When 1 mole of Fe2O3(s) reacts with H2(g) to form Fe(s) and H2O(g) by the following reaction, 98.8 kJ of energy is absorbed. Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H2O(g) (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above Represents this reaction?

A) Endothermic; A B) Endothermic; B C) Exothermic; A D) Exothermic; B E) None of these A) Endothermic; A B) Endothermic; B C) Exothermic; A D) Exothermic; B E) None of these

Determine the heat of evaporation of carbon disulfide, CS2( $\ell$ ) ? CS2(g) Given the enthalpies of reaction below. C(s) + 2 S(s) ? CS2( $\ell$ ) ?rH° = +89.4 kJ/mol-rxn C(s) + 2 S(s) ? CS2(g) ?rH° = +116.7 kJ/mol-rxn

A) -206.1 kJ B) -27.3 kJ C) +27.3 kJ D) +206.1 kJ E) +1.31 kJ A) -206.1 kJ B) -27.3 kJ C) +27.3 kJ D) +206.1 kJ E) +1.31 kJ

Determine the standard enthalpy of formation of calcium carbonate from the thermochemical equations given below. \[\begin{array} { l l } \mathrm { Ca } ( \mathrm { OH } ) _ { 2 } ( \mathrm {~s} ) \rightarrow \mathrm { CaO } ( \mathrm { s } ) + \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) & \Delta _ { r } H ^ { \circ } = 65.2 \mathrm {~kJ} / \mathrm { mol } - \mathrm { rxn } \\ \mathrm { Ca } ( \mathrm { OH } ) _ { 2 } ( \mathrm {~s} ) + \mathrm { CO } _ { 2 } ( \mathrm {~g} ) \rightarrow \mathrm { CaCO } _ { 3 } ( \mathrm {~s} ) + \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) & \Delta _ { r } H ^ { \circ } = - 113.8 \mathrm {~kJ} / \mathrm { mol } - \mathrm { rxn } \\ \mathrm { C } ( \mathrm { s } ) + \mathrm { O } _ { 2 } ( \mathrm {~g} ) \rightarrow \mathrm { CO } _ { 2 } ( \mathrm {~g} ) & \Delta _ { r } H ^ { \circ } = - 393.5 \mathrm {~kJ} / \mathrm { mol } - \mathrm { rxn } \\ 2 \mathrm { Ca } ( \mathrm { s } ) + \mathrm { O } _ { 2 } ( \mathrm {~g} ) \rightarrow 2 \mathrm { CaO } ( \mathrm { s } ) & \Delta _ { r } H ^ { \circ } = - 1270.2 \mathrm {~kJ} / \mathrm { mol } - \mathrm { rxn } \end{array}\]

A) ?1712.3 kJ/mol-rxn B) ?441.8 kJ/mol-rxn C) ?849.6 kJ/mol-rxn D) ?980.6 kJ/mol-rxn E) ?1207.6 kJ/mol-rxn A) ?1712.3 kJ/mol-rxn B) ?441.8 kJ/mol-rxn C) ?849.6 kJ/mol-rxn D) ?980.6 kJ/mol-rxn E) ?1207.6 kJ/mol-rxn

Given the thermochemical equation 4AlCl3(s) + 3O2(g) ? 2Al2O3(s) + 6Cl2(g); ?rH = -529 kJ/mol-rxn Find ?rH For the following reaction. $\frac { 1 } { 3 }$ Al2O3(s) + Cl2(g) ? $\frac{2}{3}$ AlCl3(s) + $\frac { 1 } { 2 }$ O2(g)

A) 88.2 kJ/mol-rxn B) 264.5 kJ/mol-rxn C) 529 kJ/mol-rxn D) 176.3 kJ/mol-rxn E) -176.3 kJ/mol-rxn A) 88.2 kJ/mol-rxn B) 264.5 kJ/mol-rxn C) 529 kJ/mol-rxn D) 176.3 kJ/mol-rxn E) -176.3 kJ/mol-rxn

Using the following thermochemical data: \[\begin{array} { l l } 2 \mathrm { Sm } ( s ) + 6 \mathrm { HF } ( g ) \rightarrow 2 \mathrm { SmF } _ { 3 } ( s ) + 3 \mathrm { H } _ { 2 } ( g ) & \Delta _ { r } H ^ { \circ } = - 1929.4 \mathrm {~kJ} / \text { mol-rxn } \\ 2 \mathrm { Sm } ( s ) + 6 \mathrm { HCl } ( g ) \rightarrow 2 \mathrm { SmCl } _ { 3 } ( s ) + 3 \mathrm { H } _ { 2 } ( g ) & \Delta _ { r } H ^ { \circ } = - 1498.0 \mathrm {~kJ} / \mathrm { mol } - \mathrm { rxn } \end{array}\] Calculate ?rH° for the following reaction: SmF3(s) + 3HCl(g) ? SmCl3(s) + 3HF(g)

