Measurements/Unit Cancellation/Significant Figures 1. When
... Concentration: The measure of the quantity of a solute dissolved in a given quantity of solution. Dilute Solution: A solution that contains a small amount of solute relative to the amount that could dissolve. Electrolyte: A substance that conducts a current when it dissolves in water. Empirical form ...
... Concentration: The measure of the quantity of a solute dissolved in a given quantity of solution. Dilute Solution: A solution that contains a small amount of solute relative to the amount that could dissolve. Electrolyte: A substance that conducts a current when it dissolves in water. Empirical form ...
Chap15 - Bakersfield College
... Predicting the Direction of Reaction • How could we predict the direction in which a reaction at non-equilibrium conditions will shift to reestablish equilibrium? – To answer this question, substitute the current concentrations into the reaction quotient expression and compare it to Kc. – The react ...
... Predicting the Direction of Reaction • How could we predict the direction in which a reaction at non-equilibrium conditions will shift to reestablish equilibrium? – To answer this question, substitute the current concentrations into the reaction quotient expression and compare it to Kc. – The react ...
Chem 1411 Chapter 4
... Oxidation and Reduction Reactions An oxidation reaction is the one that involves loss of electrons and a reduction reaction involves the gain of electrons. A reaction in which oxidation and reduction occurs simultaneously is called a redox reaction. The species that undergoes oxidation is the reduct ...
... Oxidation and Reduction Reactions An oxidation reaction is the one that involves loss of electrons and a reduction reaction involves the gain of electrons. A reaction in which oxidation and reduction occurs simultaneously is called a redox reaction. The species that undergoes oxidation is the reduct ...
Name_____________________________________ Chemistry
... 78. List 4 types of chemical reactions: a. b. c. d. 79. a. A + B → AB is an example of a(n) ____________________________ reaction. b. AB → A + B is an example of a(n) ____________________________ reaction. c. A + BC → AC + B is an example of a(n) ____________________________ reaction. d. AB + CD → A ...
... 78. List 4 types of chemical reactions: a. b. c. d. 79. a. A + B → AB is an example of a(n) ____________________________ reaction. b. AB → A + B is an example of a(n) ____________________________ reaction. c. A + BC → AC + B is an example of a(n) ____________________________ reaction. d. AB + CD → A ...
Thermodynamics - WordPress.com
... ΔH = ΔHbonds broken + ΔHbonds formed = 2648 kJ - 3330 kJ = -682 kJ The reaction is exothermic since enthalpy change is -682 kJ for 2 mol of methane, CH4, that is, -682 kJ/mol. Refer to your textbook p. 159 for an energy balance diagram of this reaction. NOTE: You may use ΔH = ΔHbonds broken - ΔHbond ...
... ΔH = ΔHbonds broken + ΔHbonds formed = 2648 kJ - 3330 kJ = -682 kJ The reaction is exothermic since enthalpy change is -682 kJ for 2 mol of methane, CH4, that is, -682 kJ/mol. Refer to your textbook p. 159 for an energy balance diagram of this reaction. NOTE: You may use ΔH = ΔHbonds broken - ΔHbond ...
Lecture Notes in Physical Chemistry Semester 2: Kinetics and
... is mv x . When the molecule collides with a wall parallel to the y z plane, let us assume that the x component of its velocity changes sign, and the other two components are unaffected. (This assumption corresponds to a “specular reflection”, like light off a mirror. It is not necessarily true for a ...
... is mv x . When the molecule collides with a wall parallel to the y z plane, let us assume that the x component of its velocity changes sign, and the other two components are unaffected. (This assumption corresponds to a “specular reflection”, like light off a mirror. It is not necessarily true for a ...
2 Combustion in Gas
... Note that in the second case (Tables 2-3 and 2-4), N2 can be considered as either an added diluent (Table 2-3), or a component of the oxidizer, i.e., air (Table 2-4). If it is considered part of the oxidizer then it must be included in the complete-combustion products list. Also, the oxidizer compos ...
