unit 4 practice
... A. Solutions of weak acids cannot conduct an electric current but solutions of strong acids can conduct an electric current. B. Strong acids can form concentrated solutions but weak acids cannot form co ...
... A. Solutions of weak acids cannot conduct an electric current but solutions of strong acids can conduct an electric current. B. Strong acids can form concentrated solutions but weak acids cannot form co ...
EXAM REVIEW !!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!! The examination is scheduled
... What is the fundamental equation of chemical thermodynamics? The chemical potential of a pure substance is (G/n)p,T and for a perfect gas = o + RT ln(p/po) how does this change for a real gas. In general = o + RT ln a where a is the activity. For ideal gas a = p/po. For real gas a = f/po. Wh ...
... What is the fundamental equation of chemical thermodynamics? The chemical potential of a pure substance is (G/n)p,T and for a perfect gas = o + RT ln(p/po) how does this change for a real gas. In general = o + RT ln a where a is the activity. For ideal gas a = p/po. For real gas a = f/po. Wh ...
chapter 13 - Humble ISD
... EXAMPLE PROBLEM The following reaction is allowed to go to equilibrium. ...
... EXAMPLE PROBLEM The following reaction is allowed to go to equilibrium. ...
South Pasadena • AP Chemistry
... Something that is added to a reaction to speed up the reaction – it lowers the activation energy (energy necessary for reactants to become products), therefore helping the reaction reach a state of equilibrium sooner – the addition of a catalyst does NOT change the equilibrium constant. 7. What does ...
... Something that is added to a reaction to speed up the reaction – it lowers the activation energy (energy necessary for reactants to become products), therefore helping the reaction reach a state of equilibrium sooner – the addition of a catalyst does NOT change the equilibrium constant. 7. What does ...
Lecture 8
... - The rate of reaction generally depends on the concentration of reactants. Rate =k[A]n[B]m - where k is the rate constant and n and m are the orders of reaction with respect to reactants A and B. - Orders of reaction depend on the mechanism and are not necessarily equal to the stoichiometric coeffi ...
... - The rate of reaction generally depends on the concentration of reactants. Rate =k[A]n[B]m - where k is the rate constant and n and m are the orders of reaction with respect to reactants A and B. - Orders of reaction depend on the mechanism and are not necessarily equal to the stoichiometric coeffi ...
Experiment 16: Spectrophotometric Determination of an Equilibrium Constant
... The flow of liquid is stopped when the desired calibration mark is reached, and the delivered volume is taken as the final reading minus the initial reading. Mix each solution thoroughly with a glass stirring rod. Be sure to dry off the stirring rod after mixing each solution. Immediately proceed wi ...
... The flow of liquid is stopped when the desired calibration mark is reached, and the delivered volume is taken as the final reading minus the initial reading. Mix each solution thoroughly with a glass stirring rod. Be sure to dry off the stirring rod after mixing each solution. Immediately proceed wi ...
Equilibrium - Cobb Learning
... more quickly. • To make a flameless heater, magnesium dust is mixed with salt and a little iron dust in a thin, flexible pad about the size of a playing card. • To activate the heater, a soldier adds a little water. Within seconds the flameless heater reaches the boiling point and is bubbling and st ...
... more quickly. • To make a flameless heater, magnesium dust is mixed with salt and a little iron dust in a thin, flexible pad about the size of a playing card. • To activate the heater, a soldier adds a little water. Within seconds the flameless heater reaches the boiling point and is bubbling and st ...
Topics 7 and 17 Outlines
... • Physical and chemical systems should be covered. • Relationship between Kc values for reactions that are multiples or inverses of one another should be covered. • Specific details of any industrial process are not required. 17.1 The equilibrium law Essential idea: The position of equilibrium can b ...
... • Physical and chemical systems should be covered. • Relationship between Kc values for reactions that are multiples or inverses of one another should be covered. • Specific details of any industrial process are not required. 17.1 The equilibrium law Essential idea: The position of equilibrium can b ...
Miami-Dade College
... k. Describing the effect of adding a “common ion” on the equilibrium. l. Recognizing a buffer solution and giving illustrations of its operation. m. Predicting the effect upon the pH when adding a strong acid or a strong base to 1) distilled water, 2) a strong acid, 3) a strong base, and 4) a buffer ...
... k. Describing the effect of adding a “common ion” on the equilibrium. l. Recognizing a buffer solution and giving illustrations of its operation. m. Predicting the effect upon the pH when adding a strong acid or a strong base to 1) distilled water, 2) a strong acid, 3) a strong base, and 4) a buffer ...
Chapter 6: Chemical Equilibrium
... * d. 3 < 4 < 1 < 2 from smaller no to a larger one of Kp e. 4 < 3 < 2 < 1 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 incre ...
... * d. 3 < 4 < 1 < 2 from smaller no to a larger one of Kp e. 4 < 3 < 2 < 1 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 incre ...
Study Questions
... concentration of AgNO3 does a precipitate start to form? 9. A solution is prepared by mixing 50.0 ml of 0.0100 M lead(II) nitrate with 50.0 ml of 0.0200 M sodium bromide. Will a precipitate form? 10. Write balanced chemical equations for a) the reaction when strong acid is added to H2CO3/NaHCO3 buff ...
... concentration of AgNO3 does a precipitate start to form? 9. A solution is prepared by mixing 50.0 ml of 0.0100 M lead(II) nitrate with 50.0 ml of 0.0200 M sodium bromide. Will a precipitate form? 10. Write balanced chemical equations for a) the reaction when strong acid is added to H2CO3/NaHCO3 buff ...
Ch. 16 Study Guide
... 13. Pure solids and pure liquids are not included in the equilibrium constant expression. 14. Equilibrium constants are unitless even though molarity concentrations or partial pressures are used to calculate them. ...
... 13. Pure solids and pure liquids are not included in the equilibrium constant expression. 14. Equilibrium constants are unitless even though molarity concentrations or partial pressures are used to calculate them. ...
Chemistry 432: Final Exam Review Sheet
... 1. Calculating concentration given H+ or OH- Hydrogen ion H+ is the same as the hydronium ion H3O+. 2. Calculation pH, pOH, H+, or OH- given pH, pOH, H+, or OH-. 3. Calculation molarity (M), molality (m), freezing point depression (Tf), and boiling point elevation (Tb). 4. Gas law calc ...
... 1. Calculating concentration given H+ or OH- Hydrogen ion H+ is the same as the hydronium ion H3O+. 2. Calculation pH, pOH, H+, or OH- given pH, pOH, H+, or OH-. 3. Calculation molarity (M), molality (m), freezing point depression (Tf), and boiling point elevation (Tb). 4. Gas law calc ...
Chapter 4
... Predict the combustion products—particularly of carbon-hydrogen and carbon-hydrogen-oxygen compounds—and write a balanced equation. ...
... Predict the combustion products—particularly of carbon-hydrogen and carbon-hydrogen-oxygen compounds—and write a balanced equation. ...
1 ChE 505 WORKSHOP 1 1. Why are chemical reactions important
... Calculate the equilibrium conversion of SO2 reacting with air at 25˚C and at 600˚Cfor a feed that contains 1) stoichiometric ratio of reactants 2) large excess of air. Assume constant heat or reaction. ...
... Calculate the equilibrium conversion of SO2 reacting with air at 25˚C and at 600˚Cfor a feed that contains 1) stoichiometric ratio of reactants 2) large excess of air. Assume constant heat or reaction. ...
