General Equilibrium FR worksheet
... experiment, the following equilibrium concentrations were measured. [H2] = 0.20 mol/L [CO2] = 0.30 mol/L [H2O] = [CO] = 0.55 mol/L (a) What is the mole fraction of CO(g) in the equilibrium mixture? (b) Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium const ...
... experiment, the following equilibrium concentrations were measured. [H2] = 0.20 mol/L [CO2] = 0.30 mol/L [H2O] = [CO] = 0.55 mol/L (a) What is the mole fraction of CO(g) in the equilibrium mixture? (b) Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium const ...
Notes - Text
... • Tabulate initial and equilibrium concentrations (or partial pressures) for all species in the equilibrium. • If an initial and an equilibrium concentration is given for a species, calculate the change in concentration. • Use the coefficients in the balanced chemical equation to calculate the chang ...
... • Tabulate initial and equilibrium concentrations (or partial pressures) for all species in the equilibrium. • If an initial and an equilibrium concentration is given for a species, calculate the change in concentration. • Use the coefficients in the balanced chemical equation to calculate the chang ...
File - Prairie Science
... that transfers from one object to another, because of a temperature difference between them. How does heat travel? ...
... that transfers from one object to another, because of a temperature difference between them. How does heat travel? ...
The masses of reactants and products are equal.
... An example of Lavoisier’s work is his study of the reaction of the metal mercury when heated in air. In this reaction, the reddishorange product formed has more mass than the original metal. Lavoisier placed some mercury in a jar, sealed the jar, and recorded the total mass of the setup. After the m ...
... An example of Lavoisier’s work is his study of the reaction of the metal mercury when heated in air. In this reaction, the reddishorange product formed has more mass than the original metal. Lavoisier placed some mercury in a jar, sealed the jar, and recorded the total mass of the setup. After the m ...
problem 8 on 2003B exam
... (c) Determine the equilibrium concentrations of H2(g) and I2(g). (d) On the graph above, make a sketch that shows how the concentration of H2(g) changes as a function of time. (e) Calculate the value of the following equilibrium constants at 700. K. (i) Kc (ii) Kp (f) At 1,000 K, the value of Kc for ...
... (c) Determine the equilibrium concentrations of H2(g) and I2(g). (d) On the graph above, make a sketch that shows how the concentration of H2(g) changes as a function of time. (e) Calculate the value of the following equilibrium constants at 700. K. (i) Kc (ii) Kp (f) At 1,000 K, the value of Kc for ...
Objective: The objective of the lab is to study the types of reactions
... A dissociation reaction is one that forms ions. If a molecule is made up on ions it might be able to be dissolved in water. Table salt (NaCl) is an example of a compound that is easily split into the Na+1 and the Cl-1 ions that make it up. Ions are charged particles that are very much similar to an ...
... A dissociation reaction is one that forms ions. If a molecule is made up on ions it might be able to be dissolved in water. Table salt (NaCl) is an example of a compound that is easily split into the Na+1 and the Cl-1 ions that make it up. Ions are charged particles that are very much similar to an ...
184
... methods.5 The reaction path and potential energy surface were obtained by CASSCF and MRCI calculations with large, correlation consistent basis sets. The theoretical rate constant and activation energy are in excellent agreement with experiment. The rates for BCl + H, BCl + Cl, BH + H, BH + Cl, and ...
... methods.5 The reaction path and potential energy surface were obtained by CASSCF and MRCI calculations with large, correlation consistent basis sets. The theoretical rate constant and activation energy are in excellent agreement with experiment. The rates for BCl + H, BCl + Cl, BH + H, BH + Cl, and ...
South Pasadena · AP Chemistry
... Suppose that 0.50 moles of hydrogen gas, 0.50 moles of iodine gas, and 0.75 moles of hydrogen iodide gas are introduced into a 2.0 Liter vessel and the system is allowed to reach equilibrium. H2(g) + I2(g) 2 HI(g) Calculate the concentrations of all three substances at equilibrium. At the temperatur ...
... Suppose that 0.50 moles of hydrogen gas, 0.50 moles of iodine gas, and 0.75 moles of hydrogen iodide gas are introduced into a 2.0 Liter vessel and the system is allowed to reach equilibrium. H2(g) + I2(g) 2 HI(g) Calculate the concentrations of all three substances at equilibrium. At the temperatur ...
SCI 3101 Test IV MULTIPLE CHOICE. 1) The sky is blue because air
... B) number of times each element appears as a reactant is equal to the number of times it appears as a product. C) subscripts on both sides of the reaction add up to the same number. D) number of molecules of reactants and products are equal. ...
... B) number of times each element appears as a reactant is equal to the number of times it appears as a product. C) subscripts on both sides of the reaction add up to the same number. D) number of molecules of reactants and products are equal. ...
PPT
... The atmosphere does not collapse under the downward pull of gravity because of the energy embedded in the movement of the air molecules. This movement creates the force of pressure which counters the gravitational pull on the atmosphere. The balance between the force of pressure and gravity is the h ...
... The atmosphere does not collapse under the downward pull of gravity because of the energy embedded in the movement of the air molecules. This movement creates the force of pressure which counters the gravitational pull on the atmosphere. The balance between the force of pressure and gravity is the h ...
THERMOCHEMISTRY or Thermodynamics
... This equation is valid because ∆H is a STATE FUNCTION These depend only on the state of the system and not how it got there. V, T, P, energy — and your bank account! Unlike V, T, and P, one cannot measure absolute H. Can only measure ∆H. ...
... This equation is valid because ∆H is a STATE FUNCTION These depend only on the state of the system and not how it got there. V, T, P, energy — and your bank account! Unlike V, T, and P, one cannot measure absolute H. Can only measure ∆H. ...
Thermodynamic Properties of Hydrated and Ammoniated Electrons
... coefficient of AHOII. Further insight into the nature of the temperature coefficient of AGfoe,,- is based on the following consideration. Both - (dGoe,,-/&-) and - (dGf0,,,-/i3T) are equal to Soe,,-, the standard entropy of the ammoniated electron. The large positive value of Soe,,- gives rise t o t ...
... coefficient of AHOII. Further insight into the nature of the temperature coefficient of AGfoe,,- is based on the following consideration. Both - (dGoe,,-/&-) and - (dGf0,,,-/i3T) are equal to Soe,,-, the standard entropy of the ammoniated electron. The large positive value of Soe,,- gives rise t o t ...
Cl Cl and
... Too much energy is needed to remove 4 electrons from an atom. Too much energy is needed to insert 4 electrons into an atom in order to overcome the repulsive forces between like charges. 28. Why do elements of groups 6 and 7 form ions of charge –2 and –1 respectively? By gaining electrons they achie ...
... Too much energy is needed to remove 4 electrons from an atom. Too much energy is needed to insert 4 electrons into an atom in order to overcome the repulsive forces between like charges. 28. Why do elements of groups 6 and 7 form ions of charge –2 and –1 respectively? By gaining electrons they achie ...
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.