Review of Chemical Thermodynamics 7.51 September 1999 ∆G
... ∆G — Change in free energy between reactants and products; this measures the ability of the system to do work. Reactions with negative ∆G’s proceed spontaneously and can be used to do work. Reactions with positive ∆G’s require an input of energy for the reaction to proceed. ∆H — Change in enthalpy b ...
... ∆G — Change in free energy between reactants and products; this measures the ability of the system to do work. Reactions with negative ∆G’s proceed spontaneously and can be used to do work. Reactions with positive ∆G’s require an input of energy for the reaction to proceed. ∆H — Change in enthalpy b ...
Document
... 1. The concentrations of the reacting species in the condensed phase are expressed in M. In the gaseous phase, the concentrations can be expressed in M or in atm. 2. The concentrations of pure solids, pure liquids and solvents do not appear in the equilibrium constant expressions. 3. The equilibrium ...
... 1. The concentrations of the reacting species in the condensed phase are expressed in M. In the gaseous phase, the concentrations can be expressed in M or in atm. 2. The concentrations of pure solids, pure liquids and solvents do not appear in the equilibrium constant expressions. 3. The equilibrium ...
13AP General Equilibrium FR worksheet (missing 1988)
... 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 ...
Advanced Placement Chemistry: 1984 Free Response Questions
... liquid in the radiator will either freeze or boil. ...
... liquid in the radiator will either freeze or boil. ...
Equilibrium 5
... 8. Gaseous HI is prepared from hydrogen gas and iodine vapor at a temperature where the equilibrium constant is 1.00 x 102. Suppose 5.0 x 10-1 atm of HI, 1.0 x 10-2 atm of H2 , and 5.0 x 10-3 atm of I2 are mixed inside a 5.0-L flask. Calculate the equilibrium pressure of all species. H2 (g) ...
... 8. Gaseous HI is prepared from hydrogen gas and iodine vapor at a temperature where the equilibrium constant is 1.00 x 102. Suppose 5.0 x 10-1 atm of HI, 1.0 x 10-2 atm of H2 , and 5.0 x 10-3 atm of I2 are mixed inside a 5.0-L flask. Calculate the equilibrium pressure of all species. H2 (g) ...
Chemical Equilibrium
... concentrations of all species in the equilibrium constant expression For the species where both initial and equilibrium concentrations are known, calculate the change in concentration that ...
... concentrations of all species in the equilibrium constant expression For the species where both initial and equilibrium concentrations are known, calculate the change in concentration that ...
Equilibrium
... 6. Obtain 2 graduated cylinders (both the same size) and 2 beakers. b. Label one of the beakers and cylinders as A and the other as B. c. Fill cylinder “A” a little over half full with water and no water in cylinder “B”. d. Record the volume of water in each cylinder. This will be trial 1. e. Pour ½ ...
... 6. Obtain 2 graduated cylinders (both the same size) and 2 beakers. b. Label one of the beakers and cylinders as A and the other as B. c. Fill cylinder “A” a little over half full with water and no water in cylinder “B”. d. Record the volume of water in each cylinder. This will be trial 1. e. Pour ½ ...
CH 17 Study Guide with answer Key
... When you decrease the volume of a reaction vessel, you (9) ________________________ the pressure. This causes a reaction at equilibrium to shift to the side with the (10) ________________________ number of moles. If the reaction has an equal number of moles of reactants and products, changing the vo ...
... When you decrease the volume of a reaction vessel, you (9) ________________________ the pressure. This causes a reaction at equilibrium to shift to the side with the (10) ________________________ number of moles. If the reaction has an equal number of moles of reactants and products, changing the vo ...
File
... 6. What is the effect of adding more CO2 to the following equilibrium reaction? CO2 + H2O↔ H2CO3 a. More H2CO3 is produced. b. More H2O is produced. c. The equilibrium d. No Change 7. Two opposing reactions (A + B ↔C + D) occurring simultaneously at the same rate is an example of: a. reversibility. ...
... 6. What is the effect of adding more CO2 to the following equilibrium reaction? CO2 + H2O↔ H2CO3 a. More H2CO3 is produced. b. More H2O is produced. c. The equilibrium d. No Change 7. Two opposing reactions (A + B ↔C + D) occurring simultaneously at the same rate is an example of: a. reversibility. ...
Chapter 9: Chemical Quantities
... -types of orbitals and properties(i.e. energy, types, shapes, and numbers) -electron configurations and orbital diagrams for the elements -electron configurations of ions -categories of electrons (i.e. inner core electrons and valence electrons) ...
... -types of orbitals and properties(i.e. energy, types, shapes, and numbers) -electron configurations and orbital diagrams for the elements -electron configurations of ions -categories of electrons (i.e. inner core electrons and valence electrons) ...
Le Châtelier`s Principle
... Le Châtelier’s Principle Temperature Think of heat as a reactant or product based on if the reaction is exothermic or endothermic Example: exothermic formation of SO3 ...
... Le Châtelier’s Principle Temperature Think of heat as a reactant or product based on if the reaction is exothermic or endothermic Example: exothermic formation of SO3 ...
Equilibrium and Kinetics
... 9. The half-life of a first order reaction is 24 days. (i) Calculate the rate constant for the reaction (ii) The time taken for 75% of the reactant to decay. 10. Derive an expression for the variation of reactant concentration with respect to time for a reaction which exhibits zero order kinetics. H ...
... 9. The half-life of a first order reaction is 24 days. (i) Calculate the rate constant for the reaction (ii) The time taken for 75% of the reactant to decay. 10. Derive an expression for the variation of reactant concentration with respect to time for a reaction which exhibits zero order kinetics. H ...
