Si #13
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This document contains 7 questions about chemical kinetics and equilibrium concepts. Question 1 involves calculating amounts of N2O5 remaining and half-life during its decomposition reaction. Question 2 concerns rate laws and reaction orders. Question 3 provides rate data and asks about rate laws and rates for the decomposition of N2O5. Question 4 gives a rate law and asks about reaction rates. Question 5 asks about the law of mass action. Question 6 asks to write equilibrium constants for 3 reactions. Question 7 asks which reactions favor products or reactants based on given equilibrium constants.
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![GENERAL CHEMISTRY-II (1412)
S.I. # 13
1. The 1st order rate constant for the decomposition of N2O5(g)
N2O5 (g) 2 NO2 (g) + O2 (g)
at 70°C is 6.82x10-3s-1. Start with 0.0250 mol N2O5 (g) in a volume of 2.0 L.
a. How many mole of N2O5 will remain after 2.5 min.?
b. How many minutes will it take for the quantity of N2O5 to drop to 0.010 mol?
c. What is the half life of N2O5 at 70°C?
2. A reaction A + B C obeys the following rate law: Rate = k[A] 2 [B].
a. if [A] is doubled how will the rate change? Explain
b. what are the reaction orders for A and B and the reaction overall?
c. what are the units of k?](https://image.slidesharecdn.com/chem-ii-si-13-1269456071-phpapp01/85/Si-13-1-320.jpg)
![3. The decomposition of N2O5 in carbon tetrachloride proceeds as follows:
2 N2O5 4 NO2 + O2 . The rate law is 1st order in N2O5. At 64°C the rate
constant is 4.82x10-3 s-1.
a. write the rate law for the reaction
b. what is the rate of the reaction when [N2O5] = 0.0240 M?
c. What happens to the rate when the concentration of N2O5 is doubled to 0.0480M?
4. 2 NO 2H2 (g) + 2H2O (g)
The rate law for this reaction is 1st order in H2 and 2nd order in NO. a. Write the
rate law. b. If the rate constant at 1000K is 6.0x104M-2s-1, what is the reaction rate
when [NO] = 0.025 M and [H2] = 0.015M? c. What is the reaction rate when the
concentrations are both 0.010M?
5. What is the law of mass action? Give the formula and explain.
6. Write the equilibrium constant (Kc) for the following reactions:
a. 2 O3 (g) 3 O2 (g)
b. 2 NO (g) + Cl2 (g) 2 NOCl(g)
c. Ag+ (aq) + 2 NH3 (aq) Ag (NH3)2+ (aq)](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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The document is a practice exam for general chemistry II that contains 10 multiple choice questions testing knowledge of intermolecular forces, phase changes, concentrations, vapor pressure, and nomenclature. It asks about the forces between molecules, which substance experiences only dispersion forces, the process of molecules sticking to a surface, the energy required to expand a liquid's surface area, the vapor pressure at the normal boiling point, the concentration of nitrate ions in a solution, the direct change of a solid to a gas, and the phase changes of water freezing and drying and frost forming. It concludes by listing the names and symbols of 10 chemical substances and compounds.
SI #10
This document contains 11 multiple choice and short answer questions about concepts in general chemistry including: solvent-solute interactions, hydration, enthalpy of solution, colligative properties, molality calculations, definitions of colloid and miscibility, concentration calculations involving mass percent and ppm, and molality calculations for solutions.
#23
The document contains a chemistry practice exam with 10 multiple-choice and short-answer questions testing concepts such as how the percent dissociation of a weak acid changes with concentration, calculating percent dissociation and acid dissociation constants given various parameters, determining pH and pOH values of solutions, and identifying chemical reactions between acids and bases in aqueous solutions.
SI #12
Chemical kinetics describes the rates of chemical reactions. The three factors that affect reaction rates are concentration of reactants, temperature, and presence of a catalyst. An instantaneous rate is the rate of reaction at a specific moment in time. Beer's law relates the absorption of light to the concentration of an absorbing substance in a solution. First and second order reactions have rates dependent on the first or second power of the concentration of a reactant. Half-life is the time required for half of the reactants to be converted to products at a given reaction rate. Activation energy is the minimum energy that reactant molecules must possess for a reaction to occur.
