Question 1

The specific heat of silver is 0.235 J/g·$\circ$C. How many joules of heat are required to heat a 75 g silver spoon from 20$\circ$C to 35$\circ$C

Accepted Answer

A)  240 J 
B)  250 J 
C)  260 J 
D)  270 J 
E)  None of the above 
A)  240 J 
B)  250 J 
C)  260 J 
D)  270 J 
E)  None of the above

Question 2

Calculate the standard enthalpy change for the reaction 2C8H18(l) + 21O2(g) $\rarr$8CO(g) + 8CO2(g) + 18H2O(l).Given:
2C8H18(l) + 25O2(g) $\rarr$16CO2(g) + 18H2O(l) $\Delta$H$\circ$ = -11,020 kJ/mol
2CO(g) + O2(g) $\rarr$ 2CO2(g) $\Delta$H$\circ$ = -566.0 kJ/mol

Accepted Answer

A)  -1.0454 * 104 kJ/mol 
B)  -8,756 kJ/mol 
C)  -6,492 kJ/mol 
D)  1.0454 * 104 kJ/mol 
E)  1.1586 * 104 kJ/mol 
A)  -1.0454 * 104 kJ/mol 
B)  -8,756 kJ/mol 
C)  -6,492 kJ/mol 
D)  1.0454 * 104 kJ/mol 
E)  1.1586 * 104 kJ/mol

Question 3

Find $\Delta$H$\circ$rxn for the reaction CH4(g) + 2O2(g) $\rarr$CO2(g) + 2H2O(l).[$\Delta$H$\circ$f (CH4(g)) = -74.8 kJ/mol; $\Delta$H$\circ$f (CO2(g)) = -393.5 kJ/mol; $\Delta$H$\circ$f (H2O(l)) = -285.5 kJ/mol]

Accepted Answer

A)  -879.7 kJ/mol 
B)  -889.7 kJ/mol 
C)  -899.7 kJ/mol 
D)  -909.7 kJ/mol 
E)  None of the above 
A)  -879.7 kJ/mol 
B)  -889.7 kJ/mol 
C)  -899.7 kJ/mol 
D)  -909.7 kJ/mol 
E)  None of the above

Question 4

The enthalpy of combustion of acetylene C2H2 is described by C2H2(g) + (5/2)O2(g) $\rarr$2CO2(g) + H2O(l), $\Delta$H$\circ$rxn= -1299 kJ/mol.Calculate the enthalpy of formation of acetylene, given the following enthalpies of formation
$\Delta$H$\circ$f[CO2(g)] = -393.5 kJ/mol
$\Delta$H$\circ$f[H2O(l)] = -285.8 kJ/mol

Accepted Answer

A)  216 kJ/mol 
B)  226 kJ/mol 
C)  236 kJ/mol 
D)  246 kJ/mol 
E)  None of the above 
A)  216 kJ/mol 
B)  226 kJ/mol 
C)  236 kJ/mol 
D)  246 kJ/mol 
E)  None of the above

Question 5

Thermal energy is 4

Accepted Answer

A)  the energy stored within the structural units of chemical substances. 
B)  the energy associated with the random motion of atoms and molecules. 
C)  solar energy, i.e. energy that comes from the sun. 
D)  energy available by virtue of an object's position. 
A)  the energy stored within the structural units of chemical substances. 
B)  the energy associated with the random motion of atoms and molecules. 
C)  solar energy, i.e. energy that comes from the sun. 
D)  energy available by virtue of an object's position.

Question 6

Calcium oxide and water react in an exothermic reaction: CaO(s) + H2O(l) $\rarr$ Ca(OH)2(s), $\Delta$H$\circ$rxn = -64.8 kJ/mol.How much heat would be liberated when 7.15 g CaO(s) is dropped into a beaker containing 152g H2O

Accepted Answer

A)  1.97 * 10-3 kJ 
B)  8.26 kJ 
C)  508 kJ 
D)  547 kJ 
E)  555 kJ 
A)  1.97 * 10-3 kJ 
B)  8.26 kJ 
C)  508 kJ 
D)  547 kJ 
E)  555 kJ

