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Test your knowledge of acid/base reactions, thermodynamics, and chemical kinetics with this Jeopardy game. Answer questions and earn points!
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Jeopardy Nuclear and Biochem. Acid/Base Thermo. Kinetics Equilibrium Q $100 Q $100 Q $100 Q $100 Q $100 Q $200 Q $200 Q $200 Q $200 Q $200 Q $300 Q $300 Q $300 Q $300 Q $300 Q $400 Q $400 Q $400 Q $400 Q $400 Q $500 Q $500 Q $500 Q $500 Q $500 Final Jeopardy
$100 Question from Acid/Base Which substance acts as the base in the reaction: NH3 (aq) + HNO3 (aq) <==>NH4+ (aq) + NO3- (aq)? A NH3 B HNO3 C NH4 D NO3
$100 Answer from Acid/Base A. NH3
$200 Question from Acid/Base • The label on a bottle indicates that the • substance inside has a pH of 2. • This tells you that the substance is: • neutral. • strongly acidic. • mildly basic. • strongly basic.
$200 Answer from Acid/Base B. strongly acidic.
$300 Question from Acid/Base • The equation below shows how an unknown • compound dissociates when dissolved in water. • CH H+ + C- • If this compound is 99.9% dissociated in • solution, how would it be classified? • As a strong base • As a strong acid • As a weak base • As a weak acid
$300 Answer from Acid/Base B. As a strong acid
$400 Question from Acid/Base • Mr. Lance plans to demonstrate a reaction between • a weak acid and a strong base in his class. Which • acid and base could he use to demonstrate this • reaction? • CH3COOH and NaOH • H2SO4 and NaOH • CH3COOH andNH4OH • H2SO4 and NH4OH
$400 Answer from Acid/Base • CH3COOH and NaOH
$500 Question from Acid/Base • The percentages of dissociation of four acids • are listed below. • Acid P is 0.60% dissociated. • Acid Q is 4.15% dissociated. • Acid R is 12.55% dissociated. • Acid S is 71.55% dissociated. • Which comparison of the strengths of the acids is correct? • Q is a stronger acid than R. • R is a stronger acid than S. • R is a weaker acid than Q. • P is a weaker acid than Q.
$500 Answer from Acid/Base D. P is a weaker acid than Q.
$100 Question from Thermo. Which statement correctly describes the change in molecular motion as water undergoes a change of phase? A. Molecular motion decrease as liquid water becomes ice. B. Molecular motion stays the same as liquid water becomes water vapor. C. Molecular motion decreases as liquid water becomes water vapor. D. Molecular motion decreases as ice becomes liquid water.
$100 Answer from Thermo. A. Molecular motion decrease as liquid water becomes ice.
$200 Question from Thermo. Which graph represents a chemical reaction that releases energy?
$300 Question from Thermo. How is the energy of molecules of ice at 0 oC different from the energy of liquid water molecules at 0 oC? A. Water molecules of ice have less kinetic energy B. Water molecules of ice have more kinetic energy C. Water molecules of ice have less potential energy D. Water molecules of ice have more potential energy
$300 Answer from Thermo. A. Water molecules of ice have less kinetic energy
$400 Question from Thermo. • Which statement is a correct interpretation of the graph? • Solid and liquid are present during interval A. • No heat is absorbed during interval B. • The latent heat of fusion accounts for the energy absorbed • during interval C. • D. Both liquid and gas are present during interval D.
$400 Answer from Thermo. D. Both liquid and gas are present during interval D.
$500 Question from Thermo. • What is the total heat required to raise the temperature of • 500 g of water from 25 oC to 100 oC? • (The specific heat of water is 4.18 J/oC/g.) • 8,360 J • 13,933 J • 156,750 J • 261,250 J
$500 Answer from Thermo. C. 156,750 J
$100 Question from Kinetics Which potential energy diagram BEST shows how a catalyst affects a chemical reaction?
$200 Question from Kinetics • Under normal conditions, hydrogen peroxide decomposes • very slowly to produce oxygen and water. In the presence of • manganese dioxide, the reaction proceeds at a much greater • rate. The manganese dioxide can be recovered and used to • speed the decomposition of still more hydrogen peroxide. • How does manganese dioxide increase the rate of this • reaction? • by increasing the entropy change of the reaction • by making the reaction exothermic instead of endothermic • by providing a different route with a lower activation • energy • D. by increasing the energy difference between products • and reactants
$200 Answer from Kinetics C. by providing a different route with a lower activation energy
$300 Question from Kinetics • The equation below shows the combustion of methane • (CH4) to produce carbon dioxide (CO2) and water (H2O). • How does the rate at which H2O is produced compare with • the rate at which CH4 is consumed? • H2O is produced half as fast as CH4 is consumed. • H2O is produced equally as fast as CH4 is consumed • H2O is produced twice as fast as CH4 is consumed. • H2O is produced four times as fast as CH4 is consumed.
