chat 7 sec 1&2

Exothermic matches Choice ΔH < 0 Endothermic matches Choice ΔH > 0

Match each reaction enthalpy, ΔH, with the term that generally describes it. Exothermic Endothermic ΔH > 0 ΔH < 0

fuel

The amount of energy per gram of a given food is called its ______value.

entropy

The measure of the randomness or disorder of a chemical system is called

false

True or False: 1 Calorie = 1 calorie

greater than, endothermic less than; exothermic

When the energy required to break bonds is ______ the energy released when forming bonds in a chemical reaction, the reaction is characterized as ______. Select all that apply. Multiple select question. equal to; exothermic equal to; thermodynamic greater than, endothermic less than, thermodynamic less than; exothermic

Vaporization Expansion of a gas into an evacuated chamber Melting Sublimation

Which of the following processes are associated with an increase of entropy? Select all that apply. Multiple select question. The chemical reaction of two different gases to form a solid Vaporization Expansion of a gas into an evacuated chamber Melting Sublimation

ΔH - TΔS

ΔG = Multiple choice question. ΔH + TΔS ΔH - TΔS TΔS - ΔH ΔS - TΔH TΔS - TΔH

A Br—Br bond is broken. matches Endothermic A Br—Br bond is formed. matches Exothermic

Classify (match) each process as an exothermic or endothermic change. Instructions A Br—Br bond is broken. A Br—Br bond is formed. Endothermic Exothermic

Blank 1: exothermic Blank 2: endothermic

In an enthalpy diagram, when the reactants are shown to be higher in enthalpy than the products, the diagram represents an reaction. When the reactants are shown to be lower in enthalpy than the products, the diagram represents an reaction.

952 cal released

Is the following reaction spontaneous, non-spontaneous, or spontaneous depending on temperature? 3N2H4(ℓ) → 4NH3(g) + N2(g) + energy Multiple choice question. Nonspontaneous Spontaneous Spontaneous depending on temperature

Solid Liquid Gas

Rank the following states of matter for a given substance in order of increasing entropy. The state with the lowest entropy belongs at the top of the list. Instructions Liquid Solid Gas

lower

The _____ the specific heat, the less heat is required to raise the temperature of the substance. Multiple choice question. higher lower

entropy; potential energy

The drive toward increased ______, along with a tendency to achieve a lower ______, is responsible for spontaneous chemical reactions. Multiple choice question. potential energy; entropy entropy; potential energy enthalpy; energy kinetic energy; entropy entropy; rate of reaction

False

True or False: 1 Calorie = 1 calorie True false question.TrueFalse

Changes in energy as a chemical reaction occurs can be measured. Energy that is exchanged between the system and the surroundings in the form of heat can be measured through changes in temperature. Any energy that is lost from the system is gained by the surroundings.

Which of the following statements correctly describe energy changes in chemical reactions? Select all that apply. Changes in energy as a chemical reaction occurs can be measured. The absolute value for the energy stored in a chemical system can be measured. In some reactions, both the system and the surroundings gain energy. Energy that is exchanged between the system and the surroundings in the form of heat can be measured through changes in temperature. Any energy that is lost from the system is gained by the surroundings.

Gaseous molecules and atoms are in constant motion. Gaseous molecules and atoms undergo frequent collisions. The average kinetic energy of gaseous atoms or molecules increases with increasing temperature.

Which of the following statements correctly describe the kinetic molecular theory of gases? Select all that apply. Multiple select question. Gaseous molecules and atoms move with repeating, predictable patterns. Gaseous molecules and atoms are in constant motion. Gaseous molecules and atoms undergo frequent collisions. The average kinetic energy of gaseous atoms or molecules increases with increasing temperature.

