Find the standard enthalpy of formation of ethylene, C2H4(g), given the following data: heat of combustion of C2H4(g)= -1411 kJ/mol; $\Delta$H$\circ$f[CO2(g)] = -393.5 kJ/mol; $\Delta$H$\circ$f[H2O(l)] = -285.8 kJ/mol.

A) 52 kJ/mol B) 87 kJ/mol C) 731 kJ/mol D) 1.41 * 103 kJ/mol E) 2.77 * 103 kJ/mol A) 52 kJ/mol B) 87 kJ/mol C) 731 kJ/mol D) 1.41 * 103 kJ/mol E) 2.77 * 103 kJ/mol

Find $\Delta$H$\circ$rxn for the reaction 2Ag2S(s) + 2H2O(l) $\rarr$ 4Ag(s) + 2H2S(g) + O2(g).[$\Delta$H$\circ$f (Ag2S(s)) = -32.6 kJ/mol; $\Delta$H$\circ$f (H2S(g)) = -20.5 kJ/mol; $\Delta$H$\circ$f (H2O(l)) = -285.5 kJ/mol]

A) 595.2 kJ/mol B) 585.2 kJ/mol C) 575.2 kJ/mol D) 565.2 kJ/mol E) None of the above A) 595.2 kJ/mol B) 585.2 kJ/mol C) 575.2 kJ/mol D) 565.2 kJ/mol E) None of the above

Ethanol (C2H5OH) burns according to the equation C2H5OH(l) + 3O2(g) $\rarr$ 2CO2(g) + 3H2O(l), $\Delta$H$\circ$rxn = -1367 kJ/mol.How much heat is released when 35.0 g of ethanol is burned

A) 9.61 * 10-4 kJ B) 1,040 kJ C) 1,367 kJ D) 1,797 kJ E) 4.78 * 104 kJ A) 9.61 * 10-4 kJ B) 1,040 kJ C) 1,367 kJ D) 1,797 kJ E) 4.78 * 104 kJ

The bond enthalpy of the Br-Cl bond is equal to $\Delta$E$\circ$ for the reaction BrCl(g) $\rarr$ Br(g) + Cl(g).Use the following data to find the bond enthalpy of the Br-Cl bond. $\begin{array}{ll} \mathrm{Br}_{2}(\mathrm{l}) \rightarrow \mathrm{Br}_{2}(\mathrm{~g}) & \Delta \mathrm{H}^{\circ}=30.91 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{Br}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{Br}(\mathrm{~g}) & \Delta \mathrm{H}^{\circ}=192.9 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{Cl}(\mathrm{~g}) & \Delta \mathrm{H}^{\circ}=243.4 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{Br}_{2}(\mathrm{l})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{BrCl}(\mathrm{~g}) & \Delta \mathrm{H}^{\circ}=29.2 \mathrm{~kJ} / \mathrm{mol} \end{array}$

A) 14.6 kJ/mol B) 203.5 kJ/mol C) 219.0 kJ/mol D) 438.0 kJ/mol E) 407.0 kJ/mol A) 14.6 kJ/mol B) 203.5 kJ/mol C) 219.0 kJ/mol D) 438.0 kJ/mol E) 407.0 kJ/mol

Calculate the enthalpy of reaction for H2(g) + C2H4(g) $\rarr$ C2H6(g).[$\Delta$H$\circ$f(C2H4(g)) = 52.3 kJ/mol; $\Delta$H$\circ$f(C2H6(g)) = -84.7 kJ/mol]

A) -117 kJ/mol B) -127 kJ/mol C) -137 kJ/mol D) -147 kJ/mol E) None of the above A) -117 kJ/mol B) -127 kJ/mol C) -137 kJ/mol D) -147 kJ/mol E) None of the above

The combustion of pentane produces heat according to the equation C5H12(l) + 8O2(g) $\rarr$ 5CO2(g) + 6H2O(l), $\Delta$H$\circ$rxn= -3,510 kJ/mol.How many grams of CO2 are produced per 2.50 * 103 kJ of heat released