A) -3427.4 kJ/mol-rxn B) 431.4 kJ/mol-rxn C) 215.7 kJ/mol-rxn D) 862.8 kJ/mol-rxn E) -1713.7 kJ/mol-rxn A) -3427.4 kJ/mol-rxn B) 431.4 kJ/mol-rxn C) 215.7 kJ/mol-rxn D) 862.8 kJ/mol-rxn E) -1713.7 kJ/mol-rxn

What is the standard enthalpy of formation of CaCO3(s)+ CaO(s) + CO2(g) ? CaCO3(s); ?H° = -179.4 kJ/mol-rxn \[\begin{array} { l l } \text { Substance } & \Delta _ { f } H ^ { \circ } ( \mathrm { kJ } / \text { mol-rxn } ) \\ \mathrm { CaO } ( s ) & - 634.9 \\ \mathrm { CO } _ { 2 } ( g ) & - 393.5 \end{array}\]

A) 62.0 kJ/mol-rxn B) -420.8 kJ/mol-rxn C) -849.0 kJ/mol-rxn D) -1207.8 kJ/mol-rxn E) 849.0 kJ/mol-rxn A) 62.0 kJ/mol-rxn B) -420.8 kJ/mol-rxn C) -849.0 kJ/mol-rxn D) -1207.8 kJ/mol-rxn E) 849.0 kJ/mol-rxn

Exam 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

When 1 mole of Fe₂O₃(s) reacts with H₂(g) to form Fe(s) and H₂O(g) by the following reaction, 98.8 kJ of energy is absorbed. Fe₂O₃(s) + 3 H₂(g) → 2 Fe(s) + 3 H₂O(g) (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above Represents this reaction?

(Multiple Choice)

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Question 21

Determine the heat of evaporation of carbon disulfide, CS₂( $\ell$ ) ? CS₂(g) Given the enthalpies of reaction below. C(s) + 2 S(s) ? CS₂( $\ell$ ) ?_rH° = +89.4 kJ/mol-rxn C(s) + 2 S(s) ? CS₂(g) ?_rH° = +116.7 kJ/mol-rxn

(Multiple Choice)

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Question 22

Determine the standard enthalpy of formation of calcium carbonate from the thermochemical equations given below. (()\rightarrow()+(\ell) =65.2/- (()+()\rightarrow()+(\ell) =-113.8/- ()+()\rightarrow() =-393.5/- 2()+()\rightarrow2() =-1270.2/-

(Multiple Choice)

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Question 23

Given the thermochemical equation 4AlCl₃(s) + 3O₂(g) ? 2Al₂O₃(s) + 6Cl₂(g); ?_rH = -529 kJ/mol-rxn Find ?_rH For the following reaction. $\frac { 1 } { 3 }$ Al₂O₃(s) + Cl₂(g) ? $\frac{2}{3}$ AlCl₃(s) + $\frac { 1 } { 2 }$ O₂(g)

(Multiple Choice)

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Question 24

CaO(s) reacts with water to form Ca(OH)₂(aq). If 6.50 g CaO is combined with 99.70 g H₂O in a coffee cup calorimeter, the temperature of the resulting solution increases from 21.7 °C to 43.1 °C. Calculate the enthalpy change for the reaction per mole of CaO. Assume that the specific heat capacity of the solution is 4.18 J/g⋅K.

(Multiple Choice)

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Question 25

Calculate the energy in the form of heat (in kJ) required to convert 325 grams of liquid water at 20.0 °C to steam at 115 °C. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: liquid water = 4.184 J/g⋅K, steam = 1.92 J/g⋅K)

(Multiple Choice)

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Question 26

What quantity, in moles, of hydrogen is consumed when 179.6 kJ of energy is evolved from the combustion of a mixture of H₂(g) and O₂(g)? H₂(g) + $\frac { 1 } { 2 }$ O₂(g) ? H₂O(l); ?_rH° = -285.8 kJ/mol-rxn

(Multiple Choice)

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Question 27

How much heat is liberated at constant pressure if 0.515 g of calcium carbonate reacts with 32.7 mL of 0.498 M hydrochloric acid? CaCO₃(s) + 2HCl(aq) → CaCl₂(aq) + H₂O(l) + CO₂(g); Δ_rH° = -15.2 kJ/mol-rxn

(Multiple Choice)

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Question 28

A chemical reaction in a bomb calorimeter evolves 3.86 kJ of energy in the form of heat. If the temperature of the bomb calorimeter increases by 4.17 K, what is the heat capacity of the calorimeter?