Spontaneous process matches Does not require an outside source of energy to drive the process Nonspontaneous process matches Requires an outside source of energy to drive the process

match each type of process to the correct description. Instructions Spontaneous process Nonspontaneous process Requires an outside source of energy to drive the process Does not require an outside source of energy to drive the process

Tf = 30.5°C matches Choice The heat is released by the reaction. Tf = 19.2°C matches Choice The heat is absorbed by the reaction. The reaction is exothermic. matches Choice Tf = 32.1°C The reaction is endothermic. matches Choice Tf = 20.5°C

A calorimeter containing a solution initially with a temperature of 23.3°C is used to carry out different chemical reactions. Match the final temperature of each reaction mixture in the calorimeter to the type of reaction or heat transfer that took place. Instructions Tf = 30.5°C Tf = 19.2°C The reaction is exothermic. The reaction is endothermic. The heat is absorbed by the reaction. Tf = 20.5°C Tf = 32.1°C The heat is released by the reaction.

Calorimetry may be used to determine the heat of the reaction through measuring changes in temperature. Heat is transfered from the system to the surroundings. Some of the energy stored in the bonds of the reactants is converted to kinetic energy.

A combustion reaction results in an increase in temperature of the air surrounding the reaction. Which of the following statements correctly describe this process? Select all that apply. Multiple select question. Calorimetry may be used to determine the heat of the reaction through measuring changes in temperature. Collectively, the products of the reaction are higher in potential energy than the reactants. Heat is transfered from the system to the surroundings. Some of the energy stored in the bonds of the reactants is converted to kinetic energy. The molecules in the air that surround the reaction slow down.

the entropy of the products is greater than that of the reactants.

An increase in entropy for a chemical reaction occurs when ______. Multiple choice question. the entropy of the reactants is greater than that of the products. the enthalpy of the products is greater than that of the reactants. the enthalpy of the reactants is greater than that of the products. the entropy of the products is equal to the enthalpy of the products. the entropy of the products is greater than that of the reactants.

entropy

Apart from enthalpy changes, another factor that affects reaction spontaneity is , _____which is related to the freedom of movement within a system.

entropy

Apart from enthalpy changes, another factor that affects reaction spontaneity is ,_____ which is related to the freedom of movement within a system.

Blank 1: breaking, cleavage, dissociation, breakage, or cleaving Blank 2: formation, making, or forming

Bond ____always requires an input of energy, whereas bond _____involves a release of energy.

Blank 1: breaking, cleavage, dissociation, breakage, or cleaving Blank 2: formation, making, or forming

Bond_____ always requires an input of energy, whereas bond_____ involves a release of energy.

Sproducts - Sreactants

By definition, ΔSreaction = Multiple choice question. Sproducts/Sreactants Sproducts - Sreactants Sreactants/Sproducts Sproducts + Sreactants Sproducts × Sreactants

Sproducts - Sreactants

By definition, ΔSreaction = Multiple choice question. SproductsSreactants Sproducts + Sreactants Sproducts × Sreactants Sproducts - Sreactants Sreactants/Sproducts

An exothermic reaction with products that are higher in entropy matches Choice will occur spontaneously. An endothermic reaction with products that are lower in entropy matches Choice will not be spontaneous.

Complete each sentence to correctly describe spontaneous chemical reactions. Instructions An exothermic reaction with products that are higher in entropy An endothermic reaction with products that are lower in entropy will occur spontaneously. will not be spontaneous.

Blank 1: created Blank 2: destroyed

Energy can neither be nor ; it can only be converted from one form to another.

often; sometimes

Exothermic reactions are _____ spontaneous and endothermic reactions are _____ spontaneous. Multiple choice question. often; sometimes always; sometimes always; never sometimes; never

For an exothermic reaction matches heat released by the reaction is absorbed by the surrounding solution. For an endothermic reaction matches the reactants absorb heat from the solution. The temperature of the solution increases matches in the case of an exothermic reaction. The temperature of the solution decreases matches in the case of an endothermic reaction.

For an exothermic reaction For an endothermic reaction The temperature of the solution increases The temperature of the solution decreases heat released by the reaction is absorbed by the surrounding solution. in the case of an endothermic reaction. in the case of an exothermic reaction. the reactants absorb heat from the solution.

ΔG

Free energy change is symbolized by which of the following? Multiple choice question. ΔH ΔS ΔG T

gram

Fuel value is given as the number of nutritional Calories ______per of food.

gram

Fuel value is given as the number of nutritional Calories per of food.

