'Reaction proceeds' presentation slideshows

Rates of Chemical Reactions

Rates of Chemical Reactions. Consider this reaction:. N 2 (g) + 3H 2 (g) ----> 2 NH 3 (g) + 92 kJ D G 298K = -16.8 kJ. What does this equation tell us?. N 2 (g) + 3H 2 (g) ----> 2 NH 3 (g) + 92 kJ D G 298K = -16.8 kJ. The reaction is spontaneous at 298K It is exothermic

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Unit 14: Thermochemistry

Chemistry. Unit 14: Thermochemistry. So how does this relate to a chemical equation?. Heat of Reaction: is the quantity of heat released or absorbed during a chemical reaction. It is really just the different between the stored energy of the reactants and the products.

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Keeping Track of Energy During Chemical Change

Keeping Track of Energy During Chemical Change. A coherent way to treat energy in chemical reactions. The Conventional Approach. Treatment of energy in reactions is vague Where/how is energy stored is left unanswered How energy is transferred between system and surroundings is ignored.

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Lecture 18. Chemical Reactions (Ch. 5)

Lecture 18. Chemical Reactions (Ch. 5). In chemical reactions, the products of reaction are intermixed with the reacting substances (reactants). Thus, the process is governed by two factors: (a) the energy change ( V,T=const ) or enthalpy change ( T,P=const ), and (b) the entropy change:.

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Chapter 20: Electrochemistry

Chapter 20: Electrochemistry. Juana Mendenhall, Ph.D. Assistant Professor Lecture 2 March 15. Objectives. Describe and illustrate how a voltaic cell operates, with the concepts of electrodes, salt bridges, half-cell equations, net cell reaction and cell diagram.

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Lecture 18. Chemical Reactions (Ch. 5)

Lecture 18. Chemical Reactions (Ch. 5). In chemical reactions, the products of reaction are intermixed with the reacting substances (reactants). Thus, the process is governed by two factors: (a) the energy change ( V,T=const ) or enthalpy change ( T,P=const ), and (b) the entropy change:.

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Equilibrium

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Chapter 15 Kinetics

Chapter 15 Kinetics. 15.1 Rates of Chemical Reactions 15.2 Reaction Conditions and Rate 15.3 Effect of Concentration on Reaction Rate 15.4 The Relationship between Concentration and Time 15.5 A Molecular View of Reactions 15.6 Reaction Mechanisms. Rates of Chemical Reactions.

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Keq vs. Q

Keq vs. Q. Monsurat Olaosebikan Nicole Gomez Johan Mann. K eq. K eq is the equilibrium constant which measures the extent to which a reaction proceeds to completion. Q. Q is the reaction quotient used to determine if the reaction is at equilibrium. Equations!. K eq = [C] c [D] d

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Spontaneous vs. Non-Spontaneous

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Weak Acid pH Curve

Weak Acid pH Curve. Henderson Hasslebach Equation: At first [salt] is very low, [acid] is high. As reaction proceeds, initially log [salt]/[acid] changes dramatically and hence so does pH But as [salt] and [acid] approach parity log [salt]/[acid] changes only slightly and hence so does pH.

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