(Multiple Choice)

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Question 29

Which of the following has zero standard enthalpy of formation at 25 °C?

(Multiple Choice)

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Question 30

Which of the following reactions corresponds to the thermochemical equation for the standard molar enthalpy of formation of solid zinc nitrate?

(Multiple Choice)

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Question 31

If 35.0 g H₂O at 22.7 °C is combined with 65.0 g H₂O at 87.5 °C, what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g⋅K.

(Multiple Choice)

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Question 32

Using the following thermochemical data: 2(s)+6(g)\rightarrow2(s)+3(g) =-1929.4/ mol-rxn 2(s)+6(g)\rightarrow2(s)+3(g) =-1498.0/- Calculate ?_rH° for the following reaction: SmF₃(s) + 3HCl(g) ? SmCl₃(s) + 3HF(g)

(Multiple Choice)

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Question 33

The heat of vaporization of benzene, C₆H₆, is 30.7 kJ/mol at its boiling point of 80.1 °C. How much energy in the form of heat is required to vaporize 102 g benzene at its boiling point?

(Multiple Choice)

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Question 34

What is the standard enthalpy of formation of CaCO₃(s)+ CaO(s) + CO₂(g) ? CaCO₃(s); ?H° = -179.4 kJ/mol-rxn Substance (/ mol-rxn ) (s) -634.9 (g) -393.5

(Multiple Choice)

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Question 35

What is the minimum mass of ice at 0.0 °C that must be added to 1.00 kg of water to cool the water from 28.0 °C to 12.0 °C? (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g⋅K, liquid water = 4.184 J/g⋅K)

(Multiple Choice)

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Question 36

Calculate the energy in the form of heat (in kJ) required to change 76.9 g of liquid water at 25.2 °C to ice at -15.2 °C. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: ice = 2.06 J/g⋅K, liquid water = 4.184 J/g⋅K)

(Multiple Choice)

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Question 37

According to the reaction given below, the standard enthalpy change for the combustion of 1 mole of propane is -2043.0 kJ. C₃H₈(g) + 5 O₂(g) ? 3 CO₂(g) + 4 H₂O(g) Calculate ?_fH° for propane based on the given standard molar enthalpies of formation. molecule \Delta(/ mol-rxn ) () -393.5 () -241.8

(Multiple Choice)

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Question 38

If 50.0 g of benzene (C₆H₆) absorbs 2.71 kJ of energy in the form of heat at 25.0 °C, what is the final temperature of benzene? The specific heat capacity of benzene is 1.72 J/g ⋅ K.

(Multiple Choice)

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Question 39

Exactly 149.6 J will raise the temperature of 10.0 g of a metal from 25.0 °C to 60.0 °C. What is the specific heat capacity of the metal?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 69

Exam 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

When 1 mole of Fe2O3(s) reacts with H2(g) to form Fe(s) and H2O(g) by the following reaction, 98.8 kJ of energy is absorbed. Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H2O(g) (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above Represents this reaction?

Determine the heat of evaporation of carbon disulfide, CS2( ℓ\ellℓ ) ? CS2(g) Given the enthalpies of reaction below. C(s) + 2 S(s) ? CS2( ℓ\ellℓ ) ?rH° = +89.4 kJ/mol-rxn C(s) + 2 S(s) ? CS2(g) ?rH° = +116.7 kJ/mol-rxn

Determine the standard enthalpy of formation of calcium carbonate from the thermochemical equations given below. (()\rightarrow()+(\ell) =65.2/- (()+()\rightarrow()+(\ell) =-113.8/- ()+()\rightarrow() =-393.5/- 2()+()\rightarrow2() =-1270.2/-

Given the thermochemical equation 4AlCl3(s) + 3O2(g) ? 2Al2O3(s) + 6Cl2(g); ?rH = -529 kJ/mol-rxn Find ?rH For the following reaction. 13\frac { 1 } { 3 }31​ Al2O3(s) + Cl2(g) ? 23\frac{2}{3}32​ AlCl3(s) + 12\frac { 1 } { 2 }21​ O2(g)

What quantity, in moles, of hydrogen is consumed when 179.6 kJ of energy is evolved from the combustion of a mixture of H2(g) and O2(g)? H2(g) + 12\frac { 1 } { 2 }21​ O2(g) ? H2O(l); ?rH° = -285.8 kJ/mol-rxn

How much heat is liberated at constant pressure if 0.515 g of calcium carbonate reacts with 32.7 mL of 0.498 M hydrochloric acid? CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g); ΔrH° = -15.2 kJ/mol-rxn

A chemical reaction in a bomb calorimeter evolves 3.86 kJ of energy in the form of heat. If the temperature of the bomb calorimeter increases by 4.17 K, what is the heat capacity of the calorimeter?

