At constant pressure,the combustion of 6.00 g of C4H10(g)releases 297 kJ of heat.What is ΔH for the reaction given below? 2 C4H10(g)+ 13 O2(g)→ 8 CO2(g)+ 10 H2O(l)

A) -54.2 kJ B) -779 kJ C) -6024 kJ D) -11508 kJ A) -54.2 kJ B) -779 kJ C) -6024 kJ D) -11508 kJ

For ?ES1U1B1sys S1U1B0to always be -,what must be TRUE?

A) q = w B) +q > -w C) +w > -q D) -w > +q A) q = w B) +q > -w C) +w > -q D) -w > +q

What volume of benzene (C6H6,d= 0.88 g/mL,molar mass = 78.11 g/mol)is required to produce 1.5 × 103 kJ of heat according to the following reaction? 2 C6H6(l)+ 15 O2(g)→ 12 CO2(g)+ 6 H2O(g)ΔH°rxn = -6278 kJ

A) 75 mL B) 37 mL C) 21 mL D) 19 mL E) 42 mL A) 75 mL B) 37 mL C) 21 mL D) 19 mL E) 42 mL

How much heat is absorbed/released when 25.00 g of NH3(g)reacts in the presence of excess (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) 428.6 kJ of heat are absorbed. B) 428.6 kJ of heat are released. C) 1715 kJ of heat are absorbed. D) 1715 kJ of heat are released. A) 428.6 kJ of heat are absorbed. B) 428.6 kJ of heat are released. C) 1715 kJ of heat are absorbed. D) 1715 kJ of heat are released.

Use the information provided to determine ΔH°rxn for the following reaction ΔH°f (kJ/mol)CH4(g)+ 4 Cl2(g)→ CCl4(g)+ 4 HCl(g)ΔH°rxn = ? CH4(g)-75 CCl4(g)-96 HCl(g)-92

A) -389 kJ B) -113 kJ C) +113 kJ D) -71 kJ E) +79 kJ A) -389 kJ B) -113 kJ C) +113 kJ D) -71 kJ E) +79 kJ

Use the information provided to determine ΔH°rxn for the following reaction ΔH°f (kJ/mol)CH4(g)+ 3 Cl2(g)→ CHCl3(l)+ 3 HCl(g)ΔH°rxn = ? CH4(g)-75 CHCl3(l)-134 HCl(g)-92

A) -151 kJ B) -335 kJ C) +662 kJ D) +117 kJ E) -217 kJ A) -151 kJ B) -335 kJ C) +662 kJ D) +117 kJ E) -217 kJ

Exam 10: Thermochemistry

When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C,169.5 kJ are absorbed and PΔV for the vaporization process is equal to 14.5 kJ then

(Multiple Choice)

4.9/5

(87)

Question 121

A piece of metal weighing 57.3 g is heated to a temperature of 88.0°C and is then immersed in 155 g of water at a temperature of 21.53°C.After equilibration the temperature is 24.72°C.If C_H2O = 4.184 J/g°C,what is C_metal?

(Multiple Choice)

4.8/5

(58)

Question 122

Using the following equation for the combustion of octane,calculate the amount of moles of carbon dioxide formed from 100.0 g of octane.The molar mass of octane is 114.33 g/mole.The molar mass of carbon dioxide is 44.0095 g/mole. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O ΔH°_rxn= -11018 kJ

(Multiple Choice)

4.8/5

(67)

Question 123

At constant pressure,the combustion of 6.00 g of C₄H₁₀(g)releases 297 kJ of heat.What is ΔH for the reaction given below? 2 C₄H₁₀(g)+ 13 O₂(g)→ 8 CO₂(g)+ 10 H₂O(l)

(Multiple Choice)

4.7/5

(74)

Question 124

Define molar heat capacity.

(Multiple Choice)

4.8/5

(68)

Question 125

Which of the following is TRUE if ΔE_sys = - 115 J?

(Multiple Choice)

4.7/5

(69)

Question 126

For ?E_systo always be -,what must be TRUE?