A) 0.0809 g B) 3.56 g C) 31.3 g D) 157 g E) 309 g A) 0.0809 g B) 3.56 g C) 31.3 g D) 157 g E) 309 g

Calculate the standard enthalpy change for the reaction 2A + 2A2 + 4AB + B $\rarr$ 5A2B Given: $\begin{array}{ll} 2 \mathrm{~A}+\mathrm{B} \rightarrow \mathrm{~A}_{2} \mathrm{~B} & \Delta \mathrm{H}^{\circ}=-25.0 \mathrm{~kJ} / \mathrm{mol} \\ 2 \mathrm{~A}_{2} \mathrm{~B} \rightarrow 2 \mathrm{AB}+\mathrm{A}_{2} & \Delta \mathrm{H}^{\circ}=35.0 \mathrm{~kJ} / \mathrm{mol} \end{array}$

A) - 95.0 kJ/mol B) - 60.0 kJ/mol C) - 15.0 kJ/mol D) 10.0 kJ/mol E) 45.0 kJ/mol A) - 95.0 kJ/mol B) - 60.0 kJ/mol C) - 15.0 kJ/mol D) 10.0 kJ/mol E) 45.0 kJ/mol

Calculate the heat released (kJ) in the reaction of 2.20 g of sulfur dioxide gas and excess oxygen gas to form sulfur trioxide gas: 2SO2(g) + O2(g) $\rarr$2SO3(g) Given: S(s) + O2(g) $\rarr$SO2(g) $\Delta$H = -299 kJ/mol S(s) + 3/2O2(g) $\rarr$ SO3(g) $\Delta$H = -395 kJ/mol

A) 3.10 kJ B) 3.20 kJ C) 3.30 kJ D) 3.40 kJ E) None of the above A) 3.10 kJ B) 3.20 kJ C) 3.30 kJ D) 3.40 kJ E) None of the above

Exam 6: Thermochemistry

The enthalpy change when a strong acid is neutralized by strong base is -56.1 kJ/mol. If 135 mL of 0.450 M HI at 23.15^$\circ$C is mixed with 145 mL of 0.500 M NaOH, also at 23.15^$\circ$C, what is the maximum temperature reached by the resulting solution (Assume that there is no heat loss to the container, that the specific heat of the final solution is 4.18 J/g·^$\circ$C, and that the density of the final solution is that of water.)

(Multiple Choice)

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Question 41

Calculate the amount of work done, in joules, when 2.5 mole of H₂O vaporizes at 1.0 atm and 25^$\circ$C. Assume the volume of liquid H₂O is negligible compared to that of vapor. (1 L·atm = 101.3 J)

(Multiple Choice)

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Question 42

Find the standard enthalpy of formation of ethylene, C₂H₄(g), given the following data: heat of combustion of C₂H₄(g)= -1411 kJ/mol; $\Delta$ H^$\circ$_f[CO₂(g)] = -393.5 kJ/mol; $\Delta$ H^$\circ$_f[H₂O(l)] = -285.8 kJ/mol.

(Multiple Choice)

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Question 43

Find $\Delta$ H^$\circ$_rxn for the reaction $2 \mathrm{Na}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow 2 \mathrm{NaOH}(\mathrm{aq})+2 \mathrm{H}_{2}(\mathrm{~g})$ . $\left[\Delta \mathrm{H}^{\circ}{ }_{\mathrm{f}}(\mathrm{NaOH}(\mathrm{aq}))=-426.8 \mathrm{~kJ} / \mathrm{mol} ; \Delta \mathrm{H}^{\circ}{ }_{\mathrm{f}}\left(\mathrm{H}_{2} \mathrm{O}(\mathrm{l})\right)=-285.5 \mathrm{~kJ} / \mathrm{mol}\right]$

(Multiple Choice)

