Given that ΔH°= -311 kJ for the hydrogenation of acetylene,C2H2: H-C=C-H(g)+ 2 H2(g)→ CH3-CH3(g) And the following bond dissociation energies,estimate a value for the C-to-C triple bond dissociation energy.

A) 1050 kJ/mol B) 833 kJ/mol C) 807 kJ/mol D) 397 kJ/mol A) 1050 kJ/mol B) 833 kJ/mol C) 807 kJ/mol D) 397 kJ/mol C

At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE° ? I.2 SO2(g)+ O2(g)→ 2 SO3(g) II.C3H8(g)+ 5 O2(g)→ 3 CO2(g)+ 4 H2O(l) III.H2(g)+ Cl2(g)→ 2 HCl(g) IV.N2O4(g)→ 2 NO2(g)

A) I) B) III. C) IV. D) II.and IV. A) I) B) III. C) IV. D) II.and IV.

Exam 8: Thermochemistry: Chemical Energy

Given that ΔH°= -311 kJ for the hydrogenation of acetylene,C₂H₂: H-C=C-H(g)+ 2 H₂(g)→ CH₃-CH₃(g) And the following bond dissociation energies,estimate a value for the C-to-C triple bond dissociation energy.

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Question 1

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Which is the most exothermic reaction?

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Question 2

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Find ΔE° for the reaction below if the process is carried out at a constant pressure of 1.00 atm and ΔV (the volume change)= -24.5 L.(1 L ∙ atm = 101 J) 2 CO(g)+ O₂ (g)→ 2 CO₂(g)ΔH° = -566.kJ

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Question 3

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When 0.455 g of anthracene,C₁₄H₁₀,is combusted in a bomb calorimeter that has a water jacket containing 500.g of water,the temperature of the water increases by 8.63°C.Assuming that the specific heat of water is 4.18 J/(g ∙ °C),and that the heat absorption by the calorimeter is negligible,estimate the enthalpy of combustion per mole of anthracene.

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Question 4

For a particular process that is carried out at constant pressure,q = 145 kJ and w = - 35 kJ.Therefore,

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Question 5

Which combination always results in a reaction being spontaneous?

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Question 6

It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0°C to 68.0°C.What is the specific heat of benzene?

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Question 7

When 2.000 moles of H₂(g)reacts with 1.000 mol of O₂(g)to form 2.000 mol of H₂O(l)at 25°C and a constant pressure of 1.00 atm.If 136.6 kJ of heat are released during this reaction,and PΔV is equal to -7.400 kJ,then

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Question 8

For the conversion of water to ice at 25°C and 1 atm,

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Question 9

For a process at constant pressure,49,600 calories of heat are released.This quantity of heat is equivalent to

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Question 10

The sign of ΔG for a reaction is if the reaction is spontaneous, if the reaction is at equilibrium,and if the reaction is nonspontaneous.

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Question 11

-The reaction represented in the above drawing is likely to be

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Question 12

Is thermal energy a form of kinetic or potential molecular energy?

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Question 13

At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE° ? I.2 SO₂(g)+ O₂(g)→ 2 SO₃(g) II.C₃H₈(g)+ 5 O₂(g)→ 3 CO₂(g)+ 4 H₂O(l) III.H₂(g)+ Cl₂(g)→ 2 HCl(g) IV.N₂O₄(g)→ 2 NO₂(g)

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Question 14

For the of freezing liquid ethanol at a given temperature and pressure,

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Question 15

Imagine a reaction that results in a change in both volume and temperature,as shown in the diagram below.What is the sign of the work being done and the sign of the enthalpy change involved in this reaction?

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Question 16

What is the thermodynamic criterion for equilibrium for a reaction at constant temperature and pressure (PV work only)?

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Question 17

When heated,mercury(II)oxide decomposes into elemental mercury and oxygen: 2 HgO(s)→ 2 Hg(l)+ O₂(g)ΔH° = 181.6 kJ ΔS° = 216.4 J/K Estimate the temperature at which HgO should begin to decompose if the partial pressure of O₂(g)is constant at 1.00 atm.

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Question 18

A reaction is performed in a 1-L balloon at 25°C and 1 atm pressure.At the end of the reaction the balloon has expanded to 1.5 L and the surface of the balloon has a temperature of 35°C and is at 1 atm pressure.Determine whether the signs of the heat transferred,the work,and the energy change,respectively,are positive or negative.