Blank 1: exothermic Blank 2: endothermic

In an enthalpy diagram, when the reactants are shown to be higher in enthalpy than the products, the diagram represents an____- reaction. When the reactants are shown to be lower in enthalpy than the products, the diagram represents an ______reaction.

1000; Cal

In nutrition science, the nutritional Calorie is equal to ______ calorie(s) and has the symbol ______. Multiple choice question. 1000; Cal 1000; NCal 106; NCal one; Cal

Low entropy matches A well-organized system High entropy matches A random or disordered system S matches The symbol used to represent the entropy of a substance

Match each description of entropy to the correct symbol or terms. Instructions Low entropy Low entropy drop zone empty. High entropy High entropy drop zone empty. S S drop zone empty. A well-organized system A random or disordered system The symbol used to represent the entropy of a substance

Exothermic matches ΔH < 0 Endothermic matches ΔH > 0

Match each reaction enthalpy, ΔH, with the term that generally describes it. Instructions Exothermic Exothermic drop zone empty. Endothermic Endothermic drop zone empty. ΔH < 0 ΔH > 0

ΔH > 0, ΔS > 0 matches Choice Sign of ΔG depends on temperature. ΔH > 0, ΔS < 0 matches Choice ΔG > 0 at all temperatures ΔH < 0, ΔS > 0 matches Choice ΔG < 0 at all temperatures

Match each set of thermodynamic parameters to the correct description. Instructions ΔH > 0, ΔS > 0 ΔH > 0, ΔS < 0 ΔH < 0, ΔS > 0 Sign of ΔG depends on temperature. ΔG > 0 at all temperatures ΔG < 0 at all temperatures

Potential energy matches Can be in the form of energy stored in bonds Kinetic energy matches Can be in the form of thermal energy Heat (flow) matches The transfer of thermal energy from a system to the surroundings Calorimetry matches Experimental method for measuring temperature change and calculating heats of reactions

Match each term concerning energy and changes in energy to the correct description. Instructions Potential energy Kinetic energy Heat (flow) Calorimetry Can be in the form of energy stored in bonds Experimental method for measuring temperature change and calculating heats of reactions The transfer of thermal energy from a system to the surroundings Can be in the form of thermal energy

System matches Choice The process under study Surroundings matches Choice Everything in the universe other than the process under study Change in energy matches Choice Energy absorbed or released

Match each term to the correct description when describing changes in energy. System Surroundings Change in energy Energy absorbed or released Everything in the universe other than the process under study The process under study

Q matches cal ms matches g ΔTs matches °C SHs matches calg.°C

Match each term to the correct unit concerning the equation used in calorimetry: Q = ms × ΔTs × SHs Instructions Q ms ΔTs SHs °C cal/g.°C g cal

Exothermic reaction matches A + B → C + D + heat Endothermic reaction matches heat + A + B → C + D 55 kcal + A + B → C + D matches Endothermic reaction A + B → C + D + 55 kcal matches Exothermic reaction

Match each thermochemical equation to the correct description. Exothermic reaction Endothermic reaction 55 kcal + A + B → C + D A + B → C + D + 55 kcal Endothermic reaction heat + A + B → C + D A + B → C + D + heat Exothermic reaction

Spontaneous process matches Does not require an outside source of energy to drive the process Nonspontaneous process matches Requires an outside source of energy to drive the process

Match each type of process to the correct description. Instructions Spontaneous process Nonspontaneous process Does not require an outside source of energy to drive the process Requires an outside source of energy to drive the process

Exothermic reaction matches The reaction releases energy to the surroundings. Endothermic reaction matches The reaction absorbs energy from the surroundings.

Match each type of reaction to the correct definition. The reaction is defined as the system. Exothermic reaction Endothermic reaction The reaction releases energy to the surroundings. The reaction absorbs energy from the surroundings.

Endothermic reaction matches The energy required to break the bonds in the reactants is greater than the energy released from forming bonds in the products. Exothermic reaction matches The energy required to break the bonds in the reactants is less than the energy released from forming bonds in the products.

Match each type of reaction to the correct description concerning the following process: A—B + C—D → A—C + B—D Endothermic reaction Exothermic reaction The energy required to break the bonds in the reactants is greater than the energy released from forming bonds in the products. The energy required to break the bonds in the reactants is less than the energy released from forming bonds in the products.

