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This document discusses the relationship between kinetics and the equilibrium constant K for chemical reactions. It explains that at equilibrium, the forward and backward reaction rates are equal. The equilibrium constant K is derived by setting the forward and backward rate equations equal to each other and solving for the ratio of the rate constants. K represents the fundamental connection between reaction kinetics and the equilibrium state.
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This document provides information on naming and writing formulas for various types of chemical compounds including:
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Chemistry - Chp 16 - Solutions - PowerPoint (shortened)
The document discusses key concepts about solutions, including:
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This document discusses the relationship between kinetics and the equilibrium constant K for chemical reactions. It explains that at equilibrium, the forward and backward reaction rates are equal. The equilibrium constant K is derived by setting the forward and backward rate equations equal to each other and solving for the ratio of the rate constants. K represents the fundamental connection between reaction kinetics and the equilibrium state.
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2) Solubility is defined as the maximum amount of solute that will dissolve at a specific temperature, and can be expressed in units like grams of solute per 100 grams of solvent.
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The document discusses chemical reactions and stoichiometry. It defines stoichiometry as using ratios to determine quantities of reactants and products in a chemical reaction. It explains that coefficients in a balanced chemical equation represent molar ratios and can be used to determine moles, mass, and volume of substances in a reaction. It provides examples of solving stoichiometry problems, including determining limiting reactants.
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1. Chemical reactions involve chemical changes that result in the formation of new substances.
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3. There are several types of chemical reactions including combination, decomposition, displacement, and oxidation-reduction. Combination reactions involve elements or compounds reacting to form a single product, while decomposition reactions involve a single reactant breaking down into simpler products.
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Acids and bases can be defined operationally based on experimental observations or conceptually based on theories. Operationally, acids are sour electrolytes that turn litmus red and react with metals, while bases are bitter electrolytes that turn litmus blue. Conceptually, acids are proton donors according to Arrhenius and Bronsted-Lowry, or electron pair acceptors according to Lewis. Conjugate acid-base pairs involve the transfer of a proton between an acid and its conjugate base. The strength of an acid or base depends on its tendency to donate or accept protons.
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This document discusses autoionization of water and concepts related to acid-base chemistry including:
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- Solutions can be classified as neutral, acidic, or basic based on the relative concentrations of H3O+ and OH-.
- Strong acids and bases completely ionize in solution, allowing their concentrations to determine H3O+ or OH- concentrations.
- Weak acids and bases only partially ionize in solution, with their extent of dissociation determined by their acid or base ionization constant (Ka or Kb).
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The document discusses chemical reactions and stoichiometry. It defines stoichiometry as using ratios to determine quantities of reactants and products in a chemical reaction. It explains that coefficients in a balanced chemical equation represent molar ratios and can be used to determine moles, mass, and volume of substances in a reaction. It provides examples of solving stoichiometry problems, including determining limiting reactants.
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2. Several gas laws are described, including Boyle's law, Charles' law, Avogadro's law, and Dalton's law of partial pressures. Standard temperature and pressure is defined.
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The gas laws complete
1) Boyle's law states that the volume of a gas is inversely proportional to its pressure when temperature is kept constant. Charles' law describes the direct relationship between volume and temperature of a gas at constant pressure. Gay-Lussac's law explains that pressure of a gas rises with increasing temperature at constant volume.
2) The combined gas law incorporates Boyle's, Charles's and Gay-Lussac's laws to describe the interrelationships between pressure, volume and temperature for a fixed amount of gas.
3) According to Avogadro's law, equal volumes of gases under same conditions of temperature and pressure contain equal numbers of molecules. Dalton's law states that total pressure of a gas mixture is the sum
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Introduces the 5 types of chemical reactions: synthesis, decomposition, single and double replacement, and combustion.
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Chemistry of solutions
This document discusses chemistry of solutions. It defines key terms like solute, solvent and solution. It explains that a solution is a homogeneous mixture of two or more substances. The solute is dispersed uniformly throughout the solvent. Factors that affect solubility are also discussed, like temperature, pressure, molecular size and polarity. Henry's law is introduced, which states that the solubility of a gas is directly proportional to its partial pressure.
Solution & Solubility
A solution is a homogeneous mixture of two or more substances, where the solute is dispersed uniformly throughout the solvent. The solubility of a solute is dependent on temperature, pressure, and the nature of the solute and solvent. Solubility is expressed as the maximum grams of solute that will dissolve per 100 grams of solvent. Colligative properties, such as boiling point elevation and freezing point depression, depend only on the number of solute particles and not their identity.