Question 7

The value of $\Delta$H$\circ$rxn for the following reaction is -6535 kJ/mol.2C6H6(l) + 15O2(g) $\rarr$12CO2(g) + 6H2O(g) How many kilojoules of heat will be evolved during the combustion of 16.0 g of C6H6(l)

Accepted Answer

A)  689 kJ 
B)  679 kJ 
C)  669 kJ 
D)  659 kJ 
E)  None of the above 
A)  689 kJ 
B)  679 kJ 
C)  669 kJ 
D)  659 kJ 
E)  None of the above

Question 8

Which of the following processes is exothermic, given the following: N2(g) + 2 O2(g) $\rarr$ N2O4(l) $\Delta$H$\circ$ = 9.67 kJ/mol
N2(g) + 2 O2(g) $\rarr$ 2 NO2(g) $\Delta$H$\circ$ = 67.70 kJ/mol

Accepted Answer

A)  2 N2(g) + 4 O2(g) $\rarr$ 2 N2O4(l) 
B)  ½ N2(g) + O2(g) $\rarr$ ½ N2O4(l) 
C)  N2O4(l) $\rarr$N2(g) + 2 O2(g) 
D)  2 N2(g) + 4 O2(g) $\rarr$ 2 NO2(g) + N2O4(l) 
E)  2 N2(g) + 4 O2(g) $\rarr$ 4 NO2(g) 
A)  2 N2(g) + 4 O2(g) $\rarr$ 2 N2O4(l) 
B)  ½ N2(g) + O2(g) $\rarr$ ½ N2O4(l) 
C)  N2O4(l) $\rarr$N2(g) + 2 O2(g) 
D)  2 N2(g) + 4 O2(g) $\rarr$ 2 NO2(g) + N2O4(l) 
E)  2 N2(g) + 4 O2(g) $\rarr$ 4 NO2(g)

Question 9

If 10.6 moles of water at 35$\circ$C absorbs 12.30 kJ, what is the final temperature of the water The specific heat of water is 4.184 J/g·$\circ$C.

Accepted Answer

A)  15$\circ$C 
B)  20$\circ$C 
C)  35$\circ$C 
D)  50.$\circ$C 
E)  312$\circ$C 
A)  15$\circ$C 
B)  20$\circ$C 
C)  35$\circ$C 
D)  50.$\circ$C 
E)  312$\circ$C

Question 10

Methanol (CH3OH) burns according to the equation 2CH3OH(l) + 3O2(g) $\rarr$ 2CO2(g) + 4H2O(l), $\Delta$H$\circ$rxn = -1454 kJ/mol.How much heat, in kilojoules, is given off when 75.0 g of methanol is burned

Accepted Answer

A)  727 kJ 
B)  3.22 * 103 kJ 
C)  1.45 * 103 kJ 
D)  1.70 * 103 kJ 
E)  3.41 * 103 kJ 
A)  727 kJ 
B)  3.22 * 103 kJ 
C)  1.45 * 103 kJ 
D)  1.70 * 103 kJ 
E)  3.41 * 103 kJ

Question 11

The specific heat of gold is 0.129 J/g·$\circ$C. What is the molar heat capacity of gold

Accepted Answer

A)  0.039 J/mol·$\circ$C 
B)  0.129 J/mol·$\circ$C 
C)  25.4 J/mol·$\circ$C 
D)  39.0 kJ/mol·$\circ$C 
E)  197 J/mol·$\circ$C 
A)  0.039 J/mol·$\circ$C 
B)  0.129 J/mol·$\circ$C 
C)  25.4 J/mol·$\circ$C 
D)  39.0 kJ/mol·$\circ$C 
E)  197 J/mol·$\circ$C

Question 12

How much heat (kJ) is evolved when 4.50 g of Fe2O3 is reacted with excess carbon monoxide using the equation below?
Fe2O3(s) + 3CO(g) $\rarr$ 2 Fe(s) + 3 CO2(g) $\Delta$H$\circ$rxn = - 24.8 kJ/mol,

Accepted Answer

A)  0.699 kJ 
B)  2.10 kJ 
C)  17.9 kJ 
D)  24.8 kJ 
E)  112 kJ 
A)  0.699 kJ 
B)  2.10 kJ 
C)  17.9 kJ 
D)  24.8 kJ 
E)  112 kJ

