True/ False
The rate constant increases when a) the increasing temperature and increasing activation energy b) with increasing temperature and decreasing activation energy c) with decreasing temperature and increasing activation energy d) with decreasing temperature and decreasing activation energy
B)
i. Gibbs free energy is a form of chemical potential energy. ii. Gibbs free energy can be used to determine which compound is more stable.
Both i. and ii.
i. Strong acids tend to be good oxidizing agents. ii. Halogens are typically better oxidizing agents than reducing agents.
Both i. and ii.
i. The larger the concentration of the products relative to the reactants, the larger the reaction quotient. ii. Reaction quotients are defined as concentrations and/or pressures of products over reactants, with coefficients as exponents.
Both i. and ii.
First Law of Thermodynamics
Energy cannot be created or destroyed
i. Entropy is a measure of the number of possible configurations. ii. The gas phase of a compound always has higher entropy than its liquid phase.
both
i. The equilibrium constant for endothermic reactions always increase with increasing temperature. ii. Equilibrium constants increase with decreasing temperature for reactions where heat is a product
both i and ii.
i. If the coefficients of a reaction are multiplied by two, the equilibrium constant of the new reaction is equal to the square of the original reaction. ii. If the products and reactants of a reaction are swapped, the equilibrium constant of the new reaction is equal to the inverse of the equilibrium constant of the original reaction.
both i. and ii.
i. If ∆G◦<0, then K>1. ii. If the reactants of a reaction are much more stable than the products, than the equilibrium constant will be less than one.
both i. and ii.
i. The equilibrium constants for exothermic reactions always decrease with increasing temperature. ii. Equilibrium constants increase with decreasing temperature for reactions where heat is a product
both i. and ii.
i. The pH of pure water at 25◦C is always 7.0. ii. For pure water[H+]= [OH]
both i. and ii.
i. Water boiling is an endothermic process. ii. Ice melting has a positive change in enthalpy
both i. and ii.
Second Law of Thermodynamics
every spontaneous change increases the entropy of the universe
i. Rate of a chemical reaction increases with increasing temperature because at higher temperatures chemical bonds are weaker. ii. The concentrations of the reactants affect the reaction rate but not the rate constant
ii only
A catalyst....
increases the reaction rate by providing an alternative pathway with a lower activation energy
i. Catalysts change the reaction pathway of reactions in such a way that the reactions become more exothermic. ii. Catalysts are reaction intermediates
neither
i. Catalysts increase the size of the equilibrium constant so that there are more products at equilibrium. ii. Catalysts increase the rate of the forward reaction and reduce the rate of the reverse reaction
neither
i. If a catalyst is used to speed up a reaction, it will also increase the value of the equilibrium constant. ii. If the initial concentration of the reactants is larger, the equilibrium constant will be larger.
neither
i. Oxidation state is the charge an atom would have, if all of the bonds in the molecule were purely covalent. ii. The oxidation state of each fluorine atom in fluorine gas is −1.
neither
i. The larger the activation energy, the larger the rate constant. ii. If a plot of the concentration of a reactant as a function of time is linear, it means that the reaction is first-order relative to that reactant.
neither
i. The more positive the potential of a reaction, the more positive the∆G◦ of the reaction. ii. The reactions used in electrolytic cells have positive potentials.
neither
i. When two reactions are added together, the equilibrium constant of the resulting reaction is equal to the equilibrium constants of the two original reactions added together. ii. If the products and reactants of a reaction are swapped, the equilibrium constant of the new reaction is equal to the negative of the equilibrium constant of the original reaction.
neither
Which of the following is true? i. The more positive the potential of a reaction, the more positive the G of the reaction ii. The reactions used in electrolytic cells have positive potentials.
neither i or ii
i. If a reaction goes faster, the amount of products at equilibrium will increase. ii. If the initial concentration of the reactants is larger, the equilibrium constant will be larger
neither i. and ii.
i. The larger∆G ̊, the larger K ii. If the products of a reaction are much more stable than the reactants, than the equilibrium constant will be less than one
neither i. and ii.
i. Strong oxidizing agents have large positive oxidation potentials. ii. Strong oxidizing agents tend to lose electrons to other compounds.
neither i. nor ii.
i. All reactions stop once equilibrium is reached. ii. If Q<K, the reverse reaction will be faster than the forward reaction.
neither i. or ii.
i. Strong reducinging agents have large positive reduction potentials. ii. Strong oxidizing agents tend to lose electrons to other compounds
neither i. or ii.
ΔS(universe) < 0
non-spontaneous (will not occur without any outside intervention)
2H+(aq) + Pb(s)⇄H2(g) + Pb2+(aq) K=2×104 which of the following is true? i. at equilibrium there will be more of the products than reactants ii. the potential energy of the products is greater than that of the reactants
only i.
i. A metal rusting is a redox reaction. ii. Halogens typically react by losing electrons
only i.
i. A metal rusting is a redox reaction. ii. Nonmetals typically react by losing electrons.
only i.
i. Gibbs free energy is a form of chemical potential energy ii. The change in Gibbs free energy for a reaction gets bigger the higher the temperature.
only i.
i. If ∆G = 0, the system is necessarily at equilibrium. ii. If the concentrations of the products is equal to the concentrations of the reactants, the system is necessarily at equilibrium
only i.
i. The more negative ∆G ̊, the larger K. ii. If the products of a reaction are much more stable than the reactants, than the equilibrium constant will be less than one.
only i.
i. The more positive the potential of a reaction, the more products and fewer reactants there will be once the system reaches equilibrium. ii. The reactions used in electrolytic cells have positive potentials
only i.
Which of the following is true about the reaction below at 25◦C? I2(s) + Ni(s)⇄2I-(aq) + Ni2+(aq) i. Its equilibrium constant is less than one. ii. The products are more stable than the reactant
only ii.
i The larger the concentration of the reactants relative to the products, the larger the reaction quotient. ii. Reaction quotients are defined as concentrations and/or pressures of products over reactants, with coefficients as exponents.
only ii.
i. All reactions stop once equilibrium is reached. ii. If Q>K, the reverse reaction will be faster than the forward reaction.
only ii.
i. Entropy is a measure of disorder. ii. Heating a compound always increases its entropy.
only ii.
i. If ∆G◦= 0, the system is necessarily at equilibrium. ii. If Q = K, the system is necessarily at equilibrium.
only ii.
i. If∆G = K, the system is necessarily at equilibrium ii. If Q = K, the system is necessarily at equilibrium
only ii.
i. Its equilibrium constant is less than one. ii. The products are more stable than the reactants
only ii.
i. Strong acids tend to be good reducing agents. ii. Metal elements are typically better reducing agents than oxidizing agents.
only ii.
i. The larger the activation energy, the larger the rate constant. ii. If a plot of the natural log of the concentration of a reactant as a function of time is linear it means that the reaction is first-order relative to that reactant
only ii.
i. The pH of pure water is always 7.0 ii. For a neutral solution[H+]= [OH].
only ii.
i. The rate of a chemical reaction increases with increasing temperature because of a decrease in the activation energy at higher temperatures. ii. The concentrations of the reactants affect the reaction rate but not the rate constant.
only ii.
From the Arrhenius equation one can say that
rate constant always increases with increasing temperature
ΔS(universe) = 0
reversible
ΔS(universe) > 0
spontaneous (occurs without any outside intervention
Third Law of Thermodynamics
the entropy of a perfect crystalline substance is zero at 0 K
In the potential energy profile of a reaction, the species that exists at the maximum on the curve is called the
transition state
