance specifi ...
8872 Chemistry H1 syllabus for 2016
... (a) explain, in terms of rates of the forward and reverse reactions, what is meant by a reversible reaction and dynamic equilibrium (b) state Le Chatelier’s Principle and apply it to deduce qualitatively (from appropriate information) the effects of changes in concentration, pressure or temperature, ...
... (a) explain, in terms of rates of the forward and reverse reactions, what is meant by a reversible reaction and dynamic equilibrium (b) state Le Chatelier’s Principle and apply it to deduce qualitatively (from appropriate information) the effects of changes in concentration, pressure or temperature, ...
Electrolysis of water
Electrolysis of water is the decomposition of water (H2O) into oxygen (O2) and hydrogen gas (H2) due to an electric current being passed through the water.This technique can be used to make hydrogen fuel (hydrogen gas) and breathable oxygen; though currently most industrial methods make hydrogen fuel from natural gas instead.