Endothermic reaction matches Surroundings become colder as the reaction absorbs heat from the surroundings Exothermic reaction matches Surroundings become warmer as the reaction releases heat to the surroundings Energy is a reactant and is required in the reaction. matches Endothermic reaction Energy is a product and is released in the reaction. matches Exothermic reaction

Match each type of reaction to the correct description. Instructions Endothermic reaction Exothermic reaction Energy is a reactant and is required in the reaction. Energy is a product and is released in the reaction. Exothermic reaction Surroundings become colder as the reaction absorbs heat from the surroundings Surroundings become warmer as the reaction releases heat to the surroundings Endothermic reaction

Hreactants > Hproducts matches ΔHreaction < 0 Hreactants < Hproducts matches ΔHreaction > 0

Match the relative enthalpies of reactants and products to the correct change in enthalpy given ΔHreaction = Hproducts - Hreactants. Hreactants > Hproducts Hreactants>Hproducts drop zone empty. Hreactants < Hproducts Hreactants<Hproducts drop zone empty. ΔHreaction > 0 ΔHreaction < 0

Hreactants > Hproducts matches ΔHreaction < 0 Hreactants < Hproducts matches ΔHreaction > 0

Match the relative enthalpies of reactants and products to the correct change in enthalpy given ΔHreaction = Hproducts - Hreactants. Instructions Hreactants > Hproducts Hreactants < Hproducts ΔHreaction < 0 ΔHreaction > 0

Condensation matches Decrease in entropy Vaporization matches Increase in entropy Increase in entropy matches Decomposition of a liquid to form gaseous molecules Decrease in entropy matches Separation of a gaseous mixture into individual components

Matching Question Match each process to the correct change in entropy associated with it. Instructions Condensation Vaporization Increase in entropy Decrease in entropy Decomposition of a liquid to form gaseous molecules Increase in entropy Decrease in entropy Separation of a gaseous mixture into individual components

Solid Liquid Gas

Rank the following states of matter for a given substance in order of increasing entropy. The state with the lowest entropy belongs at the top of the list. Instructions Gas Solid Liquid

less than; exothermic greater than, endothermic

Select all that apply When the energy required to break bonds is ______ the energy released when forming bonds in a chemical reaction, the reaction is characterized as ______. Select all that apply. Multiple select question. less than; exothermic equal to; thermodynamic less than, thermodynamic greater than, endothermic equal to; exothermic

Free energy change is the combined contribution of the enthalpy and entropy values for a chemical reaction. Free energy change is the ultimate predictor of reaction spontaneity

Select all that apply Which of the following options correctly describe a change in free energy? Select all that apply. Multiple select question. Free energy change is the combined contribution of the enthalpy and entropy values for a chemical reaction. Free energy change represents the change in enthalpy between products and reactants. Free energy change represents the change in entropy between products and reactants. Free energy change is the ultimate predictor of reaction spontaneity.

ΔG < 0 ΔH < 0, ΔS > 0

Select all that apply Which sets of thermodynamic parameters represent a spontaneous process in terms of the system? Select all that apply. Multiple select question. ΔG < 0 ΔH < 0, ΔS > 0 ΔH > 0, ΔS < 0 at high temperatures ΔG > 0 at high temperatures

Blank 1: break Blank 2: form

Some molecular collisions, with sufficient energy, will ______bonds in molecules and allow for new ______bonds to

Substance A

Substance A has a specific heat of 1.2 calories/g °C. Substance B has a specific heat of 1.5 calories/g °C. If both substances are exposed to the same amount of heat, which substance will have a higher temperature? Multiple choice question. Substance A Substance B Both will be the same.

Blank 1: fuel

The amount of energy per gram of a given food is called its value.

Blank 1: products Blank 2: reactants

The change in enthalpy is the energy difference between the ____and ______of a chemical reaction and is symbolized as ΔH.

Energy cannot be created or destroyed, only converted from one form to another. The universe spontaneously tends toward increasing disorder or randomness.