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Question 44

Find $\Delta$ H^$\circ$_rxn for the reaction 2Ag₂S(s) + 2H₂O(l) $\rarr$ 4Ag(s) + 2H₂S(g) + O₂(g).[ $\Delta$ H^$\circ$_f (Ag₂S(s)) = -32.6 kJ/mol; $\Delta$ H^$\circ$_f (H₂S(g)) = -20.5 kJ/mol; $\Delta$ H^$\circ$_f (H₂O(l)) = -285.5 kJ/mol]

(Multiple Choice)

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Question 45

Ethanol (C₂H₅OH) burns according to the equation C₂H₅OH(l) + 3O₂(g) $\rarr$ 2CO₂(g) + 3H₂O(l), $\Delta$ H^$\circ$_rxn = -1367 kJ/mol.How much heat is released when 35.0 g of ethanol is burned

(Multiple Choice)

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Question 46

The bond enthalpy of the Br-Cl bond is equal to $\Delta$ E^$\circ$ for the reaction BrCl(g) $\rarr$ Br(g) + Cl(g).Use the following data to find the bond enthalpy of the Br-Cl bond. ()\rightarrow() \Delta=30.91/ ()\rightarrow2() \Delta=192.9/ ()\rightarrow2() \Delta=243.4/ ()+()\rightarrow2() \Delta=29.2/

(Multiple Choice)

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Question 47

Calculate the enthalpy of reaction for H₂(g) + C₂H₄(g) $\rarr$ C₂H₆(g).[ $\Delta$ H^$\circ$_f(C₂H₄(g)) = 52.3 kJ/mol; $\Delta$ H^$\circ$_f(C₂H₆(g)) = -84.7 kJ/mol]

(Multiple Choice)

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Question 48

A 0.3423 g sample of pentane, C₅H₁₂, was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.000 kg of water contained therein rose from 20.22^$\circ$C to 22.82^$\circ$C. The heat capacity of the calorimeter is 2.21 kJ/^$\circ$C. The heat capacity of water = 4.184 J/g·^$\circ$C. How much heat was given off during combustion of the sample of pentane

(Multiple Choice)

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Question 49

The combustion of pentane produces heat according to the equation C₅H₁₂(l) + 8O₂(g) $\rarr$ 5CO₂(g) + 6H₂O(l), $\Delta$ H^$\circ$_rxn= -3,510 kJ/mol.How many grams of CO₂ are produced per 2.50 * 10³ kJ of heat released

(Multiple Choice)

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Question 50

Aluminum oxide can be reduced to aluminum metal using carbon, the other reaction product being carbon monoxide. Determine the enthalpy change when 12.5 g of aluminum is produced by this method. [ $\Delta$ H^$\circ$_f(carbon monoxide) = -110.5 kJ/mol; $\Delta$ H^$\circ$_f(aluminum oxide) = -1669.8 kJ/mol]

(Multiple Choice)

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Question 51

At 25^$\circ$C, the standard enthalpy of formation of anhydrous sodium carbonate is -1130.9 kJ/mol, whereas the standard enthalpy of formation of sodium carbonate monohydrate is -1430.1 kJ/mol. Determine $\Delta$ H^$\circ$ at 25^$\circ$C for the reaction Na₂CO₃(s) + H₂O(l) $\rarr$ Na₂CO₃·H₂O(s).(Given: $\Delta$ H^$\circ$_f[H₂O(l)] = -285.8 kJ/mol)

(Multiple Choice)

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Question 52

The heat of solution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH₄NO₃ is added to 40.0 mL of water in a calorimeter at 23.5^$\circ$C, what is the minimum temperature reached by the solution (The specific heat of water = 4.18 J/g·^$\circ$C; the heat capacity of the calorimeter = 650. J/^$\circ$C.)

(Multiple Choice)

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Question 53

A 26.2 g piece of copper metal is heated from 21.5^$\circ$C to 201.6^$\circ$C. Calculate the amount of heat absorbed by the metal. The specific heat of Cu is 0.385 J/g·^$\circ$C.

(Multiple Choice)

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Question 54

When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000. g of water, a temperature rise of 3.60^$\circ$C was observed. What is the heat capacity of the bomb calorimeter, excluding the water The heat of combustion of benzoic acid is -26.42 kJ/g.

