ppt - UCLA Chemistry and Biochemistry
... Gas Phase Equilibrium Solution Phase Equilibrium Extent of Reaction Direction of Reaction ...
... Gas Phase Equilibrium Solution Phase Equilibrium Extent of Reaction Direction of Reaction ...
GCE Chemistry Teachers` Guide (A2) Word Document
... choice of four. Additionally there is a need to balance the type of experiment chosen: some involve a substantial planning element while others involve the preparation and quantitative analysis of a compound and there should therefore be no more than one experiment of the planning type. To be specif ...
... choice of four. Additionally there is a need to balance the type of experiment chosen: some involve a substantial planning element while others involve the preparation and quantitative analysis of a compound and there should therefore be no more than one experiment of the planning type. To be specif ...
Possibilities of using thermal mass in buildings to save energy, cut
... The building sector needs to become more energy efficient. Traditional ways to reduce energy consumption in buildings are to increase the insulation (reducing conductive heat losses), make buildings more air-tight and reduce ventilation losses by heat recovery. Another aspect to consider is the user ...
... The building sector needs to become more energy efficient. Traditional ways to reduce energy consumption in buildings are to increase the insulation (reducing conductive heat losses), make buildings more air-tight and reduce ventilation losses by heat recovery. Another aspect to consider is the user ...
EXPERIMENT 3 – Keto-Enol Equilibrium Using NMR
... in at least four different solvents (C6D6, C6D12, CD3CN, H2O/D2O, CDCl3, acetone-d6 and/or dimethyl sulfoxide-d6) at a concentration of ~1 mM. Prepare them at least 60 minutes in advance of running the proton NMR spectrum (to let the enol-keto ratio equilibrate). The solutions should be prepared dir ...
... in at least four different solvents (C6D6, C6D12, CD3CN, H2O/D2O, CDCl3, acetone-d6 and/or dimethyl sulfoxide-d6) at a concentration of ~1 mM. Prepare them at least 60 minutes in advance of running the proton NMR spectrum (to let the enol-keto ratio equilibrate). The solutions should be prepared dir ...
Power Point for Equilibrium
... • Therefore, the larger K the more products are present at equilibrium. • Conversely, the smaller K the more reactants are present at equilibrium. • If K >> 1, then products dominate at equilibrium and equilibrium lies to the right. • If K << 1, then reactants dominate at equilibrium and the equilib ...
... • Therefore, the larger K the more products are present at equilibrium. • Conversely, the smaller K the more reactants are present at equilibrium. • If K >> 1, then products dominate at equilibrium and equilibrium lies to the right. • If K << 1, then reactants dominate at equilibrium and the equilib ...
In_Class_Practice Chapter 17 PreAP
... Calculate Keq for this equilibrium using the data [NOBr] = 0.0474 mol/L, [NO] = 0.312 mol/L, and [Br2] = 0.259 mol/L. Practice Problems 3. The following is the chemical equation for the decomposition of formamide. HCONH2(g) NH3(g) + CO(g) Calculate Keq using the equilibrium data [HCONH2] = 0.0637 ...
... Calculate Keq for this equilibrium using the data [NOBr] = 0.0474 mol/L, [NO] = 0.312 mol/L, and [Br2] = 0.259 mol/L. Practice Problems 3. The following is the chemical equation for the decomposition of formamide. HCONH2(g) NH3(g) + CO(g) Calculate Keq using the equilibrium data [HCONH2] = 0.0637 ...
19_Worked_Examples
... metal to the cooler water. The final temperature, after the metal and water achieve the same temperature (thermal equilibrium), will be somewhere between the initial temperatures of the metal and the water. (b) Experience tells us that this process is not spontaneous— we certainly have never seen hy ...
... metal to the cooler water. The final temperature, after the metal and water achieve the same temperature (thermal equilibrium), will be somewhere between the initial temperatures of the metal and the water. (b) Experience tells us that this process is not spontaneous— we certainly have never seen hy ...