The law(s) of thermodynamics that are relevant when predicting if a chemical reaction is spontaneous or not include(s) which of the following? Multiple select question. The disorder of a pure, perfect crystal at absolute zero is zero. Energy cannot be created or destroyed, only converted from one form to another. The universe spontaneously tends toward increasing disorder or randomness.

the number of calories of heat needed to raise the temperature of 1 gram of the substance 1 degree Celsius

The specific heat of a substance is defined as ______. Multiple choice question. the number of calories of heat needed to raise the temperature of 1 gram of the substance 1 degree Celsius the number of degrees Celsius the substance is raised when 1 gram of substance absorbs 1 calorie of heat the number of grams of the substance needed to result in a 1 degree Celsius temperature change after 1 calorie of heat is absorbed the specific amount of heat required to complete an endothermic chemical reaction

Blank 1: enthalpy Blank 2: entropy

The spontaneity of a chemical reaction depends on the relative magnitude of the and values.

heat energy work

Thermodynamics includes the study of _____. Select all that apply. Multiple select question. heat kinetics time energy work

the study of heat lost or gained when a substance changes phase the calculation of the quantity of energy released or consumed in a physical change the calculation of the quantity of heat obtained from a chemical reaction the study of energy, work, and heat for a chemical process

Thermodynamics may be applied to _____. Select all that apply. Multiple select question. the calculation of the time a chemical reaction requires to reach completion the study of heat lost or gained when a substance changes phase the calculation of the quantity of energy released or consumed in a physical change the calculation of the quantity of heat obtained from a chemical reaction the study of energy, work, and heat for a chemical process

Endothermic reaction matches Products are at a higher enthalpy than reactants. Exothermic reaction matches Products are at a lower enthalpy than reactants. Enthalpy (energy) is released when the reaction progresses from reactants to products. matches Exothermic reaction Enthalpy (energy) is required when the reaction progresses from reactants to products. matches Endothermic reaction

Use the figure shown to match each statement to the correct type of reaction. Instructions Endothermic reaction Exothermic reaction Enthalpy (energy) is released when the reaction progresses from reactants to products. Enthalpy (energy) is released when the reaction progresses from reactants to products. Enthalpy (energy) is required when the reaction progresses from reactants to products. Enthalpy (energy) is required when the reaction progresses from reactants to products. Products are at a higher enthalpy than reactants. Products are at a lower enthalpy than reactants. Endothermic reaction Exothermic reaction

ΔH < 0, ΔS > 0, ΔG < 0

What are the signs of ΔH, ΔS, and ΔG for the following reaction? C6H12O6(s) → 2C2H5OH(l) + 2CO2(g) + 16 kcal Multiple choice question. ΔH > 0, ΔS > 0, ΔG > 0 ΔH < 0, ΔS > 0, ΔG > 0 ΔH > 0, ΔS < 0, ΔG > 0 ΔH < 0, ΔS > 0, ΔG < 0 ΔH > 0, ΔS > 0, ΔG < 0

Energy cannot be created or destroyed. The disorder of a pure, perfect crystal at absolute zero (0 Kelvin) is zero. The universe spontaneously tends toward increasing disorder or randomness.

What are the three basic laws of thermodynamics? Select all that apply. Multiple select question. Energy cannot be created or destroyed. Energy cannot be converted from one form to another. The disorder of a pure, perfect crystal at absolute zero (0 Kelvin) is zero. All chemical reactions occur spontaneously. The universe spontaneously tends toward increasing disorder or randomness.

An increase in entropy The chemical reaction is exothermic. ΔSreaction > 0

What factors favor a spontaneous chemical reaction? Select all that apply. Multiple select question. ΔHreaction > 0 An increase in entropy ΔHreaction = ΔSreaction The chemical reaction is exothermic. ΔSreaction > 0

ΔSreaction > 0 The chemical reaction is exothermic. An increase in entropy

What factors favor a spontaneous chemical reaction? Select all that apply. Multiple select question. ΔSreaction > 0 ΔHreaction = ΔSreaction The chemical reaction is exothermic. ΔHreaction > 0 An increase in entropy

released; absorbed

When a chlorine-chlorine bond is formed, 58 kcal of energy is ______. To break the same bond, 58 kcal of energy is ______. absorbed; released absorbed; absorbed released; released released; absorbed

Calorimetry involves the measurement of the change in temperature of a quantity of water or solution that is in contact with a reaction. The device used to measure heat changes in a system is called a calorimeter. Calorimetry is the measurement of heat energy changes in a chemical reaction.

