Question 1

A 22.0 g block of copper at 45$\circ$C absorbs 2.50 kJ of heat. Given the specific heat of Cu is 0.385 J/g·$\circ$C what will be the final temperature of the Cu

Accepted Answer

A)  45$\circ$C 
B)  340.$\circ$C 
C)  295$\circ$C 
D)  30.$\circ$C 
E)  250.$\circ$C 
A)  45$\circ$C 
B)  340.$\circ$C 
C)  295$\circ$C 
D)  30.$\circ$C 
E)  250.$\circ$C

Question 2

The heat released when one mole of water is formed from the elements is 1,198 kJ. An experiment was conducted that permitted water to form in this manner, and the heat was contained in 2.0 liters of water. The water temperature before the reaction was 34.5$\circ$C, and after the reaction it had risen to 52.0$\circ$C. How many moles of water were formed (The specific heat of water is 4.184 J/g·$\circ$C.)

Accepted Answer

A)  0.42 mole 
B)  0.32 mole 
C)  0.22 mole 
D)  0.12 mole 
E)  None of the above 
A)  0.42 mole 
B)  0.32 mole 
C)  0.22 mole 
D)  0.12 mole 
E)  None of the above

Question 3

The heat absorbed by a system at constant pressure is equal to DE - PDV.

Accepted Answer

A) True 
 B)False

Question 4

Calculate the amount of heat necessary to raise the temperature of 135.0 g of water from 50.4$\circ$F to 85.0$\circ$F. The specific heat of water = 4.184 J/g·$\circ$C.

Accepted Answer

A)  1.1 kJ 
B)  10.9 kJ 
C)  16.6 kJ 
D)  19.5 kJ 
E)  48.0 kJ 
A)  1.1 kJ 
B)  10.9 kJ 
C)  16.6 kJ 
D)  19.5 kJ 
E)  48.0 kJ

Question 5

How much heat is required to raise the temperature of 1.5 x 103 g of water from 45$\circ$F to 130.$\circ$F The specific heat of water is 4.184 J/g·$\circ$C.

Accepted Answer

A)  3.0 x 101 kJ 
B)  3.0 x 102 kJ 
C)  3.4 x 102 kJ 
D)  5.3 x 102 kJ 
E)  8.2 x 102 kJ 
A)  3.0 x 101 kJ 
B)  3.0 x 102 kJ 
C)  3.4 x 102 kJ 
D)  5.3 x 102 kJ 
E)  8.2 x 102 kJ

Question 6

Determine the heat given off to the surroundings when 9.0 g of aluminum reacts according to the equation 2Al + Fe2O3 $\rarr$Al2O3 + 2Fe, $\Delta$H$\circ$rxn= -849 kJ/mol.

Accepted Answer

A)  1.4 * 102 kJ 
B)  2.8 * 102 kJ 
C)  5.6 * 102 kJ 
D)  2.5 * 103 kJ 
E)  7.6 * 103 kJ 
A)  1.4 * 102 kJ 
B)  2.8 * 102 kJ 
C)  5.6 * 102 kJ 
D)  2.5 * 103 kJ 
E)  7.6 * 103 kJ

Question 7

Concerning the reaction $\mathrm{C} \text { (graphite) }+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=-393 \mathrm{~kJ} / \mathrm{mol}$ how many grams of C(graphite) must be burned to release 275 kJ of heat

Accepted Answer

A)  0.70 g 
B)  8.40 g 
C)  12.0 g 
D)  17.1 g 
E)  22.3 g 
A)  0.70 g 
B)  8.40 g 
C)  12.0 g 
D)  17.1 g 
E)  22.3 g

Question 8

An endothermic reaction causes the surroundings to

Accepted Answer

A)  warm up. 
B)  decrease in temperature. 
C)  become acidic. 
D)  release CO2. 
E)  condense. 
A)  warm up. 
B)  decrease in temperature. 
C)  become acidic. 
D)  release CO2. 
E)  condense.

Question 9

How many grams of ethylene (C2H4) would have to be burned to produce 450 kJ of heat
C2H4(g) + 3O2(g) $\rarr$ 2CO2(g) + H2O(l) $\Delta$H$\circ$rxn = -1411 kJ/mol

Accepted Answer

A)  5.95 g 
B)  695 g 
C)  7.95 g 
D)  8.95 g 
E)  None of the above 
A)  5.95 g 
B)  695 g 
C)  7.95 g 
D)  8.95 g 
E)  None of the above

Question 10

Butane (C4H10) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given $\Delta$H$\circ$f[C4H10(g)] = -124.7 kJ/mol, $\Delta$H$\circ$f[CO2(g)] = -393.5 kJ/mol, $\Delta$H$\circ$f[H2O(g)] = -241.8 kJ/mol, how much energy is released (kJ) when 8.30 g of butane is burned

