At constant pressure,the combustion of 25.0 g of C2H6(g)releases 1300 kJ of heat.What is ΔH for the reaction given below? 2 C2H6(g)+ 7 O2(g)→ 4 CO2(g)+ 6 H2O(l)

A) -215 kJ B) -390 kJ C) -1560 kJ D) -3120 kJ A) -215 kJ B) -390 kJ C) -1560 kJ D) -3120 kJ

Calculate the enthalpy of combustion per mole for C6H12O6.Assume that the combustion products are CO2(g)and H2O(l).

A) -5336 kJ/mol B) -2816 kJ/mol C) -1939 kJ/mol D) 580.7 kJ/mol A) -5336 kJ/mol B) -2816 kJ/mol C) -1939 kJ/mol D) 580.7 kJ/mol

How much heat is absorbed/released when 10.00 g of NH3(g)reacts in the presence of excess O2(g)to produce NO(g)and H2O(l)according to the following chemical equation? 4 NH3(g)+ 5 O2(g)→ 4 NO(g)+ 6 H2O(l)ΔH° = +1168 kJ

A) 171.5 kJ of heat are absorbed. B) 171.5 kJ of heat are released. C) 686.0 kJ of heat are absorbed. D) 686.0 kJ of heat are released. A) 171.5 kJ of heat are absorbed. B) 171.5 kJ of heat are released. C) 686.0 kJ of heat are absorbed. D) 686.0 kJ of heat are released.

Given: 4 NO2(g)+ O2(g)→ 2 N2O5(g)ΔH° = -110.2 kJ find ΔH° for 8 N2O5(g)→ 16 NO2(g)+ 4 O2(g).

A) -220.4 kJ B) -440.8 kJ C) 440.8 kJ D) 220.4 kJ A) -220.4 kJ B) -440.8 kJ C) 440.8 kJ D) 220.4 kJ

Exam 9: Thermochemistry: Chemical Energy

At constant pressure,the combustion of 25.0 g of C₂H₆(g)releases 1300 kJ of heat.What is ΔH for the reaction given below? 2 C₂H₆(g)+ 7 O₂(g)→ 4 CO₂(g)+ 6 H₂O(l)

(Multiple Choice)

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Question 41

A slice of cheese pizza has a caloric content of 550 Cal.If this energy could be used to power a 2500 Watt microwave oven,how many minutes could the microwave oven be operated? 1 W = 1 J/s

(Multiple Choice)

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Question 42

Calculate the enthalpy of combustion per mole for C₆H₁₂O₆.Assume that the combustion products are CO₂(g)and H₂O(l).

(Multiple Choice)

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Question 43

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.

(Multiple Choice)

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Question 44

The following drawing is a representation of the exothermic reaction in which ozone forms dioxygen. -This reaction is likely to be

(Multiple Choice)

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Question 45

When 1.0 mole of MgSO₄ is dissolved in water contained in a calorimeter,the temperature of the water and dissolved ions increases.Therefore the sign of ΔH for this reaction is ,heat is transferred the system the surroundings,and the reaction is classified as .

(Short Answer)

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Question 46

The net reaction is represented by

(Multiple Choice)

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Question 47

How much heat is absorbed/released when 10.00 g of NH₃(g)reacts in the presence of excess O₂(g)to produce NO(g)and H₂O(l)according to the following chemical equation? 4 NH₃(g)+ 5 O₂(g)→ 4 NO(g)+ 6 H₂O(l)ΔH° = +1168 kJ

(Multiple Choice)

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Question 48

At 1 atm pressure,the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol.To the correct number of significant figures,how much heat is required to melt 1.50 mol of gallium at 1 atm pressure?

(Multiple Choice)

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Question 49

A reaction for which ΔE = -850 kJ is one in which products have 850 kJ internal energy than the reactants,and products are stable than the reactants.

(Short Answer)

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Question 50

What are the signs of ΔH,ΔS,and ΔG for the following spontaneous change?

(Multiple Choice)

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Question 51

When 0.500 mol of CH₄(g)reacts with excess Cl₂(g)at constant pressure according to the chemical equation shown below,354 kJ of heat are released.Calculate the value of ΔH for this reaction,as written. 2 CH₄(g)+ 3 Cl₂(g)→ 2 CHCl₃(l)+ 3 H₂(g)ΔH = ?

(Multiple Choice)

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Question 52

For a particular process that is carried out at constant pressure,q = 200 kJ and w = -85 kJ.Therefore,

(Multiple Choice)

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Question 53

Which depends only on the initial and final state?

(Multiple Choice)

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Question 54

Which of the following scenarios involves a transfer of heat from system to surroundings?

(Multiple Choice)

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Question 55

Given: 4 NO₂(g)+ O₂(g)→ 2 N₂O₅(g)ΔH° = -110.2 kJ find ΔH° for 8 N₂O₅(g)→ 16 NO₂(g)+ 4 O₂(g).