Which of the following options correctly describe calorimetry? Select all that apply. Multiple select question. Calorimetry involves the measurement of the change in temperature of a quantity of water or solution that is in contact with a reaction. The device used to measure heat changes in a system is called a calorimeter. Calorimetry is the measurement of heat energy changes in a chemical reaction. In calorimetry, heat escapes from the system to the surroundings and is lost; therefore, temperature changes are measured for the system only.

Calorimetry is the measurement of heat energy changes in a chemical reaction. The device used to measure heat changes in a system is called a calorimeter. Calorimetry involves the measurement of the change in temperature of a quantity of water or solution that is in contact with a reaction.

Which of the following options correctly describe calorimetry? Select all that apply. Multiple select question. Calorimetry is the measurement of heat energy changes in a chemical reaction. In calorimetry, heat escapes from the system to the surroundings and is lost; therefore, temperature changes are measured for the system only. The device used to measure heat changes in a system is called a calorimeter. Calorimetry involves the measurement of the change in temperature of a quantity of water or solution that is in contact with a reaction.

The change in enthalpy is represented by the symbol ΔH. The change in enthalpy is the energy difference between the products and reactants of a chemical reaction. Enthalpy is a term used to represent heat.

Which of the following options correctly describes enthalpy? Multiple select question. The change in enthalpy is always a positive value. The change in enthalpy is represented by the symbol ΔH. The change in enthalpy is the energy difference between the products and reactants of a chemical reaction. Enthalpy is a term used to represent heat.

B + CD → AD + BC + heat The reaction of 1 mole of CH4(g) with 1 mole of Cl2(g) releases 26.4 kcal of heat.

Which of the following options represent(s) an exothermic reaction? Multiple select question. The decomposition of NO2(g) to NO(g) and O2(g) requires energy. AB + CD → AD + BC + heat 18 kcal + CH4(g) → C(s) + 2H2(g) The reaction of 1 mole of CH4(g) with 1 mole of Cl2(g) releases 26.4 kcal of heat.

A + B → C + D, ΔH = 21.1 kcal SO2(g) → S(s) + O2(g), ΔH = 71 kcal

Which of the following processes are endothermic? Select all that apply. Multiple select question. A + B → C + D, ΔH = 21.1 kcal 2HNO3(ℓ) → N2O5(g) + H2O (ℓ), ΔH = -18.3 kcal SO2(g) → S(s) + O2(g), ΔH = 71 kcal AB + CD → AD + BC, ΔH = -10.3 kcal

H—CI: → H· + CI: H—O—H → H —O· + ·H

Which of the following reactions are endothermic? Choose all that apply. Multiple select question. H· + Br: → H — Br: H—CI: → H· + CI: H—O—H → H —O· + ·H

CH4(g) + 2O2(g) → CO2(g) + 2H2O(ℓ) + 213 kcal C6H12O6(s) → 2C2H6O(ℓ) + 2CO2(g) + 16 kcal

Which of the following reactions are exothermic? Select all that apply. Multiple select question. CH4(g) + 2O2(g) → CO2(g) + 2H2O(ℓ) + 213 kcal C6H12O6(s) → 2C2H6O(ℓ) + 2CO2(g) + 16 kcal 22.0 kcal + 2NH3(g) → 3H2(g) + N2(g)

H2O(g) CO2(g

Which of the following substances is/are expected to have a higher entropy than H2O(l)? Select all that apply. Multiple select question. H2O(s) CO2(s) H2O(g) CO2(g)

ΔG < 0 matches Spontaneous process ΔG > 0 matches Nonspontaneous process ΔH < 0 matches Exothermic process ΔH > 0 matches Endothermic process ΔS > 0 matches Process moves to a state of increased disorder.

ΔG < 0 ΔG > 0 ΔH < 0 ΔH > 0 ΔS > 0 Endothermic process Spontaneous process Nonspontaneous process Process moves to a state of increased disorder. Exothermic process