Question 13

During volcanic eruptions, hydrogen sulfide gas is given off and oxidized by air according to the following chemical equation: 2H2S(g) + 3O2(g) $\rarr$ 2SO2(g) + 2H2O(g)
Calculate the standard enthalpy change for the above reaction given: $\begin{array}{ll}
3 \mathrm{~S}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{~g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})+\mathrm{SO}_{2}(\mathrm{~g}) & \Delta \mathrm{H}^{\circ}=146.9 \mathrm{~kJ} / \mathrm{mol} \
\mathrm{~S}(\mathrm{~s})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{SO}_{2}(\mathrm{~g}) & \Delta \mathrm{H}^{\circ}=-296.4 \mathrm{~kJ} / \mathrm{mol}
\end{array}$

Accepted Answer

A)  -1036.1 kJ/mol 
B)  -742.3 kJ/mol 
C)  -149.5 kJ/mol 
D)  443.3 kJ/mol 
E)  742.3 kJ/mol 
A)  -1036.1 kJ/mol 
B)  -742.3 kJ/mol 
C)  -149.5 kJ/mol 
D)  443.3 kJ/mol 
E)  742.3 kJ/mol

Question 14

At body temperature 2,404 joules of energy are required to evaporate 1.00 g of water. After vigorous exercise, a person feels chilly because the body is giving up heat to evaporate the perspiration. A typical person perspires 25 mL of water after 20. minutes of exercise. How much body heat is this person using to evaporate this water

Accepted Answer

A)  6.0 * 104 J 
B)  6.3 * 104 J 
C)  6.5 * 104 J 
D)  6.7 * 104 J 
E)  None of the above 
A)  6.0 * 104 J 
B)  6.3 * 104 J 
C)  6.5 * 104 J 
D)  6.7 * 104 J 
E)  None of the above

Question 15

The reaction that represents the standard enthalpy of formation for sucrose (C12H22O11) is:

Accepted Answer

A)  C12H22O11(s) + 12 O2 $\rarr$ 12 CO2(g) + 11 H2O(g) 
B)  12 C(diamond) + 11 H2(g) + 11/2 O2(g) $\rarr$ C12H22O11(s) 
C)  12 C(graphite) + 11 H2(g) + 11/2 O2(g) $\rarr$ C12H22O11(s) 
D)  24 C(diamond) + 22 H2(g) + 11 O2(g) $\rarr$ 2 C12H22O11(s) 
E)  C12H22O11(s) $\rarr$ 2 C(graphite) + 11 H2(g) + 11/2 O2(g) 
A)  C12H22O11(s) + 12 O2 $\rarr$ 12 CO2(g) + 11 H2O(g) 
B)  12 C(diamond) + 11 H2(g) + 11/2 O2(g) $\rarr$ C12H22O11(s) 
C)  12 C(graphite) + 11 H2(g) + 11/2 O2(g) $\rarr$ C12H22O11(s) 
D)  24 C(diamond) + 22 H2(g) + 11 O2(g) $\rarr$ 2 C12H22O11(s) 
E)  C12H22O11(s) $\rarr$ 2 C(graphite) + 11 H2(g) + 11/2 O2(g)

Question 16

A 100. mL sample of 0.200 M aqueous hydrochloric acid is added to 100. mL of 0.200 M aqueous ammonia in a calorimeter whose heat capacity (excluding any water) is 480. J/K. The following reaction occurs when the two solutions are mixed.HCl(aq) + NH3(aq) $\rarr$NH4Cl(aq) The temperature increase is 2.34$\circ$C. Calculate $\Delta$H per mole of HCl and NH3 reacted.