$300 Answer from Kinetics C. H2O is produced twice as fast as CH4 is consumed.
$400 Question from Kinetics • The equation for the production of sulfur trioxide (SO3) from • sulfur dioxide (SO2) and oxygen (O2) is shown below. • Why does decreasing the pressure on the reacting gases • decrease the rate of this reaction? • Molecules collide with less kinetic energy. • The number of collisions between molecules decreases. • Collisions between molecules occur at different angles. • The molecules slow down and have more time to react • when they collide.
$400 Answer from Kinetics B. The number of collisions between molecules decreases.
$500 Question from Kinetics • What are two reasons that an decrease in temperature causes • an decrease in reaction rate? • Activation energy decreases and concentration decreases. • Concentration decreases and the number of collisions • decreases. • C. Kinetic energy of molecules decreases and activation • energy decreases. • D. The number of collisions decreases and kinetic energy of • molecules decreases.
$500 Answer from Kinetics D. The number of collisions decreases and kinetic energy of molecules decreases.
$100 Question from Equilibrium • When a chemical reaction and its reverse are occurring at the • same time and at the same rate, the reaction has achieved • Displacement • Equilibrium • Imbalance • Decomposition.
$100 Answer from Equilibrium B. Equilibrium
$200 Question from Equilibrium • What is the relationship between chemical equilibrium and the • rates of forward and reverse reaction? • In equilibrium, the forward reaction rate must be greater • than the reverse reaction rate. • In equilibrium, the forward reaction rate must be less than • the reverse reaction rate • In equilibrium, the forward and reverse reaction rates must • be equal. • In equilibrium, both forward and reverse reactions must • stop.
$200 Answer from Equilibrium • In equilibrium, the forward and reverse reaction rates must • be equal.
$300 Question from Equilibrium • For the equilibrium: • NH3 (aq) + HNO3 (aq) <==>NH4+ (aq) + NO3- (aq) • What will happen if HNO3 is added? • Shift left • Shift right • Stay the same • None of the above
$300 Answer from Equilibrium B. Shift right
$400 Question from Equilibrium • For the equilibrium: • NH3 (aq) + HNO3 (aq) <==>NH4+ (aq) + NO3- (aq) • What will happen if NH3 is removed? • Shift left • Shift right • Stay the same • None of the above
$400 Answer from Equilibrium • Shift left
$500 Question from Equilibrium • For the equilibrium: • NH3 (aq) + HNO3 (aq) <==>NH4+ (aq) + NO3- (aq) • What will happen if pressure is increased? • Shift left • Shift right • Stay the same • None of the above
$500 Answer from Equilibrium C. Stay the same
$100 Question from Nuclear and Biochem • The process of nuclear change in an atom of radioactive • material is called • Nuclear decay • Isotopes • Nuclear mass • Radon.
$100 Answer from Nuclear and Biochem • Nuclear decay
$200 Question from Nuclear and Biochem • The type of nuclear radiation that can penetrate farthest • through matter is called • Radons • Gamma rays • Neutron emission • X rays
$200 Answer from Nuclear and Biochem B. Gamma rays
$300 Question from Nuclear and Biochem • A sufficiently large nucleus is unstable and has a tendency to show • spontaneous radioactive emissions. What is the reason for these • spontaneous emissions? • The nuclear force between the protons overcomes the • electrostatic force of repulsion. • The electrostatic force of repulsion between the protons • overcomes the nuclear force. • The electrostatic force of repulsion between the protons reduces • and becomes equal to the nuclear force. • The nuclear force between the protons reduces and becomes • equal to the electrostatic force of repulsion.
$300 Answer from Nuclear and Biochem • The electrostatic force of repulsion between the protons • overcomes the nuclear force.
$400 Question from Nuclear and Biochem • Which polymer is made up of glucose subunits? • Crystals • Hydrocarbons • Proteins • Starches
$400 Answer from Nuclear and Biochem D. Starches
$500 Question from Nuclear and Biochem • Proteins can be referred to as polypeptides. How are peptides • related to amino acids? • Peptides are the monomers, amino acids are the linkages • between them. • Amino acids are the monomers, peptides are the linkages • between them. • Amino acids and peptides are different names for the • same structures. • Amino acids are the side groups, peptides the main chain • of a protein.