#19
This document covers Bronsted-Lowry acids and bases, conjugate acids and bases, and acid-base equilibrium. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. Conjugate acids are formed when a base gains a proton, and conjugate bases are formed when an acid loses a proton. Several examples of conjugate acid-base pairs are given. The document also discusses how the strength of an acid or base determines the position of acid-base equilibrium and the autoionization process and ion product constant for water.
SI #3 Key
1. The document discusses key concepts from general chemistry including:
- The van der Waals equation accounting for non-zero particle volumes and interparticle interactions.
- Using the ideal gas law to calculate changes in volume with temperature changes.
- The value of the gas constant R at standard temperature and pressure.
- Conversions between various pressure and volume units.
- Calculating moles, pressure, volume, and number of molecules using the ideal gas law.
Key SI #7
The critical temperature is the highest temperature at which a distinct liquid phase can form. It is the highest temperature at which a liquid can exist. Non-polar substances with weak intermolecular forces have lower critical temperatures.
The vapor pressure of a liquid increases nonlinearly with increasing temperature.
Viscosity increases as temperature decreases, molecular weight increases, and intermolecular forces increase.
#18
This document contains 6 chemistry problems involving gas phase chemical equilibria. Problem 1 involves calculating the equilibrium partial pressure and equilibrium constant for the reaction N2O4(g) ⇌ 2NO2(g). Problem 2 involves calculating equilibrium concentrations and the equilibrium constant for the reaction H2(g) + Br2(g) ⇌ 2HBr(g). Problem 3 asks to calculate the equilibrium constant for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g) given the value of Kp at a specific temperature.
#20
The document provides a chemistry problem set involving calculations of hydrogen ion (H+) and hydroxide ion (OH-) concentrations in solution, definitions and calculations of pH and pOH, and properties of strong acids, weak acids, and weak bases. It asks students to calculate pH and concentrations of H+ given OH- concentrations and vice versa. It also asks students to list strong acids and bases, properties of strong and weak acids, what weak acids and bases have in common, and why HCl is a strong acid but weak base.
SI #7
This document contains questions about chemistry concepts and definitions. It asks to define critical temperature and strong electrolyte, and explains that hydration refers to water molecules surrounding ions when strong electrolytes dissolve in water. It also asks how temperature, molecular weight, and intermolecular forces affect a molecule's viscosity. Finally, it lists the names or formulas of 20 chemical substances.
Si #15 Key
The document defines key concepts related to reaction rates in chemistry:
1) Reaction rate is defined as the change in concentration of a reactant or product with time.
2) The rate formula relates the rate of a reaction to the change in concentration of a reactant or product over time.
3) The concentration of reactants is directly proportional to the rate of reaction according to the rate formula.
4) A catalyst increases the reaction rate by participating in the reaction without being consumed and allowing collisions between molecules to result in reaction at lower energies.
Key SI #6
Intermolecular forces exist between molecules, while intramolecular forces exist within molecules. Melting points increase as intermolecular forces strengthen. Polar molecules have partial charges and can form ion-dipole attractions. The main intermolecular forces are London dispersion, dipole-dipole, and hydrogen bonding. Ionic and covalent bonds are stronger than any intermolecular force within a molecule. A flow chart determines the dominant intermolecular force based on whether ions or polar molecules are present.
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SI #2 Key
This document provides 13 multiple choice and calculation questions about key concepts in general chemistry including the ideal gas law, density, molar mass, reaction stoichiometry involving gases, and gas behavior. It tests understanding of gas laws, calculations using the ideal gas equation, and properties that affect how real gases deviate from ideal behavior. The final question indicates that an ideal gas is distinguished from real gases by the fact that ideal gas molecules have no attraction for one another.
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The half-life of N2O5 for a first order reaction is:
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(1) The decomposition of N2O5 at 45°C is a first-order reaction, with a rate equation of Rate = k[N2O5]1. (2) Using the initial concentration and rate of decline provided, the rate constant k is calculated to be 5.733 x 10-4 s-1. (3) For the first-order reaction converting cyclobutane to 1-butene at 42°C, with a given rate constant and initial concentration, the concentration after 24 hours is calculated to be 3.9 x 10-3 M.