CHEMICAL EQUILIBRIUM
... 8. Even though the individual sets of equilibrium concentrations are quite different for the different situations, the equilibrium constant which depends on the ratio of the concentrations, remains the same. 9. Each set of equilibrium concentrations is called an ______________________________. 10. ...
... 8. Even though the individual sets of equilibrium concentrations are quite different for the different situations, the equilibrium constant which depends on the ratio of the concentrations, remains the same. 9. Each set of equilibrium concentrations is called an ______________________________. 10. ...
The Effect of Temperature on Spontaneity
... The sign of ΔSsurr depends on the direction of the heat flow. At constant temperature , an exothermic process in the system causes the heat flow into the surrounding. It increases the random motions and the entropy of the surroundings. ΔSsurr is positive The magnitude of ΔSsurr depends on the temper ...
... The sign of ΔSsurr depends on the direction of the heat flow. At constant temperature , an exothermic process in the system causes the heat flow into the surrounding. It increases the random motions and the entropy of the surroundings. ΔSsurr is positive The magnitude of ΔSsurr depends on the temper ...
Equilibrium
... equilibrium concentration of H2O(g) is 0.1990 M, what concentrations of CO and H2 would you expect to find? 13. When nitrogen monoxide gas comes in contact with air, it oxidizes to the brown gas nitrogen dioxide according to the following equation: 2NO(g) + O2(g) ↔ 2NO2(g) a. The equilibrium constan ...
... equilibrium concentration of H2O(g) is 0.1990 M, what concentrations of CO and H2 would you expect to find? 13. When nitrogen monoxide gas comes in contact with air, it oxidizes to the brown gas nitrogen dioxide according to the following equation: 2NO(g) + O2(g) ↔ 2NO2(g) a. The equilibrium constan ...
AP Chemistry: Bonding Multiple Choice
... (A) are made up of atoms that are intrinsically hard because of their electronic structures (B) consist of positive and negative ions that are strongly attracted to each other (C) are giant molecules in which each atom forms strong covalent bonds with all of its neighboring atoms (D) are formed unde ...
... (A) are made up of atoms that are intrinsically hard because of their electronic structures (B) consist of positive and negative ions that are strongly attracted to each other (C) are giant molecules in which each atom forms strong covalent bonds with all of its neighboring atoms (D) are formed unde ...
CHEMISTRY 102 Spring 2012 Hour Exam III Page 20 1. For the
... After equilibrium is reached, which of the following statements (a-d) regarding these experiments is true? a) In experiment 1, the rate of the forward reaction at equilibrium will be greater than the rate of the reverse reaction at equilibrium. b) Equilibrium cannot be reached in experiment 2 becaus ...
... After equilibrium is reached, which of the following statements (a-d) regarding these experiments is true? a) In experiment 1, the rate of the forward reaction at equilibrium will be greater than the rate of the reverse reaction at equilibrium. b) Equilibrium cannot be reached in experiment 2 becaus ...
Physical Chemistry Lab Report Rubric –Veldman Fall 2012
... raise the temperature of the water quickly and significantly due to the heat evolved during the course of the reaction. This process will give initial temperature (Tinitial ) and final temperature (T f inal ), which will be used to determine the heat capacity (Cvcal ) of the calorimeter via the foll ...
... raise the temperature of the water quickly and significantly due to the heat evolved during the course of the reaction. This process will give initial temperature (Tinitial ) and final temperature (T f inal ), which will be used to determine the heat capacity (Cvcal ) of the calorimeter via the foll ...
L-12 Spontaneity of chemical reactions
... (ii) the gaseous state is the most disordered state, hence its entropy is the maximum, and (iii) the disorder in the liquid state is intermediate between the solid and the gaseous state. When a system changes from one state to another, the change of entropy S is given by S = ...
... (ii) the gaseous state is the most disordered state, hence its entropy is the maximum, and (iii) the disorder in the liquid state is intermediate between the solid and the gaseous state. When a system changes from one state to another, the change of entropy S is given by S = ...