Accepted Answer

A)  -154 kJ/mol 
B)  -1.96 kJ/mol 
C)  1.96 kJ/mol 
D)  154 kJ/mol 
E)  485 kJ/mol 
A)  -154 kJ/mol 
B)  -1.96 kJ/mol 
C)  1.96 kJ/mol 
D)  154 kJ/mol 
E)  485 kJ/mol

Question 17

The combustion of butane produces heat according to the equation 2C4H10(g) + 13O2(g) $\rarr$8CO2(g) + 10H2O(l), $\Delta$H$\circ$rxn= -5,314 kJ/mol.How many grams of CO2 are produced per 1.00 * 104 kJ of heat released

Accepted Answer

A)  23.4 g 
B)  44.0 g 
C)  82.3 g 
D)  187 g 
E)  662 g 
A)  23.4 g 
B)  44.0 g 
C)  82.3 g 
D)  187 g 
E)  662 g

Question 18

10.1 g CaO is dropped into a styrofoam coffee cup containing 157 g H2O at 18.0$\circ$C.If the following reaction occurs, what temperature will the water reach, assuming that the cup is a perfect insulator and that the cup absorbs only a negligible amount of heat (The specific heat of water = 4.18 J/g·$\circ$C)
CaO(s) + H2O(l) $\rarr$Ca(OH)2(s) $\Delta$H$\circ$rxn = -64.8 kJ/mol

Accepted Answer

A)  18.02$\circ$C 
B)  35.8$\circ$C 
C)  42.2$\circ$C 
D)  117$\circ$C 
E)  311$\circ$C 
A)  18.02$\circ$C 
B)  35.8$\circ$C 
C)  42.2$\circ$C 
D)  117$\circ$C 
E)  311$\circ$C

Question 19

Heat is

Accepted Answer

A)  a measure of temperature. 
B)  a measure of the change in temperature. 
C)  a measure of thermal energy. 
D)  a measure of thermal energy transferred between two bodies at different temperature. 
A)  a measure of temperature. 
B)  a measure of the change in temperature. 
C)  a measure of thermal energy. 
D)  a measure of thermal energy transferred between two bodies at different temperature.

The specific heat of silver is 0.235 J/g·^$\circ$C. How many joules of heat are required to heat a 75 g silver spoon from 20^$\circ$C to 35^$\circ$C

Calculate the standard enthalpy change for the reaction 2C₈H₁₈(l) + 21O₂(g) $\rarr$ 8CO(g) + 8CO₂(g) + 18H₂O(l).Given: 2C₈H₁₈(l) + 25O₂(g) $\rarr$ 16CO₂(g) + 18H₂O(l) $\Delta$ H^$\circ$ = -11,020 kJ/mol 2CO(g) + O₂(g) $\rarr$ 2CO₂(g) $\Delta$ H^$\circ$ = -566.0 kJ/mol

Find $\Delta$ H^$\circ$_rxn for the reaction CH₄(g) + 2O₂(g) $\rarr$ CO₂(g) + 2H₂O(l).[ $\Delta$ H^$\circ$_f (CH₄(g)) = -74.8 kJ/mol; $\Delta$ H^$\circ$_f (CO₂(g)) = -393.5 kJ/mol; $\Delta$ H^$\circ$_f (H₂O(l)) = -285.5 kJ/mol]

Thermal energy is 4

Calcium oxide and water react in an exothermic reaction: CaO(s) + H₂O(l) $\rarr$ Ca(OH)₂(s), $\Delta$ H^$\circ$_rxn = -64.8 kJ/mol.How much heat would be liberated when 7.15 g CaO(s) is dropped into a beaker containing 152g H₂O

The value of $\Delta$ H^$\circ$_rxn for the following reaction is -6535 kJ/mol.2C₆H₆(l) + 15O₂(g) $\rarr$ 12CO₂(g) + 6H₂O(g) How many kilojoules of heat will be evolved during the combustion of 16.0 g of C₆H₆(l)

Which of the following processes is exothermic, given the following: N₂(g) + 2 O₂(g) $\rarr$ N₂O₄(l) $\Delta$ H^$\circ$ = 9.67 kJ/mol N₂(g) + 2 O₂(g) $\rarr$ 2 NO₂(g) $\Delta$ H^$\circ$ = 67.70 kJ/mol

If 10.6 moles of water at 35^$\circ$C absorbs 12.30 kJ, what is the final temperature of the water The specific heat of water is 4.184 J/g·^$\circ$C.