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Question 55

Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. The heat of combustion of naphthalene is -40.1 kJ/g. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000. g of water, a temperature rise of 4.21^$\circ$C was observed. What is the heat capacity of the bomb calorimeter excluding the water

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Question 56

For which of these reactions will the difference between $\Delta$ H^$\circ$ and $\Delta$ E^$\circ$be the greatest

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Question 57

Calculate the standard enthalpy change for the reaction 2A + 2A₂ + 4AB + B $\rarr$ 5A₂B Given: 2+\rightarrow \Delta=-25.0/ 2\rightarrow2+ \Delta=35.0/

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Question 58

Calculate the heat released (kJ) in the reaction of 2.20 g of sulfur dioxide gas and excess oxygen gas to form sulfur trioxide gas: 2SO₂(g) + O₂(g) $\rarr$ 2SO₃(g) Given: S(s) + O₂(g) $\rarr$ SO₂(g) $\Delta$ H = -299 kJ/mol S(s) + 3/2O₂(g) $\rarr$ SO₃(g) $\Delta$ H = -395 kJ/mol

(Multiple Choice)

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Question 59

The heat of solution of LiCl is -37.1 kJ/mol, and the lattice energy of LiCl(s) is 828 kJ/mol. Calculate the total heat of hydration of 1.00 mol of gas phase Li⁺ ions and Cl^- ions.

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Question 60

Showing 41 - 60 of 119

Calculate the amount of work done, in joules, when 2.5 mole of H₂O vaporizes at 1.0 atm and 25^$\circ$C. Assume the volume of liquid H₂O is negligible compared to that of vapor. (1 L·atm = 101.3 J)

Find the standard enthalpy of formation of ethylene, C₂H₄(g), given the following data: heat of combustion of C₂H₄(g)= -1411 kJ/mol; $\Delta$ H^$\circ$_f[CO₂(g)] = -393.5 kJ/mol; $\Delta$ H^$\circ$_f[H₂O(l)] = -285.8 kJ/mol.

Find $\Delta$ H^$\circ$_rxn for the reaction 2Ag₂S(s) + 2H₂O(l) $\rarr$ 4Ag(s) + 2H₂S(g) + O₂(g).[ $\Delta$ H^$\circ$_f (Ag₂S(s)) = -32.6 kJ/mol; $\Delta$ H^$\circ$_f (H₂S(g)) = -20.5 kJ/mol; $\Delta$ H^$\circ$_f (H₂O(l)) = -285.5 kJ/mol]

Ethanol (C₂H₅OH) burns according to the equation C₂H₅OH(l) + 3O₂(g) $\rarr$ 2CO₂(g) + 3H₂O(l), $\Delta$ H^$\circ$_rxn = -1367 kJ/mol.How much heat is released when 35.0 g of ethanol is burned

Calculate the enthalpy of reaction for H₂(g) + C₂H₄(g) $\rarr$ C₂H₆(g).[ $\Delta$ H^$\circ$_f(C₂H₄(g)) = 52.3 kJ/mol; $\Delta$ H^$\circ$_f(C₂H₆(g)) = -84.7 kJ/mol]

The combustion of pentane produces heat according to the equation C₅H₁₂(l) + 8O₂(g) $\rarr$ 5CO₂(g) + 6H₂O(l), $\Delta$ H^$\circ$_rxn= -3,510 kJ/mol.How many grams of CO₂ are produced per 2.50 * 10³ kJ of heat released

A 26.2 g piece of copper metal is heated from 21.5^$\circ$C to 201.6^$\circ$C. Calculate the amount of heat absorbed by the metal. The specific heat of Cu is 0.385 J/g·^$\circ$C.

When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000. g of water, a temperature rise of 3.60^$\circ$C was observed. What is the heat capacity of the bomb calorimeter, excluding the water The heat of combustion of benzoic acid is -26.42 kJ/g.