Which of the following has zero standard enthalpy of formation at 25 °C?

Which of the following reactions corresponds to the thermochemical equation for the standard molar enthalpy of formation of solid zinc nitrate?

If 35.0 g H2O at 22.7 °C is combined with 65.0 g H2O at 87.5 °C, what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g⋅K.

Using the following thermochemical data: 2(s)+6(g)\rightarrow2(s)+3(g) =-1929.4/ mol-rxn 2(s)+6(g)\rightarrow2(s)+3(g) =-1498.0/- Calculate ?rH° for the following reaction: SmF3(s) + 3HCl(g) ? SmCl3(s) + 3HF(g)

The heat of vaporization of benzene, C6H6, is 30.7 kJ/mol at its boiling point of 80.1 °C. How much energy in the form of heat is required to vaporize 102 g benzene at its boiling point?

What is the standard enthalpy of formation of CaCO3(s)+ CaO(s) + CO2(g) ? CaCO3(s); ?H° = -179.4 kJ/mol-rxn Substance (/ mol-rxn ) (s) -634.9 (g) -393.5

What is the minimum mass of ice at 0.0 °C that must be added to 1.00 kg of water to cool the water from 28.0 °C to 12.0 °C? (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g⋅K, liquid water = 4.184 J/g⋅K)

According to the reaction given below, the standard enthalpy change for the combustion of 1 mole of propane is -2043.0 kJ. C3H8(g) + 5 O2(g) ? 3 CO2(g) + 4 H2O(g) Calculate ?fH° for propane based on the given standard molar enthalpies of formation. molecule \Delta(/ mol-rxn ) () -393.5 () -241.8

If 50.0 g of benzene (C6H6) absorbs 2.71 kJ of energy in the form of heat at 25.0 °C, what is the final temperature of benzene? The specific heat capacity of benzene is 1.72 J/g ⋅ K.

Exactly 149.6 J will raise the temperature of 10.0 g of a metal from 25.0 °C to 60.0 °C. What is the specific heat capacity of the metal?

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Determine the heat of evaporation of carbon disulfide, CS₂( $\ell$ ) ? CS₂(g) Given the enthalpies of reaction below. C(s) + 2 S(s) ? CS₂( $\ell$ ) ?_rH° = +89.4 kJ/mol-rxn C(s) + 2 S(s) ? CS₂(g) ?_rH° = +116.7 kJ/mol-rxn

Given the thermochemical equation 4AlCl₃(s) + 3O₂(g) ? 2Al₂O₃(s) + 6Cl₂(g); ?_rH = -529 kJ/mol-rxn Find ?_rH For the following reaction. $\frac { 1 } { 3 }$ Al₂O₃(s) + Cl₂(g) ? $\frac{2}{3}$ AlCl₃(s) + $\frac { 1 } { 2 }$ O₂(g)

What quantity, in moles, of hydrogen is consumed when 179.6 kJ of energy is evolved from the combustion of a mixture of H₂(g) and O₂(g)? H₂(g) + $\frac { 1 } { 2 }$ O₂(g) ? H₂O(l); ?_rH° = -285.8 kJ/mol-rxn

How much heat is liberated at constant pressure if 0.515 g of calcium carbonate reacts with 32.7 mL of 0.498 M hydrochloric acid? CaCO₃(s) + 2HCl(aq) → CaCl₂(aq) + H₂O(l) + CO₂(g); Δ_rH° = -15.2 kJ/mol-rxn

If 35.0 g H₂O at 22.7 °C is combined with 65.0 g H₂O at 87.5 °C, what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g⋅K.

Using the following thermochemical data: 2(s)+6(g)\rightarrow2(s)+3(g) =-1929.4/ mol-rxn 2(s)+6(g)\rightarrow2(s)+3(g) =-1498.0/- Calculate ?_rH° for the following reaction: SmF₃(s) + 3HCl(g) ? SmCl₃(s) + 3HF(g)

The heat of vaporization of benzene, C₆H₆, is 30.7 kJ/mol at its boiling point of 80.1 °C. How much energy in the form of heat is required to vaporize 102 g benzene at its boiling point?

What is the standard enthalpy of formation of CaCO₃(s)+ CaO(s) + CO₂(g) ? CaCO₃(s); ?H° = -179.4 kJ/mol-rxn Substance (/ mol-rxn ) (s) -634.9 (g) -393.5

If 50.0 g of benzene (C₆H₆) absorbs 2.71 kJ of energy in the form of heat at 25.0 °C, what is the final temperature of benzene? The specific heat capacity of benzene is 1.72 J/g ⋅ K.