Methanol (CH₃OH) burns according to the equation 2CH₃OH(l) + 3O₂(g) $\rarr$ 2CO₂(g) + 4H₂O(l), $\Delta$ H^$\circ$_rxn = -1454 kJ/mol.How much heat, in kilojoules, is given off when 75.0 g of methanol is burned

The specific heat of gold is 0.129 J/g·^$\circ$C. What is the molar heat capacity of gold

How much heat (kJ) is evolved when 4.50 g of Fe₂O₃ is reacted with excess carbon monoxide using the equation below? Fe₂O₃(s) + 3CO(g) $\rarr$ 2 Fe(s) + 3 CO₂(g) $\Delta$ H^$\circ$_rxn = - 24.8 kJ/mol,

The reaction that represents the standard enthalpy of formation for sucrose (C₁₂H₂₂O₁₁) is:

The combustion of butane produces heat according to the equation 2C₄H₁₀(g) + 13O₂(g) $\rarr$ 8CO₂(g) + 10H₂O(l), $\Delta$ H^$\circ$_rxn= -5,314 kJ/mol.How many grams of CO₂ are produced per 1.00 * 10⁴ kJ of heat released

Heat is

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

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Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

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Exam 6: Thermochemistry

The specific heat of silver is 0.235 J/g· ∘\circ∘ C. How many joules of heat are required to heat a 75 g silver spoon from 20 ∘\circ∘ C to 35 ∘\circ∘ C

Calculate the standard enthalpy change for the reaction 2C8H18(l) + 21O2(g) →\rarr→ 8CO(g) + 8CO2(g) + 18H2O(l).Given: 2C8H18(l) + 25O2(g) →\rarr→ 16CO2(g) + 18H2O(l) Δ\DeltaΔ H ∘\circ∘ = -11,020 kJ/mol 2CO(g) + O2(g) →\rarr→ 2CO2(g) Δ\DeltaΔ H ∘\circ∘ = -566.0 kJ/mol

Find Δ\DeltaΔ H ∘\circ∘ rxn for the reaction CH4(g) + 2O2(g) →\rarr→ CO2(g) + 2H2O(l).[ Δ\DeltaΔ H ∘\circ∘ f (CH4(g)) = -74.8 kJ/mol; Δ\DeltaΔ H ∘\circ∘ f (CO2(g)) = -393.5 kJ/mol; Δ\DeltaΔ H ∘\circ∘ f (H2O(l)) = -285.5 kJ/mol]

Thermal energy is 4

Calcium oxide and water react in an exothermic reaction: CaO(s) + H2O(l) →\rarr→ Ca(OH)2(s), Δ\DeltaΔ H ∘\circ∘ rxn = -64.8 kJ/mol.How much heat would be liberated when 7.15 g CaO(s) is dropped into a beaker containing 152g H2O

The value of Δ\DeltaΔ H ∘\circ∘ rxn for the following reaction is -6535 kJ/mol.2C6H6(l) + 15O2(g) →\rarr→ 12CO2(g) + 6H2O(g) How many kilojoules of heat will be evolved during the combustion of 16.0 g of C6H6(l)

Which of the following processes is exothermic, given the following: N2(g) + 2 O2(g) →\rarr→ N2O4(l) Δ\DeltaΔ H ∘\circ∘ = 9.67 kJ/mol N2(g) + 2 O2(g) →\rarr→ 2 NO2(g) Δ\DeltaΔ H ∘\circ∘ = 67.70 kJ/mol

If 10.6 moles of water at 35 ∘\circ∘ C absorbs 12.30 kJ, what is the final temperature of the water The specific heat of water is 4.184 J/g· ∘\circ∘ C.