(Multiple Choice)

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Question 56

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

(Multiple Choice)

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Question 57

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

(Multiple Choice)

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Question 58

Calculate the work energy,w,gained or lost by the system when a gas expands from 20 L to 35 L against a constant external pressure of 2.0 atm.[1 L ∙ atm = 101 J]

(Multiple Choice)

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Question 59

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.

(Short Answer)

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Question 60

Showing 41 - 60 of 170

Exam 9: Thermochemistry: Chemical Energy

At constant pressure,the combustion of 25.0 g of C2H6(g)releases 1300 kJ of heat.What is ΔH for the reaction given below? 2 C2H6(g)+ 7 O2(g)→ 4 CO2(g)+ 6 H2O(l)

A slice of cheese pizza has a caloric content of 550 Cal.If this energy could be used to power a 2500 Watt microwave oven,how many minutes could the microwave oven be operated? 1 W = 1 J/s

Calculate the enthalpy of combustion per mole for C6H12O6.Assume that the combustion products are CO2(g)and H2O(l).

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.

The following drawing is a representation of the exothermic reaction in which ozone forms dioxygen. -This reaction is likely to be

When 1.0 mole of MgSO4 is dissolved in water contained in a calorimeter,the temperature of the water and dissolved ions increases.Therefore the sign of ΔH for this reaction is ________,heat is transferred ________ the system ________ the surroundings,and the reaction is classified as ________.

The net reaction is represented by

How much heat is absorbed/released when 10.00 g of NH3(g)reacts in the presence of excess O2(g)to produce NO(g)and H2O(l)according to the following chemical equation? 4 NH3(g)+ 5 O2(g)→ 4 NO(g)+ 6 H2O(l)ΔH° = +1168 kJ

At 1 atm pressure,the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol.To the correct number of significant figures,how much heat is required to melt 1.50 mol of gallium at 1 atm pressure?

A reaction for which ΔE = -850 kJ is one in which products have 850 kJ ________ internal energy than the reactants,and products are ________ stable than the reactants.

What are the signs of ΔH,ΔS,and ΔG for the following spontaneous change?

When 0.500 mol of CH4(g)reacts with excess Cl2(g)at constant pressure according to the chemical equation shown below,354 kJ of heat are released.Calculate the value of ΔH for this reaction,as written. 2 CH4(g)+ 3 Cl2(g)→ 2 CHCl3(l)+ 3 H2(g)ΔH = ?

For a particular process that is carried out at constant pressure,q = 200 kJ and w = -85 kJ.Therefore,

Which depends only on the initial and final state?

Which of the following scenarios involves a transfer of heat from system to surroundings?

Given: 4 NO2(g)+ O2(g)→ 2 N2O5(g)ΔH° = -110.2 kJ find ΔH° for 8 N2O5(g)→ 16 NO2(g)+ 4 O2(g).

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

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

Calculate the work energy,w,gained or lost by the system when a gas expands from 20 L to 35 L against a constant external pressure of 2.0 atm.[1 L ∙ atm = 101 J]

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At constant pressure,the combustion of 25.0 g of C₂H₆(g)releases 1300 kJ of heat.What is ΔH for the reaction given below? 2 C₂H₆(g)+ 7 O₂(g)→ 4 CO₂(g)+ 6 H₂O(l)

Calculate the enthalpy of combustion per mole for C₆H₁₂O₆.Assume that the combustion products are CO₂(g)and H₂O(l).

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.

When 1.0 mole of MgSO₄ is dissolved in water contained in a calorimeter,the temperature of the water and dissolved ions increases.Therefore the sign of ΔH for this reaction is ,heat is transferred the system the surroundings,and the reaction is classified as .

How much heat is absorbed/released when 10.00 g of NH₃(g)reacts in the presence of excess O₂(g)to produce NO(g)and H₂O(l)according to the following chemical equation? 4 NH₃(g)+ 5 O₂(g)→ 4 NO(g)+ 6 H₂O(l)ΔH° = +1168 kJ

A reaction for which ΔE = -850 kJ is one in which products have 850 kJ internal energy than the reactants,and products are stable than the reactants.

When 0.500 mol of CH₄(g)reacts with excess Cl₂(g)at constant pressure according to the chemical equation shown below,354 kJ of heat are released.Calculate the value of ΔH for this reaction,as written. 2 CH₄(g)+ 3 Cl₂(g)→ 2 CHCl₃(l)+ 3 H₂(g)ΔH = ?

Given: 4 NO₂(g)+ O₂(g)→ 2 N₂O₅(g)ΔH° = -110.2 kJ find ΔH° for 8 N₂O₅(g)→ 16 NO₂(g)+ 4 O₂(g).