(Multiple Choice)

4.8/5

(85)

Question 127

What volume of benzene (C₆H₆,d= 0.88 g/mL,molar mass = 78.11 g/mol)is required to produce 1.5 × 10³ kJ of heat according to the following reaction? 2 C₆H₆(l)+ 15 O₂(g)→ 12 CO₂(g)+ 6 H₂O(g)ΔH°_rxn= -6278 kJ

(Multiple Choice)

4.8/5

(80)

Question 128

How much heat is absorbed/released when 25.00 g of NH₃(g)reacts in the presence of excess (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)

4.8/5

(81)

Question 129

Use the information provided to determine ΔH°_rxn for the following reaction ΔH°_f (kJ/mol)CH₄(g)+ 4 Cl₂(g)→ CCl₄(g)+ 4 HCl(g)ΔH°_rxn= ? CH₄(g)-75 CCl₄(g)-96 HCl(g)-92

(Multiple Choice)

4.8/5

(82)

Question 130

The specific heat capacity of liquid water is 4.18 J/g-K.How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1°C to 65.3°C?

(Multiple Choice)

4.9/5

(81)

Question 131

Use the information provided to determine ΔH°_rxn for the following reaction ΔH°_f (kJ/mol)CH₄(g)+ 3 Cl₂(g)→ CHCl₃(l)+ 3 HCl(g)ΔH°_rxn= ? CH₄(g)-75 CHCl₃(l)-134 HCl(g)-92

(Multiple Choice)

4.8/5

(68)

Question 132

How much energy is evolved during the reaction of 51.2 g of Al,according to the reaction below? Assume that there is excess Fe₂O₃. Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)ΔH°_rxn= -852 kJ

(Multiple Choice)

4.7/5

(89)

Question 133

A sample of NI3 is contained in a piston and cylinder.The samples rapidly decomposes to form nitrogen gas and iodine gas,and releases 3.30 kJ of heat and does 950 J of work.What is ∆E?

(Multiple Choice)

4.9/5

(89)

Question 134

A 21.8 g sample of ethanol (C₂H₅OH)is burned in a bomb calorimeter,according to the following reaction.If the temperature rises from 25.0 to 62.3°C,determine the heat capacity of the calorimeter.The molar mass of ethanol is 46.07 g/mol. C₂H₅OH(l)+ 3 O₂(g)→ 2 CO₂(g)+ 3 H₂O(g)ΔH°_rxn= -1235 kJ

(Multiple Choice)

4.8/5

(81)

Question 135

The specific heat capacity of methane gas is 2.20 J/g-K.How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C?

(Multiple Choice)

4.8/5

(76)

Question 136

Calculate the kinetic energy of a 150 g baseball moving at a speed of 39.m/s ( 87 mph).

(Multiple Choice)

4.7/5

(72)

Question 137

Which of the following is NOT a standard state?

(Multiple Choice)

4.9/5

(70)

Question 138

All the following are state functions EXCEPT

(Multiple Choice)

4.9/5

(66)

Question 139

In the presence of excess oxygen,methane gas burns in a constant-pressure system to yield carbon dioxide and water: (g)+ (g)→ (g)+ O(l)ΔH = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

(Multiple Choice)

4.8/5

(66)

Question 140

Showing 121 - 140 of 145

Exam 10: Thermochemistry

When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C,169.5 kJ are absorbed and PΔV for the vaporization process is equal to 14.5 kJ then

A piece of metal weighing 57.3 g is heated to a temperature of 88.0°C and is then immersed in 155 g of water at a temperature of 21.53°C.After equilibration the temperature is 24.72°C.If CH2O = 4.184 J/g°C,what is Cmetal?

Using the following equation for the combustion of octane,calculate the amount of moles of carbon dioxide formed from 100.0 g of octane.The molar mass of octane is 114.33 g/mole.The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

At constant pressure,the combustion of 6.00 g of C4H10(g)releases 297 kJ of heat.What is ΔH for the reaction given below? 2 C4H10(g)+ 13 O2(g)→ 8 CO2(g)+ 10 H2O(l)

Define molar heat capacity.

Which of the following is TRUE if ΔEsys = - 115 J?

For ?Esys to always be -,what must be TRUE?