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#27
This document contains questions about oxidation-reduction reactions and voltaic cells. It asks the student to identify oxidizing and reducing agents, write half reactions, identify anodes and cathodes, and determine the direction of electron and ion flow. It also contains questions about standard cell potentials, units of electrical potential, and a half reaction for a hydrogen electrode.
#26 Key
1. The document provides steps to convert between solubility in grams per liter, molar solubility in mol/L, molar concentrations of ions, and Ksp.
2. It gives the definitions of a reducing agent, oxidizing agent, and half-reaction. A reducing agent causes reduction, an oxidizing agent causes oxidation. Half-reactions involve electrons.
3. An anode is where oxidation occurs and a cathode is where reduction occurs in a voltaic cell. Electrons flow from the anode through the external circuit to the cathode.
#26
The document discusses solubility and solubility products, oxidation-reduction reactions, and voltaic cells. It defines key concepts like reducing agents, oxidizing agents, and half-reactions. It also discusses standard reduction potentials, how to determine if a reaction involves oxidation-reduction, and how to balance half-reactions to indicate oxidation or reduction. Sample problems are provided to calculate equilibrium constants from solubility products and oxidation states in reactions.
#25 Key
1. The common ion effect decreases the ionization of a weak electrolyte when a strong electrolyte with a common ion is added to the solution.
2. Buffer capacity refers to how much acid or base can be neutralized before the pH begins to change significantly.
3. A buffer solution contains a weak acid or base and its salt. It has the ability to resist changes in pH.
4. The pH range of a buffer depends on the acid's Ka value and the relative concentrations of the acid and base in the buffer solution. It is the range over which the buffer acts effectively.
#25
The document provides 10 questions related to general chemistry concepts including:
1) Defining the common ion effect and buffer capacity
2) Providing the Henderson-Hasselbalch equation
3) Calculating the pH of different buffer solutions
#24 Key
This document provides examples of calculating the pH of various strong acid solutions, including nitric acid, perchloric acid, hydrochloric acid, a mixture of hydrochloric acid and hydroiodic acid, and a solution of bromoacetic acid that is partially ionized. It also asks questions about weak acids, Lewis acids, and which compounds form more acidic solutions based on cation properties.
#20 Key
The document provides information about acid-base chemistry including:
1) Calculating the concentration of H+ ions and determining if solutions are acidic or basic based on the relative concentrations of H+ and OH- ions.
2) Defining pH as the negative logarithm of the H+ ion concentration and calculating pH values from given [H+] values.
3) Relating pH and pOH through the equation pH + pOH = 14.
4) Listing the 7 strong acids and their formulas as well as the 7 strong bases and their formulas.
#19 Key
This document discusses Bronsted-Lowry acid-base chemistry. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. It explains that conjugate acids are formed by adding a proton to a base and conjugate bases are formed by removing a proton from an acid. Several examples of conjugate acid-base pairs are given. The document also states that the stronger the acid, the weaker its conjugate base, and the stronger the base, the weaker its conjugate acid. It describes how the position of equilibrium favors transfer of a proton to the stronger base. Finally, it provides the autoionization reaction of water and defines the ion product constant, Kw, for water.
#17 Key
1. The document contains 7 chemistry problems involving calculation of equilibrium constants (Keq and Kc) for various chemical reactions.
2. Problem 3 calculates Keq as 1.84x10-2 for the decomposition of HI gas into H2 and I2 gases at 425C, given the partial pressures of reactants and products at equilibrium.
3. Problem 7 involves a multiple step chemical equilibrium problem, calculating the initial and equilibrium partial pressures and concentrations of gases in a reaction between CO2, H2 and H2O, and determining the equilibrium constant Kp.
SI #16
The document contains a chemistry practice problem set with 10 multiple choice questions about reaction rates and rate laws. The questions cover topics such as how the rates of reactants and products are related in a chemical reaction, how to write rate laws from reaction equations, determining reaction orders from rate equations, and calculating rate constants. It also includes a nomenclature list of 38 chemical species.
#11 Key
The document contains a chemistry problem set with 10 questions:
1) It asks to calculate the molarity of three aqueous solutions.