Methanol (CH3OH) burns according to the equation 2CH3OH(l) + 3O2(g) →\rarr→ 2CO2(g) + 4H2O(l), Δ\DeltaΔ H ∘\circ∘ rxn = -1454 kJ/mol.How much heat, in kilojoules, is given off when 75.0 g of methanol is burned

The specific heat of gold is 0.129 J/g· ∘\circ∘ C. What is the molar heat capacity of gold

How much heat (kJ) is evolved when 4.50 g of Fe2O3 is reacted with excess carbon monoxide using the equation below? Fe2O3(s) + 3CO(g) →\rarr→ 2 Fe(s) + 3 CO2(g) Δ\DeltaΔ H ∘\circ∘ rxn = - 24.8 kJ/mol,

The reaction that represents the standard enthalpy of formation for sucrose (C12H22O11) is:

The combustion of butane produces heat according to the equation 2C4H10(g) + 13O2(g) →\rarr→ 8CO2(g) + 10H2O(l), Δ\DeltaΔ H ∘\circ∘ rxn= -5,314 kJ/mol.How many grams of CO2 are produced per 1.00 * 104 kJ of heat released

Heat is

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

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The specific heat of silver is 0.235 J/g·^$\circ$C. How many joules of heat are required to heat a 75 g silver spoon from 20^$\circ$C to 35^$\circ$C

Calculate the standard enthalpy change for the reaction 2C₈H₁₈(l) + 21O₂(g) $\rarr$ 8CO(g) + 8CO₂(g) + 18H₂O(l).Given: 2C₈H₁₈(l) + 25O₂(g) $\rarr$ 16CO₂(g) + 18H₂O(l) $\Delta$ H^$\circ$ = -11,020 kJ/mol 2CO(g) + O₂(g) $\rarr$ 2CO₂(g) $\Delta$ H^$\circ$ = -566.0 kJ/mol

Find $\Delta$ H^$\circ$_rxn for the reaction CH₄(g) + 2O₂(g) $\rarr$ CO₂(g) + 2H₂O(l).[ $\Delta$ H^$\circ$_f (CH₄(g)) = -74.8 kJ/mol; $\Delta$ H^$\circ$_f (CO₂(g)) = -393.5 kJ/mol; $\Delta$ H^$\circ$_f (H₂O(l)) = -285.5 kJ/mol]

Calcium oxide and water react in an exothermic reaction: CaO(s) + H₂O(l) $\rarr$ Ca(OH)₂(s), $\Delta$ H^$\circ$_rxn = -64.8 kJ/mol.How much heat would be liberated when 7.15 g CaO(s) is dropped into a beaker containing 152g H₂O

The value of $\Delta$ H^$\circ$_rxn for the following reaction is -6535 kJ/mol.2C₆H₆(l) + 15O₂(g) $\rarr$ 12CO₂(g) + 6H₂O(g) How many kilojoules of heat will be evolved during the combustion of 16.0 g of C₆H₆(l)

Which of the following processes is exothermic, given the following: N₂(g) + 2 O₂(g) $\rarr$ N₂O₄(l) $\Delta$ H^$\circ$ = 9.67 kJ/mol N₂(g) + 2 O₂(g) $\rarr$ 2 NO₂(g) $\Delta$ H^$\circ$ = 67.70 kJ/mol

If 10.6 moles of water at 35^$\circ$C absorbs 12.30 kJ, what is the final temperature of the water The specific heat of water is 4.184 J/g·^$\circ$C.

Methanol (CH₃OH) burns according to the equation 2CH₃OH(l) + 3O₂(g) $\rarr$ 2CO₂(g) + 4H₂O(l), $\Delta$ H^$\circ$_rxn = -1454 kJ/mol.How much heat, in kilojoules, is given off when 75.0 g of methanol is burned

The specific heat of gold is 0.129 J/g·^$\circ$C. What is the molar heat capacity of gold

How much heat (kJ) is evolved when 4.50 g of Fe₂O₃ is reacted with excess carbon monoxide using the equation below? Fe₂O₃(s) + 3CO(g) $\rarr$ 2 Fe(s) + 3 CO₂(g) $\Delta$ H^$\circ$_rxn = - 24.8 kJ/mol,

The reaction that represents the standard enthalpy of formation for sucrose (C₁₂H₂₂O₁₁) is:

The combustion of butane produces heat according to the equation 2C₄H₁₀(g) + 13O₂(g) $\rarr$ 8CO₂(g) + 10H₂O(l), $\Delta$ H^$\circ$_rxn= -5,314 kJ/mol.How many grams of CO₂ are produced per 1.00 * 10⁴ kJ of heat released