... Note that in the second case (Tables 2-3 and 2-4), N2 can be considered as either an added diluent (Table 2-3), or a component of the oxidizer, i.e., air (Table 2-4). If it is considered part of the oxidizer then it must be included in the complete-combustion products list. Also, the oxidizer compos ...
2005 - NESACS
... 42. The hydrogen emission spectrum for galaxy NGC 3310 is shown below. Marked on the spectrum with a vertical line is the red hydrogen emission line, Hα, at 6562.8 Å (656.2 nm) that originates from the Balmer series (32) at the spot where it would be found in a hydrogen spectrum produced in a labor ...
... 42. The hydrogen emission spectrum for galaxy NGC 3310 is shown below. Marked on the spectrum with a vertical line is the red hydrogen emission line, Hα, at 6562.8 Å (656.2 nm) that originates from the Balmer series (32) at the spot where it would be found in a hydrogen spectrum produced in a labor ...
College Chemistry I PHS 1025 Fall 2012 Practice Exam 3A
... 25) Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ___ NH3(g) + ___ O2(g) → ___ NO(g) + ___ H2O(l) A) 18.8 L ...
... 25) Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ___ NH3(g) + ___ O2(g) → ___ NO(g) + ___ H2O(l) A) 18.8 L ...
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C2_revision_slides_V3_+_questions_+_MS_-_H[1]
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
Ionic bonding
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
Ionic bonding - Animated Science
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
2002 local exam - Virginia Section
... The answers for questions 4 through 7 follow. Select the lettered choice that best fits the statement for each question and fill in the corresponding block on the answer sheet. You may use a choice more than once, once, or not at all. (A) density (B) equilibrium constant (C) freezing point (D) molar ...
... The answers for questions 4 through 7 follow. Select the lettered choice that best fits the statement for each question and fill in the corresponding block on the answer sheet. You may use a choice more than once, once, or not at all. (A) density (B) equilibrium constant (C) freezing point (D) molar ...
Revision Y12 Chemistry PLC
... Hess’ law and enthalpy cycles (g) Hess’ law for construction of enthalpy cycles and calculations to determine indirectly: (i) i) an enthalpy change of reaction from enthalpy changes of combustion (ii) ii) an enthalpy change of reaction from enthalpy changes of formation (iii iii) enthalpy changes fr ...
... Hess’ law and enthalpy cycles (g) Hess’ law for construction of enthalpy cycles and calculations to determine indirectly: (i) i) an enthalpy change of reaction from enthalpy changes of combustion (ii) ii) an enthalpy change of reaction from enthalpy changes of formation (iii iii) enthalpy changes fr ...
Transition state theory
Transition state theory (TST) explains the reaction rates of elementary chemical reactions. The theory assumes a special type of chemical equilibrium (quasi-equilibrium) between reactants and activated transition state complexes.TST is used primarily to understand qualitatively how chemical reactions take place. TST has been less successful in its original goal of calculating absolute reaction rate constants because the calculation of absolute reaction rates requires precise knowledge of potential energy surfaces, but it has been successful in calculating the standard enthalpy of activation (Δ‡Hɵ), the standard entropy of activation (Δ‡Sɵ), and the standard Gibbs energy of activation (Δ‡Gɵ) for a particular reaction if its rate constant has been experimentally determined. (The ‡ notation refers to the value of interest at the transition state.)This theory was developed simultaneously in 1935 by Henry Eyring, then at Princeton University, and by Meredith Gwynne Evans and Michael Polanyi of the University of Manchester. TST is also referred to as ""activated-complex theory,"" ""absolute-rate theory,"" and ""theory of absolute reaction rates.""Before the development of TST, the Arrhenius rate law was widely used to determine energies for the reaction barrier. The Arrhenius equation derives from empirical observations and ignores any mechanistic considerations, such as whether one or more reactive intermediates are involved in the conversion of a reactant to a product. Therefore, further development was necessary to understand the two parameters associated with this law, the pre-exponential factor (A) and the activation energy (Ea). TST, which led to the Eyring equation, successfully addresses these two issues; however, 46 years elapsed between the publication of the Arrhenius rate law, in 1889, and the Eyring equation derived from TST, in 1935. During that period, many scientists and researchers contributed significantly to the development of the theory.