Chapter 1 Chemistry: The Study of Matter
... Potential- stored energy Kinetic Energy- energy something has because its moving Heat- the energy that moves because of a temperature difference. Chemical energy- energy released or absorbed in a chemical change. Electrical energy - energy of moving ...
... Potential- stored energy Kinetic Energy- energy something has because its moving Heat- the energy that moves because of a temperature difference. Chemical energy- energy released or absorbed in a chemical change. Electrical energy - energy of moving ...
Energy Transformation
... -- Energy can be transferred from one object or system to another through the interaction of forces between the objects -- Energy comes in multiple forms: kinetic, potential, thermal (heat), chemical, electromagnetic, and nuclear energy. ...
... -- Energy can be transferred from one object or system to another through the interaction of forces between the objects -- Energy comes in multiple forms: kinetic, potential, thermal (heat), chemical, electromagnetic, and nuclear energy. ...
Enzymes: “Helper” Protein molecules
... Enzymes aren’t used up Enzymes are not changed by the reaction used only temporarily re-used again for the same reaction with other molecules very little enzyme needed to help in many reactions ...
... Enzymes aren’t used up Enzymes are not changed by the reaction used only temporarily re-used again for the same reaction with other molecules very little enzyme needed to help in many reactions ...
Physical Properties
... A chemical property indicates whether and sometimes how readily a material undergoes a chemical change with another material. For example, a chemical property of hydrogen gas is that it reacts vigorously with oxygen gas. ...
... A chemical property indicates whether and sometimes how readily a material undergoes a chemical change with another material. For example, a chemical property of hydrogen gas is that it reacts vigorously with oxygen gas. ...
Chem 1711 Review Exam 2
... Enthalpy, ΔH: equate enthalpy change for a process to energy change for that process if it occurs at constant P; ΔH = qP ΔH = Hfinal — Hinitial ΔH associated with physical changes: ΔHvap, ΔHfus, ΔHsub where vap = vaporization, (g l), fus = fusion (l s), sub = sublimation (s g). This is not in ...
... Enthalpy, ΔH: equate enthalpy change for a process to energy change for that process if it occurs at constant P; ΔH = qP ΔH = Hfinal — Hinitial ΔH associated with physical changes: ΔHvap, ΔHfus, ΔHsub where vap = vaporization, (g l), fus = fusion (l s), sub = sublimation (s g). This is not in ...
IB:Enthalpy Review Questions
... c. Identify a thermodynamic function that can be used to predict reaction spontaneity, at 25 OC. Determine the value of this function, stating its units, and state the meaning of the sign obtained. Is CuSO4. 5H2O(s) or CuSO4. H2O(s) is more stable at 25 OC? d. Determine the Centigrade temperature ab ...
... c. Identify a thermodynamic function that can be used to predict reaction spontaneity, at 25 OC. Determine the value of this function, stating its units, and state the meaning of the sign obtained. Is CuSO4. 5H2O(s) or CuSO4. H2O(s) is more stable at 25 OC? d. Determine the Centigrade temperature ab ...
Chemical Kinetics
... Two key points 1. The concentration of the products do not appear in the rate law because this is an initial rate. 2. The order (exponent) must be determined experimentally, can’t be obtained from the equation ...
... Two key points 1. The concentration of the products do not appear in the rate law because this is an initial rate. 2. The order (exponent) must be determined experimentally, can’t be obtained from the equation ...
Thermodynamics I
... The reaction is complete and 393.5 kJ of heat is released, thus by definition, DHfo(CO2, g) = -393.5 kJ • However, for other compounds, it is more difficult to find DHfo because the direct synthesis of the compound from its elements in their standard states is impossible e.g.; The reaction: C(graphi ...
... The reaction is complete and 393.5 kJ of heat is released, thus by definition, DHfo(CO2, g) = -393.5 kJ • However, for other compounds, it is more difficult to find DHfo because the direct synthesis of the compound from its elements in their standard states is impossible e.g.; The reaction: C(graphi ...
3.0 Hess`s Law
... • The basis for calculating enthalpies of reaction is 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 ta ...
... • The basis for calculating enthalpies of reaction is 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 ta ...
study packet for chapter 5
... B) is the sum of the rotational, vibrational, and translational energies of all of its components C) refers only to the energies of the nuclei of the atoms of the component molecules D) is the sum of the potential and kinetic energies of the components E) none of the above ...
... B) is the sum of the rotational, vibrational, and translational energies of all of its components C) refers only to the energies of the nuclei of the atoms of the component molecules D) is the sum of the potential and kinetic energies of the components E) none of the above ...
use-2012_review_sheettest_form_c_reactions
... Write a balanced equation if a reaction happens. Otherwise, write “no reaction.” a. Lead is placed into an iron (III) nitrate solution. b. Magnesium is dipped into a nickel (II) chloride solution. ...
... Write a balanced equation if a reaction happens. Otherwise, write “no reaction.” a. Lead is placed into an iron (III) nitrate solution. b. Magnesium is dipped into a nickel (II) chloride solution. ...
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.