LOYOLA COLLEGE (AUTONOMOUS), CHENNAI –600 034 B.Sc., DEGREE EXAMINATION - CHEMISTRY
... 11. Show that for an ideal gas u H ) T = 0. a) ( ) T = 0. b) ( v P 12. Internal energy and enthalpy remain constant in the isothermal expansion of an ideal gas Explain. 13. For the reaction N2 (g) + 3H2 (g) 2 NH3(g). Kp is 1.64 x 10-4 at 673 k. Calculate G when the partial pressure of N2, H2 ...
... 11. Show that for an ideal gas u H ) T = 0. a) ( ) T = 0. b) ( v P 12. Internal energy and enthalpy remain constant in the isothermal expansion of an ideal gas Explain. 13. For the reaction N2 (g) + 3H2 (g) 2 NH3(g). Kp is 1.64 x 10-4 at 673 k. Calculate G when the partial pressure of N2, H2 ...
Chapter 6: Chemical Equilibrium
... 9. The reaction, Q + 2 SO3(g) 2 SO2(g) + O2(g) is endothermic. Predict what will happen if the temperature is increased. a. Kc remains the same b. Kc decreases c. the pressure decreases d. more SO3(g) is produced * e. Kc increases T increase, reaction will shift to right side and Kc increase 10. Con ...
... 9. The reaction, Q + 2 SO3(g) 2 SO2(g) + O2(g) is endothermic. Predict what will happen if the temperature is increased. a. Kc remains the same b. Kc decreases c. the pressure decreases d. more SO3(g) is produced * e. Kc increases T increase, reaction will shift to right side and Kc increase 10. Con ...
2012 Coaches Institute Presentation
... Dynamic equilibrium - forward and reverse processes occur at same rate } Results in the formation of a mixture of reactants and products whose concentrations are in dynamic equilibrium ...
... Dynamic equilibrium - forward and reverse processes occur at same rate } Results in the formation of a mixture of reactants and products whose concentrations are in dynamic equilibrium ...
Chapter 19, part II Notes
... Equilibrium Reactions LeChatelier’s Principle Equilibrium Constants ...
... Equilibrium Reactions LeChatelier’s Principle Equilibrium Constants ...
Equilibrium Constant - Faculty Server Contact
... dilution is used as the standard state; -- the activity of H2O = 1 at infinite dilution. The activity of water is related to the mole fraction of pure water, XH2O as follows: mH2O = moH2O + RTlnXH2O In most cases, we are dealing with dilute solutions and we can set the activity of H2O = 1. In more c ...
... dilution is used as the standard state; -- the activity of H2O = 1 at infinite dilution. The activity of water is related to the mole fraction of pure water, XH2O as follows: mH2O = moH2O + RTlnXH2O In most cases, we are dealing with dilute solutions and we can set the activity of H2O = 1. In more c ...
Unit 13 Worksheet Answers
... 2) It is found that a 10oC increase in temperature roughly doubles the rate of many chemical reactions. If a reaction takes 20 seconds at 40oC, how long would it take at 60oC? 5 seconds 3) Use the collision theory to explain why each factor (concentration, temperature, surface area) alters the rate ...
... 2) It is found that a 10oC increase in temperature roughly doubles the rate of many chemical reactions. If a reaction takes 20 seconds at 40oC, how long would it take at 60oC? 5 seconds 3) Use the collision theory to explain why each factor (concentration, temperature, surface area) alters the rate ...
13AP General Equilibrium FR worksheet (missing 1988)
... (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375 K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375 ...
... (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375 K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375 ...
Chemical Equilibrium Stress? What stress? 1
... Manipulating the Equilibrium… There is a principle that can be studied to govern changes in equilibrium (Le Chatelier’s Principle). Le Chatelier’s Principle states: “If a stress is applied to a system in dynamic equilibrium, the system changes to relieve the stress.” Stresses are changes in ...
... Manipulating the Equilibrium… There is a principle that can be studied to govern changes in equilibrium (Le Chatelier’s Principle). Le Chatelier’s Principle states: “If a stress is applied to a system in dynamic equilibrium, the system changes to relieve the stress.” Stresses are changes in ...
Lecture 10 Activity of chemical components
... dilute solution. For example in 0.1 molar solutions it could differ by factor of three. Similarly, if we were to consider the effect of added electrolyte like Na Acetate, we can recalculate the activity coefficient using Debye model. ...
... dilute solution. For example in 0.1 molar solutions it could differ by factor of three. Similarly, if we were to consider the effect of added electrolyte like Na Acetate, we can recalculate the activity coefficient using Debye model. ...
Equilibrium Constant- Keq
... Equilibrium Constant- Keq 1. In an experiment, 0.500 mol/L of hydrogen bromide gas is decomposed into hydrogen and bromine gases. a) Write the equilibrium equation and equilibrium law for this reaction. b) The equilibrium concentrations in this system are [HBr(g)] =0.240 mol/L and [H2(g)]=0.130 mol/ ...
... Equilibrium Constant- Keq 1. In an experiment, 0.500 mol/L of hydrogen bromide gas is decomposed into hydrogen and bromine gases. a) Write the equilibrium equation and equilibrium law for this reaction. b) The equilibrium concentrations in this system are [HBr(g)] =0.240 mol/L and [H2(g)]=0.130 mol/ ...
Chemical equilibrium
In a chemical reaction, chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. Usually, this state results when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and backward reactions are generally not zero, but equal. Thus, there are no net changes in the concentrations of the reactant(s) and product(s). Such a state is known as dynamic equilibrium.