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Question 19

At 1 atm pressure the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol.How much heat is required to melt 1.50 mol of gallium at 1 atm pressure?

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Question 20

Showing 1 - 20 of 163

Exam 8: Thermochemistry: Chemical Energy

Given that ΔH°= -311 kJ for the hydrogenation of acetylene,C2H2: H-C=C-H(g)+ 2 H2(g)→ CH3-CH3(g) And the following bond dissociation energies,estimate a value for the C-to-C triple bond dissociation energy.

Which is the most exothermic reaction?

Find ΔE° for the reaction below if the process is carried out at a constant pressure of 1.00 atm and ΔV (the volume change)= -24.5 L.(1 L ∙ atm = 101 J) 2 CO(g)+ O2 (g)→ 2 CO2(g)ΔH° = -566.kJ

For a particular process that is carried out at constant pressure,q = 145 kJ and w = - 35 kJ.Therefore,

Which combination always results in a reaction being spontaneous?

It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0°C to 68.0°C.What is the specific heat of benzene?

When 2.000 moles of H2(g)reacts with 1.000 mol of O2(g)to form 2.000 mol of H2O(l)at 25°C and a constant pressure of 1.00 atm.If 136.6 kJ of heat are released during this reaction,and PΔV is equal to -7.400 kJ,then

For the conversion of water to ice at 25°C and 1 atm,

For a process at constant pressure,49,600 calories of heat are released.This quantity of heat is equivalent to

The sign of ΔG for a reaction is if the reaction is spontaneous,________ if the reaction is at equilibrium,and ________ if the reaction is nonspontaneous.

-The reaction represented in the above drawing is likely to be

Is thermal energy a form of kinetic or potential molecular energy?

At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE° ? I.2 SO2(g)+ O2(g)→ 2 SO3(g) II.C3H8(g)+ 5 O2(g)→ 3 CO2(g)+ 4 H2O(l) III.H2(g)+ Cl2(g)→ 2 HCl(g) IV.N2O4(g)→ 2 NO2(g)

For the of freezing liquid ethanol at a given temperature and pressure,

Imagine a reaction that results in a change in both volume and temperature,as shown in the diagram below.What is the sign of the work being done and the sign of the enthalpy change involved in this reaction?

What is the thermodynamic criterion for equilibrium for a reaction at constant temperature and pressure (PV work only)?

When heated,mercury(II)oxide decomposes into elemental mercury and oxygen: 2 HgO(s)→ 2 Hg(l)+ O2(g)ΔH° = 181.6 kJ ΔS° = 216.4 J/K Estimate the temperature at which HgO should begin to decompose if the partial pressure of O2(g)is constant at 1.00 atm.

At 1 atm pressure the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol.How much heat is required to melt 1.50 mol of gallium at 1 atm pressure?

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Given that ΔH°= -311 kJ for the hydrogenation of acetylene,C₂H₂: H-C=C-H(g)+ 2 H₂(g)→ CH₃-CH₃(g) And the following bond dissociation energies,estimate a value for the C-to-C triple bond dissociation energy.

Find ΔE° for the reaction below if the process is carried out at a constant pressure of 1.00 atm and ΔV (the volume change)= -24.5 L.(1 L ∙ atm = 101 J) 2 CO(g)+ O₂ (g)→ 2 CO₂(g)ΔH° = -566.kJ

When 2.000 moles of H₂(g)reacts with 1.000 mol of O₂(g)to form 2.000 mol of H₂O(l)at 25°C and a constant pressure of 1.00 atm.If 136.6 kJ of heat are released during this reaction,and PΔV is equal to -7.400 kJ,then

The sign of ΔG for a reaction is if the reaction is spontaneous, if the reaction is at equilibrium,and if the reaction is nonspontaneous.

At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE° ? I.2 SO₂(g)+ O₂(g)→ 2 SO₃(g) II.C₃H₈(g)+ 5 O₂(g)→ 3 CO₂(g)+ 4 H₂O(l) III.H₂(g)+ Cl₂(g)→ 2 HCl(g) IV.N₂O₄(g)→ 2 NO₂(g)

When heated,mercury(II)oxide decomposes into elemental mercury and oxygen: 2 HgO(s)→ 2 Hg(l)+ O₂(g)ΔH° = 181.6 kJ ΔS° = 216.4 J/K Estimate the temperature at which HgO should begin to decompose if the partial pressure of O₂(g)is constant at 1.00 atm.