For which of these reactions will the difference between $\Delta$ H^$\circ$ and $\Delta$ E^$\circ$be the greatest

Calculate the standard enthalpy change for the reaction 2A + 2A₂ + 4AB + B $\rarr$ 5A₂B Given: 2+\rightarrow \Delta=-25.0/ 2\rightarrow2+ \Delta=35.0/

Calculate the heat released (kJ) in the reaction of 2.20 g of sulfur dioxide gas and excess oxygen gas to form sulfur trioxide gas: 2SO₂(g) + O₂(g) $\rarr$ 2SO₃(g) Given: S(s) + O₂(g) $\rarr$ SO₂(g) $\Delta$ H = -299 kJ/mol S(s) + 3/2O₂(g) $\rarr$ SO₃(g) $\Delta$ H = -395 kJ/mol

The heat of solution of LiCl is -37.1 kJ/mol, and the lattice energy of LiCl(s) is 828 kJ/mol. Calculate the total heat of hydration of 1.00 mol of gas phase Li⁺ ions and Cl^- ions.

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Exam 6: Thermochemistry

Calculate the amount of work done, in joules, when 2.5 mole of H2O vaporizes at 1.0 atm and 25 ∘\circ∘ C. Assume the volume of liquid H2O is negligible compared to that of vapor. (1 L·atm = 101.3 J)

Find the standard enthalpy of formation of ethylene, C2H4(g), given the following data: heat of combustion of C2H4(g)= -1411 kJ/mol; Δ\DeltaΔ H ∘\circ∘ f[CO2(g)] = -393.5 kJ/mol; Δ\DeltaΔ H ∘\circ∘ f[H2O(l)] = -285.8 kJ/mol.

Find Δ\DeltaΔ H ∘\circ∘ rxn for the reaction 2Ag2S(s) + 2H2O(l) →\rarr→ 4Ag(s) + 2H2S(g) + O2(g).[ Δ\DeltaΔ H ∘\circ∘ f (Ag2S(s)) = -32.6 kJ/mol; Δ\DeltaΔ H ∘\circ∘ f (H2S(g)) = -20.5 kJ/mol; Δ\DeltaΔ H ∘\circ∘ f (H2O(l)) = -285.5 kJ/mol]

Ethanol (C2H5OH) burns according to the equation C2H5OH(l) + 3O2(g) →\rarr→ 2CO2(g) + 3H2O(l), Δ\DeltaΔ H ∘\circ∘ rxn = -1367 kJ/mol.How much heat is released when 35.0 g of ethanol is burned

Calculate the enthalpy of reaction for H2(g) + C2H4(g) →\rarr→ C2H6(g).[ Δ\DeltaΔ H ∘\circ∘ f(C2H4(g)) = 52.3 kJ/mol; Δ\DeltaΔ H ∘\circ∘ f(C2H6(g)) = -84.7 kJ/mol]

The combustion of pentane produces heat according to the equation C5H12(l) + 8O2(g) →\rarr→ 5CO2(g) + 6H2O(l), Δ\DeltaΔ H ∘\circ∘ rxn= -3,510 kJ/mol.How many grams of CO2 are produced per 2.50 * 103 kJ of heat released

A 26.2 g piece of copper metal is heated from 21.5 ∘\circ∘ C to 201.6 ∘\circ∘ C. Calculate the amount of heat absorbed by the metal. The specific heat of Cu is 0.385 J/g· ∘\circ∘ C.

When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000. g of water, a temperature rise of 3.60 ∘\circ∘ C was observed. What is the heat capacity of the bomb calorimeter, excluding the water The heat of combustion of benzoic acid is -26.42 kJ/g.

For which of these reactions will the difference between Δ\DeltaΔ H ∘\circ∘ and Δ\DeltaΔ E ∘\circ∘ be the greatest

Calculate the standard enthalpy change for the reaction 2A + 2A2 + 4AB + B →\rarr→ 5A2B Given: 2+\rightarrow \Delta=-25.0/ 2\rightarrow2+ \Delta=35.0/

Calculate the heat released (kJ) in the reaction of 2.20 g of sulfur dioxide gas and excess oxygen gas to form sulfur trioxide gas: 2SO2(g) + O2(g) →\rarr→ 2SO3(g) Given: S(s) + O2(g) →\rarr→ SO2(g) Δ\DeltaΔ H = -299 kJ/mol S(s) + 3/2O2(g) →\rarr→ SO3(g) Δ\DeltaΔ H = -395 kJ/mol

The heat of solution of LiCl is -37.1 kJ/mol, and the lattice energy of LiCl(s) is 828 kJ/mol. Calculate the total heat of hydration of 1.00 mol of gas phase Li+ ions and Cl- ions.