What volume of benzene (C6H6,d= 0.88 g/mL,molar mass = 78.11 g/mol)is required to produce 1.5 × 103 kJ of heat according to the following reaction? 2 C6H6(l)+ 15 O2(g)→ 12 CO2(g)+ 6 H2O(g)ΔH°rxn = -6278 kJ

How much heat is absorbed/released when 25.00 g of NH3(g)reacts in the presence of excess (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

Use the information provided to determine ΔH°rxn for the following reaction ΔH°f (kJ/mol)CH4(g)+ 4 Cl2(g)→ CCl4(g)+ 4 HCl(g)ΔH°rxn = ? CH4(g)-75 CCl4(g)-96 HCl(g)-92

The specific heat capacity of liquid water is 4.18 J/g-K.How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1°C to 65.3°C?

Use the information provided to determine ΔH°rxn for the following reaction ΔH°f (kJ/mol)CH4(g)+ 3 Cl2(g)→ CHCl3(l)+ 3 HCl(g)ΔH°rxn = ? CH4(g)-75 CHCl3(l)-134 HCl(g)-92

How much energy is evolved during the reaction of 51.2 g of Al,according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s)+ 2 Al(s)→ Al2O3(s)+ 2 Fe(s)ΔH°rxn = -852 kJ

A sample of NI3 is contained in a piston and cylinder.The samples rapidly decomposes to form nitrogen gas and iodine gas,and releases 3.30 kJ of heat and does 950 J of work.What is ∆E?

A 21.8 g sample of ethanol (C2H5OH)is burned in a bomb calorimeter,according to the following reaction.If the temperature rises from 25.0 to 62.3°C,determine the heat capacity of the calorimeter.The molar mass of ethanol is 46.07 g/mol. C2H5OH(l)+ 3 O2(g)→ 2 CO2(g)+ 3 H2O(g)ΔH°rxn = -1235 kJ

The specific heat capacity of methane gas is 2.20 J/g-K.How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C?

Calculate the kinetic energy of a 150 g baseball moving at a speed of 39.m/s ( 87 mph).

Which of the following is NOT a standard state?

All the following are state functions EXCEPT

In the presence of excess oxygen,methane gas burns in a constant-pressure system to yield carbon dioxide and water: (g)+ (g)→ (g)+ O(l)ΔH = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

A piece of metal weighing 57.3 g is heated to a temperature of 88.0°C and is then immersed in 155 g of water at a temperature of 21.53°C.After equilibration the temperature is 24.72°C.If C_H2O = 4.184 J/g°C,what is C_metal?

Using the following equation for the combustion of octane,calculate the amount of moles of carbon dioxide formed from 100.0 g of octane.The molar mass of octane is 114.33 g/mole.The molar mass of carbon dioxide is 44.0095 g/mole. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O ΔH°_rxn= -11018 kJ

At constant pressure,the combustion of 6.00 g of C₄H₁₀(g)releases 297 kJ of heat.What is ΔH for the reaction given below? 2 C₄H₁₀(g)+ 13 O₂(g)→ 8 CO₂(g)+ 10 H₂O(l)

Which of the following is TRUE if ΔE_sys = - 115 J?

For ?E_systo always be -,what must be TRUE?

What volume of benzene (C₆H₆,d= 0.88 g/mL,molar mass = 78.11 g/mol)is required to produce 1.5 × 10³ kJ of heat according to the following reaction? 2 C₆H₆(l)+ 15 O₂(g)→ 12 CO₂(g)+ 6 H₂O(g)ΔH°_rxn= -6278 kJ

How much heat is absorbed/released when 25.00 g of NH₃(g)reacts in the presence of excess (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

Use the information provided to determine ΔH°_rxn for the following reaction ΔH°_f (kJ/mol)CH₄(g)+ 4 Cl₂(g)→ CCl₄(g)+ 4 HCl(g)ΔH°_rxn= ? CH₄(g)-75 CCl₄(g)-96 HCl(g)-92

Use the information provided to determine ΔH°_rxn for the following reaction ΔH°_f (kJ/mol)CH₄(g)+ 3 Cl₂(g)→ CHCl₃(l)+ 3 HCl(g)ΔH°_rxn= ? CH₄(g)-75 CHCl₃(l)-134 HCl(g)-92

How much energy is evolved during the reaction of 51.2 g of Al,according to the reaction below? Assume that there is excess Fe₂O₃. Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)ΔH°_rxn= -852 kJ