2) It asks to calculate the percentage by mass of nitric acid in a 16 M commercial solution.
3) It asks to calculate the osmotic pressure of a solution formed by dissolving aspirin in water.
4) It asks to order solutions by increasing boiling point.
5) It defines hydrophobic and hydrophilic colloids and provides examples.
6) It asks to identify colloids as hydrophobic or hydrophilic.
#10 Key
This document provides definitions and examples of key concepts in general chemistry including:
1. Solvation refers to the attractive interaction between solvent molecules and a solute. Hydration describes the interaction when water is the solvent.
2. The overall enthalpy change of a solution can be either positive (endothermic) or negative (exothermic).
3. A saturated solution is one in equilibrium with undissolved solute where dissolution and crystallization occur at equal rates. Unsaturated and supersaturated solutions contain less or more solute respectively.
4. Colligative properties include vapor pressure depression, freezing point depression, boiling point elevation, and osmotic pressure.
#9 Key
London dispersion forces are the attractive force between two molecules with hydrogen bonded to the oxygen atom. CH4 has dispersion forces as its only intermolecular force. Adsorption is the process of a substance sticking to the surface of another. Surface tension is the energy required to expand the surface area of a liquid by a unit amount of area. The vapor pressure of any substance at its normal boiling point is 1 atm. The concentration of nitrate ion in a solution containing 0.900 M aluminum nitrate is 2.70 M. Sublimination is the direct conversion of a solid to a gas.
#8 Key
1. Ionic bonding involves the complete transfer of an electron from one element to another.
2. Covalent bonds have equally shared pairs of electrons between atoms.
3. Polar covalent bonds are defined as occurring when one atom exerts a greater attraction for the bonding electrons.
SI #11
The document contains 10 chemistry problems related to calculating molarity and percent composition of solutions, osmotic pressure, boiling points of solutions, definitions of hydrophilic and hydrophobic colloids, and identifying examples of each. It also contains 10 chemistry nomenclature problems to identify chemical formulas and names.
Si #13
- 1. GENERAL CHEMISTRY-II (1412) S.I. # 13 1. The 1st order rate constant for the decomposition of N2O5(g) N2O5 (g) 2 NO2 (g) + O2 (g) at 70°C is 6.82x10-3s-1. Start with 0.0250 mol N2O5 (g) in a volume of 2.0 L. a. How many mole of N2O5 will remain after 2.5 min.? b. How many minutes will it take for the quantity of N2O5 to drop to 0.010 mol? c. What is the half life of N2O5 at 70°C? 2. A reaction A + B C obeys the following rate law: Rate = k[A] 2 [B]. a. if [A] is doubled how will the rate change? Explain b. what are the reaction orders for A and B and the reaction overall? c. what are the units of k?
- 2. 3. The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2 N2O5 4 NO2 + O2 . The rate law is 1st order in N2O5. At 64°C the rate constant is 4.82x10-3 s-1. a. write the rate law for the reaction b. what is the rate of the reaction when [N2O5] = 0.0240 M? c. What happens to the rate when the concentration of N2O5 is doubled to 0.0480M? 4. 2 NO 2H2 (g) + 2H2O (g) The rate law for this reaction is 1st order in H2 and 2nd order in NO. a. Write the rate law. b. If the rate constant at 1000K is 6.0x104M-2s-1, what is the reaction rate when [NO] = 0.025 M and [H2] = 0.015M? c. What is the reaction rate when the concentrations are both 0.010M? 5. What is the law of mass action? Give the formula and explain. 6. Write the equilibrium constant (Kc) for the following reactions: a. 2 O3 (g) 3 O2 (g) b. 2 NO (g) + Cl2 (g) 2 NOCl(g) c. Ag+ (aq) + 2 NH3 (aq) Ag (NH3)2+ (aq)
- 3. 7. Which of the following reactions lies to the right, favoring the formation of products, and which lies to the left, favoring the reactants? a. 2NO (g) O2 (g) 2 NO2 (g) ; Kc = 5.0x1012 b. 2 HBr (g) H2 (g) + Br2 (g) ; Kc = 5.8x10-18