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Calculate the amount of work done, in joules, when 2.5 mole of H₂O vaporizes at 1.0 atm and 25^$\circ$C. Assume the volume of liquid H₂O is negligible compared to that of vapor. (1 L·atm = 101.3 J)

Find the standard enthalpy of formation of ethylene, C₂H₄(g), given the following data: heat of combustion of C₂H₄(g)= -1411 kJ/mol; $\Delta$ H^$\circ$_f[CO₂(g)] = -393.5 kJ/mol; $\Delta$ H^$\circ$_f[H₂O(l)] = -285.8 kJ/mol.

Find $\Delta$ H^$\circ$_rxn for the reaction 2Ag₂S(s) + 2H₂O(l) $\rarr$ 4Ag(s) + 2H₂S(g) + O₂(g).[ $\Delta$ H^$\circ$_f (Ag₂S(s)) = -32.6 kJ/mol; $\Delta$ H^$\circ$_f (H₂S(g)) = -20.5 kJ/mol; $\Delta$ H^$\circ$_f (H₂O(l)) = -285.5 kJ/mol]

Ethanol (C₂H₅OH) burns according to the equation C₂H₅OH(l) + 3O₂(g) $\rarr$ 2CO₂(g) + 3H₂O(l), $\Delta$ H^$\circ$_rxn = -1367 kJ/mol.How much heat is released when 35.0 g of ethanol is burned

Calculate the enthalpy of reaction for H₂(g) + C₂H₄(g) $\rarr$ C₂H₆(g).[ $\Delta$ H^$\circ$_f(C₂H₄(g)) = 52.3 kJ/mol; $\Delta$ H^$\circ$_f(C₂H₆(g)) = -84.7 kJ/mol]

The combustion of pentane produces heat according to the equation C₅H₁₂(l) + 8O₂(g) $\rarr$ 5CO₂(g) + 6H₂O(l), $\Delta$ H^$\circ$_rxn= -3,510 kJ/mol.How many grams of CO₂ are produced per 2.50 * 10³ kJ of heat released

A 26.2 g piece of copper metal is heated from 21.5^$\circ$C to 201.6^$\circ$C. Calculate the amount of heat absorbed by the metal. The specific heat of Cu is 0.385 J/g·^$\circ$C.

When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000. g of water, a temperature rise of 3.60^$\circ$C was observed. What is the heat capacity of the bomb calorimeter, excluding the water The heat of combustion of benzoic acid is -26.42 kJ/g.

For which of these reactions will the difference between $\Delta$ H^$\circ$ and $\Delta$ E^$\circ$be the greatest

Calculate the standard enthalpy change for the reaction 2A + 2A₂ + 4AB + B $\rarr$ 5A₂B Given: 2+\rightarrow \Delta=-25.0/ 2\rightarrow2+ \Delta=35.0/

Calculate the heat released (kJ) in the reaction of 2.20 g of sulfur dioxide gas and excess oxygen gas to form sulfur trioxide gas: 2SO₂(g) + O₂(g) $\rarr$ 2SO₃(g) Given: S(s) + O₂(g) $\rarr$ SO₂(g) $\Delta$ H = -299 kJ/mol S(s) + 3/2O₂(g) $\rarr$ SO₃(g) $\Delta$ H = -395 kJ/mol

The heat of solution of LiCl is -37.1 kJ/mol, and the lattice energy of LiCl(s) is 828 kJ/mol. Calculate the total heat of hydration of 1.00 mol of gas phase Li⁺ ions and Cl^- ions.