Review for Chem110 Test 7 Deltech-Owens Campus
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| Thermodynamics is __ | The study of energy, work, and heat.
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| A system contains __ | the process under study
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| Surroundings are | the rest of the universe
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| First law of Thermodynamics | Energy of the universe is constant
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| Another name for the first law of thermodynamics is | The law of conservation of energy
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| Every chemical bond is really __ | stored chemical energy
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| Bonds must __ for a reaction to occur | break
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| Breaking bonds requires __ | energy
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| When energy from a system is released into its surroundings, this is called an __ reaction. | exothermic
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| When energy from a system's surroundings is released into the system, this is called an __ reaction | endothermic
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| If the energy required to break a chemical bond is __ than the energy released when the bonds are formed, there is a net __ of energy. This is a __ reaction. | less, release, exothermic
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| If the energy required to break a chemical bond is __ than the energy released when the bond is formed, there will be an __ __ of energy. This is a __ reaction. | larger/greater, external supply, endothermic
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| If the equation ends with +#kcal (or C), it is __. | exothermic
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| If the equation begins with #kcal (or C), it is __. | endothermic
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| Enthalpy represents __ | heat energy
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| The energy difference between the products and reactants of a chemical reaction is __ | enthalpy
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| When energy is __, the enthalpy charge is __. (As in -#kcal or -C.) This is an __ reaction. | released, negative, exothermic
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| When energy is __, the enthalpy charge is __. (As in +#kcal or +C. )This is an __ reaction. | absorbed, positive, endothermic
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| When a reaction occurs without any external energy input, it is a __ reaction. | spontaneous
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| Most __ reactions are spontaneous. | exothermic
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| __ is used to predict if a reaction will occur. | Thermodynamics
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| Besides thermodynamics, another factor used to predict whether a chemical reaction will occur or not is called __. | entropy
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| Exothermic reactions are always __. | negative
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| T or F: Fuel oil burned in a furnace is an example of an endothermic reaction. | false, it's exothermic
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| The 2nd Law of Thermodynamics says that __ | the universe spontaneously tends toward increasing disorder or randomness
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| Entropy is __ | a measure of the randomness of a chemical system
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| When a system has high entropy, that means it is __ | highly disordered, or lacking a repeating and regular pattern
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| When a system has low entropy, that means it is __ | well organized. It may have a crystalline structure.
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| There is no such thing as __ entropy. | negative
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| A positive (+) ΔS means an __ in the disorder of the reaction. | increase
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| A negative (-) ΔS means a __ in the disorder of the reaction. | decrease
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| Name 3 processes that have positive entropy. | melting, vaporization, dissolution (they all have a +ΔS)
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| If a reaction is exothermic and has a +ΔS, then it is __ | spontaneous
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| If a reaction is endothermic and has a -ΔS, is is __ | nonspontaneous
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| If a reaction is not endothermic or exothermic, then it is spontaneous or nonspontaneous based on the relative size of __ and __. | ΔH and ΔS
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| Gas has __ entropy than water. | greater or more (gas is highly disorganized)
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| A solid has __ entropy than water. | less (solids are highly organized)
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| Free energy is represented by a __ | ΔG
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| Free energy represents the __ | combined contribution of the enthalpy and entropy values for a chemical reaction
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| Free energy predicts __ of chemical reactions | spontaneity
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| Negative ΔG is always __ | spontaneous
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| Positive ΔG is always __ | nonspontaneous
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| In an equation, the letter T stands for __ | temperature in Kelvin
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| What do you need to know to predict the sign of ΔG of a reaction? | ΔH and ΔS
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| Calorimetry is the __ | measurement of heat energy changes in a chemical reaction
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| A calorimeter is a __ | device which measures heat changes in calories
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| The change in temperature measured by a calorimeter is used to measure the __ | loss or gain of heat
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| In an exothermic reaction, heat that has been released is __ | absorbed
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| In an endothermic reaction, reactants __ heat from the solution | absorb
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| Specific heat, or SH, is the __ | number of calories of heat needed to raise the temperature of 1 g of the substance by 1 degree C
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| Regarding specific heat, what is the formula you must remember? | Q=ms X ΔT X SHs (the lower case s stands for solution, or for our purposes, water)
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| The specific heat (HS) for water is __ | 1.0 cal/g degrees C
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| To determine heat released or absorbed, you need to know __ | specific heat, total grams of solution, temperature change (did it increase or decrease?)
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| If you see a word problem on the test, remember that __ are not needed to work the equation. | moles
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| A capital C, or kilocalorie, is also used as a __ calorie. | nutritional
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| Thermal kinetics is the study of __ | the rate, or speed, of chemical reactions.
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| Kinetic information represents changes over __ | time
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| Change in __ can be used to monitor the progress of a chemical reaction | color
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| The __ of color change can help us calculate the rate of the chemical reaction | rate
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| If sufficient energy is available, chemical bonds will break and atoms will recombine in a __ __ arrangement | lower energy
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| An __ collision is one that produces product molecules | effective
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| Activation energy is the __ | minimum amount of energy required to initiate a chemical reaction.
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| An activated complex is __ | an extremely unstable, short-lived intermediate complex
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| An activated complex cannot be __ from the reaction mixture | isolated
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| Activation energy is the __ between the energy of the reactants and that of the activated complex. | difference
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| What are the 6 factors that affect reaction rate? | 1) structure of reacting species 2) molecular shape and orientation 3) concentration of reactants 4) temp of reactants 5) physical state of reactants 6) presence of a catalyst
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| In a reaction, oppositely charged species reactant more __ | rapidly
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| Ions with the same charge __ | do not react
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| The magnitude of the activation energy is related to __ | bond strength
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| The rate of a reaction will generally increase as the concentration __ | increases
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| A higher kinetic energy means a __ of these collisions will result in product formation | higher percentage
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| Reactions are fastest in the __ state and slowest in the __ state. | liquid, gaseous
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| A catalyst is a __ | substance that increases the reaction rate of a chemical reaction.
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| The catalyst __ __ __ the final product of the reaction and undergoes no net change. | does not alter
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| Equilibrium reactions are __ | incomplete chemical reactions.
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| When a chemical reaction is complete, that means that all __ | reactants have been converted to products.
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| Physical equilibria reactions are __ | reversible
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| Examples of reversible reactions, or physical equilibrium reactions, include: | dissolved oxygen in lake water, stalactite formation, sugar dissolved in water
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| A reversible reaction is a process that __ | can occur in both directions and uses the the double arrow symbol
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| You have dynamic equilibrium when the rate __ | of the forward process in a reversible reaction is exactly balanced by the rate of the process in reverse
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| T or F: if you add 100 g of sugar to 100 mL of water, nothing happens. | False, even though it may appear that way
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| Equilibrium occurs when the rate __ | of reactant depletion is equal to the rate of product depletion
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| LeChateleir's Principle says that __ | if a stress is placed on a system at equilibrium, the system will respond by altering the equilibrium composition to minimize the stress
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| The term "stressed," as applied in LeChateleir's Principle, means that the equilibrium will be __ | disturbed
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| Pressure affects equilibrium only if one or more of the substances in the reaction are __ | gases
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| The relative number of gas moles on reactant and product side must __ to effect pressure | differ
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| When pressure goes up, it shifts to the side with __ | less moles of gas
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| A catalyst affects the rate of both the forward and reverse reaction to the __ extant | same
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