Different types of chemical reactions(ppt)
Utkarsh Singh presented on the different types of chemical reactions. There are several types including combination reactions, decomposition reactions, displacement reactions, and double displacement reactions. Combination reactions involve elements or compounds combining to form a new substance. Decomposition reactions involve breaking a substance down into simpler substances. Displacement reactions involve one element replacing another in a compound. Double displacement reactions involve ion exchange between two ionic compounds. Oxidation-reduction reactions involve the transfer of electrons between reactants. Exothermic reactions release heat while endothermic reactions absorb heat from their surroundings.
CHEMICAL EQUATIONS AND REACTIONS
1. Chemical reactions involve chemical changes that result in the formation of new substances.
2. Chemical equations are used to represent chemical reactions, with reactants on the left side of the arrow and products on the right. These equations must be balanced and follow the law of conservation of mass.
3. There are several types of chemical reactions including combination, decomposition, displacement, and oxidation-reduction. Combination reactions involve elements or compounds reacting to form a single product, while decomposition reactions involve a single reactant breaking down into simpler products.
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This document appears to contain grade data for a first semester chemistry class of 30 students. It lists the percentage scores and letter grades for four topics: charm, electron, photon, and truth. The percentage scores range from 43.48% to 106% while the letter grades range from 1 to 4, with lower numbers indicating better performance. The data is presented numerically by student number for each of the four topics.
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This document describes two methods for balancing redox reactions:
1. The oxidation number method which involves assigning oxidation numbers, identifying the reducing and oxidizing agents, computing electrons lost and gained, and balancing the reaction.
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Acids and bases can be defined operationally based on experimental observations or conceptually based on theories. Operationally, acids are sour electrolytes that turn litmus red and react with metals, while bases are bitter electrolytes that turn litmus blue. Conceptually, acids are proton donors according to Arrhenius and Bronsted-Lowry, or electron pair acceptors according to Lewis. Conjugate acid-base pairs involve the transfer of a proton between an acid and its conjugate base. The strength of an acid or base depends on its tendency to donate or accept protons.
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This document discusses autoionization of water and concepts related to acid-base chemistry including:
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- Weak acids and bases only partially ionize in solution, with their extent of dissociation determined by their acid or base ionization constant (Ka or Kb).
Risk and hazard
Risk refers to the chance that harm will occur from a hazard, requiring both a hazard and exposure to be present. Hazard refers to the intrinsic ability of a situation or substance to cause harm. For a risk to exist, there must be not only a hazard but also exposure to that hazard. An example is given of a dangerous animal that is a hazard when free but presents no risk when caged, since there is then no exposure. Risk assessment considers both the hazard and likelihood of exposure to determine if and how harm might occur from a given situation.
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Chem Eq Lec1
- 1. Chemical Equilibrium Presentation Part 1 c!e-γ˚T 2010
- 2. Equilibrium – “balance of force”
- 7. k1 CO(g) + 2 H2(g) CH3OH(g) k-1 [CH3OH] [CH3OH] [CH3OH] [CO][H2]2 [CO][H2] [CO](2[H2]) 14.2 M-2 0.596 M-1 1.19 M-1 14.2 M-2 1.09 M-1 2.17 M-1 14.2 M-2 1.28 M-1 2.55 M-1
- 10. KEQ from Rate Law The following equations show how KEQ expression can be derived from the Rateforward = Ratereverse. Forward reaction: N2O4 (g) 2 NO2 (g) Rate law: Rate = kf [N2O4] Reverse reaction: 2 NO2 (g) N2O4 (g) Rate law: Rate = kr [NO2]2 Therefore, at equilibrium, Ratef = Rater kf [N2O4] = kr [NO2]2 Rewriting, it becomes
- 11. Rules in writing KEQ and Q expression amounts is be expressed in terms of molar concentration (for both aqueous and gas) or partial pressure (gas). products are always in the numerator, and the reactants are always in the denominator Coefficients in the chemical equations are the exponents used in the expression The stoichiometric coefficient of each molecule or compound is used in place of the experimentally determined exponents because the reaction is assumed to occur at a fast reversible single step. solids and liquids are not included in the expression, why? unit less
- 12. Practice writing KCand KP expression for the following reactions: formation of ozone from oxygen gas formation of ammonia from nitrogen and hydrogen gas decomposition of phosphorus pentachloride into phosphorus trichloride and chlorine gas formation of sulphur trioxide from oxygen and sulphur dioxide reaction of the aqueous sodium carbonate and calcium chloride to form solid calcium carbonate and sodium chloride solution decomposition of solid calcium carbonate into lime and carbon dioxide
Editor's Notes
- Mechanical, thermal, chemical equilibrium
- Equilibrium is reached from either direction
- magnitude