Chemical Equilibrium - The Gurukul Institute
... 2. One mole of H2, 2 mol of l2 and 3 mol of Hl are injected in a 1 litre flask. What will be the concentration of H2, l2 and Hl at equilibrium? Kc for the equilibrium, H2(g) + l2(g) ⇌ 2Hl is 45.9. 3. 15 g sample of BaO2 is heated to 794o C in a closed evacuated vessel of 5 litres capacity. How many ...
... 2. One mole of H2, 2 mol of l2 and 3 mol of Hl are injected in a 1 litre flask. What will be the concentration of H2, l2 and Hl at equilibrium? Kc for the equilibrium, H2(g) + l2(g) ⇌ 2Hl is 45.9. 3. 15 g sample of BaO2 is heated to 794o C in a closed evacuated vessel of 5 litres capacity. How many ...
ppt
... not affect the final position of equilibrium • Inert Gases • Increases the pressure, which will increase reaction rate • Increases the probability of successful collisions for BOTH products and reactants equally • Decreases the time required to reach equilibrium but does not affect the final positio ...
... not affect the final position of equilibrium • Inert Gases • Increases the pressure, which will increase reaction rate • Increases the probability of successful collisions for BOTH products and reactants equally • Decreases the time required to reach equilibrium but does not affect the final positio ...
Collected Essays chapter 13 answers
... (b) Some extra NH3 gas is injected into the vessel containing the sample described in part (a). When equilibrium is reestablished at 25°C, the partial pressure of NH3 is twice the partial pressure of H2S. Calculate the numerical value of the partial pressure of NH3 and the partial pressure of H2S in ...
... (b) Some extra NH3 gas is injected into the vessel containing the sample described in part (a). When equilibrium is reestablished at 25°C, the partial pressure of NH3 is twice the partial pressure of H2S. Calculate the numerical value of the partial pressure of NH3 and the partial pressure of H2S in ...
Ch. 16 Study Guide
... 15. No matter how a reaction is set up, the value of the equilibrium will be the same if the temperature is kept constant. 16. The reaction quotient, Qc , is expressed as concentration of products over concentration of reactants, with each substance raised to its stoichiometric power. There is also ...
... 15. No matter how a reaction is set up, the value of the equilibrium will be the same if the temperature is kept constant. 16. The reaction quotient, Qc , is expressed as concentration of products over concentration of reactants, with each substance raised to its stoichiometric power. There is also ...
GCE Chemistry Question Paper Unit 04 - Kinetics, Equilibria
... Calculate the amounts, in moles, of hydrogen and of iodine in the equilibrium mixture. Moles of hydrogen ............................................................................................................. Moles of iodine ..................................................................... ...
... Calculate the amounts, in moles, of hydrogen and of iodine in the equilibrium mixture. Moles of hydrogen ............................................................................................................. Moles of iodine ..................................................................... ...
Thermal performance improvements in low
... fuel switches or improvements in heating appliances. However, if these changes in space heating fuels/appliances/behaviour happen during the project cycle, they will be included in emissions calcul ...
... fuel switches or improvements in heating appliances. However, if these changes in space heating fuels/appliances/behaviour happen during the project cycle, they will be included in emissions calcul ...
Hein and Arena - faculty at Chemeketa
... In 1888, the French chemist Henri LeChatelier This generalization, known as set forth a far-reaching generalization on the LeChatelier’s Principle, states behavior of equilibrium systems. If a stress or strain is applied to a system in equilibrium, the system will respond in such a way as to reliev ...
... In 1888, the French chemist Henri LeChatelier This generalization, known as set forth a far-reaching generalization on the LeChatelier’s Principle, states behavior of equilibrium systems. If a stress or strain is applied to a system in equilibrium, the system will respond in such a way as to reliev ...
BONUS: Which line in the above graph represents G for the reaction
... which change will cause an increase in the pressure of CO2(g) when equilibrium is re-established? (A) ...
... which change will cause an increase in the pressure of CO2(g) when equilibrium is re-established? (A) ...