Accepted Answer

A)  22,100 kJ 
B)  2,658.3 kJ 
C)  379 kJ 
D)  759 kJ 
E)  2,910 kJ 
A)  22,100 kJ 
B)  2,658.3 kJ 
C)  379 kJ 
D)  759 kJ 
E)  2,910 kJ

Question 11

Which of the following processes always results in an increase in the energy of a system

Accepted Answer

A)  The system loses heat and does work on the surroundings. 
B)  The system gains heat and does work on the surroundings. 
C)  The system loses heat and has work done on it by the surroundings. 
D)  The system gains heat and has work done on it by the surroundings. 
E)  None of these is always true. 
A)  The system loses heat and does work on the surroundings. 
B)  The system gains heat and does work on the surroundings. 
C)  The system loses heat and has work done on it by the surroundings. 
D)  The system gains heat and has work done on it by the surroundings. 
E)  None of these is always true.

Question 12

Aluminum metal has a specific heat of 0.900 J/g·$\circ$C. Calculate the amount of heat required to raise the temperature of 10.5 moles of Al from 30.5 $\circ$C to 225$\circ$C.

Accepted Answer

A)  1.84 kJ 
B)  2.41 kJ 
C)  65.1 kJ 
D)  49.6 kJ 
E)  57.3 kJ 
A)  1.84 kJ 
B)  2.41 kJ 
C)  65.1 kJ 
D)  49.6 kJ 
E)  57.3 kJ

Question 13

Suppose a 50.0 g block of silver (specific heat = 0.2350 J/g·$\circ$C) at 100$\circ$C is placed in contact with a 50.0 g block of iron (specific heat = 0.4494 J/g·$\circ$C) at 0$\circ$C, and the two blocks are insulated from the rest of the universe. The final temperature of the two blocks

Accepted Answer

A)  will be higher than 50$\circ$C. 
B)  will be lower than 50$\circ$C. 
C)  will be exactly 50$\circ$C. 
D)  is unrelated to the composition of the blocks. 
E)  cannot be predicted. 
A)  will be higher than 50$\circ$C. 
B)  will be lower than 50$\circ$C. 
C)  will be exactly 50$\circ$C. 
D)  is unrelated to the composition of the blocks. 
E)  cannot be predicted.

Question 14

Given the specific heat for aluminum is 0.900 J/g·$\circ$C, how much heat is released when a 3.8 g sample of Al cools from 450.0$\circ$C to 25$\circ$C

Accepted Answer

A)  54 J 
B)  60 J 
C)  86 J 
D)  1.5 kJ 
E)  1.7 kJ 
A)  54 J 
B)  60 J 
C)  86 J 
D)  1.5 kJ 
E)  1.7 kJ

Question 15

The reaction that represents the standard enthalpy of formation for acetone (CH3COCH3), a common ingredient in nail polish remover is:

Accepted Answer

A)  3 C(graphite) + 3 H2(g) + ½ O2(g) $\rarr$ CH3COCH3(l) 
B)  6 C(diamond) + 6 H2(g) + O2(g) $\rarr$ 2 CH3COCH3(l) 
C)  3 C(diamond) + 3 H2(g) + ½ O2(g) $\rarr$ CH3COCH3(l) 
D)  CH3COCH3(l) $\rarr$ 3 C(graphite) + 3 H2(g) + ½ O2(g) 
E)  CH3COCH3(l) + 4 O2(g) $\rarr$ 3 CO2(g) + 3 H2O(g) 
A)  3 C(graphite) + 3 H2(g) + ½ O2(g) $\rarr$ CH3COCH3(l) 
B)  6 C(diamond) + 6 H2(g) + O2(g) $\rarr$ 2 CH3COCH3(l) 
C)  3 C(diamond) + 3 H2(g) + ½ O2(g) $\rarr$ CH3COCH3(l) 
D)  CH3COCH3(l) $\rarr$ 3 C(graphite) + 3 H2(g) + ½ O2(g) 
E)  CH3COCH3(l) + 4 O2(g) $\rarr$ 3 CO2(g) + 3 H2O(g)

Question 16

Radiant energy is

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 17

The heat of neutralization of HCl by NaOH is $\Delta$H$\circ$rxn = -56.2 kJ/mol. How much heat is released when 125 mL of 1.750 M HCl is mixed with 195 mL of 0.667 M NaOH

Accepted Answer

A)  7.11 kJ 
B)  7.21 kJ 
C)  7.31 kJ 
D)  7.41 kJ 
E)  None of the above 
A)  7.11 kJ 
B)  7.21 kJ 
C)  7.31 kJ 
D)  7.41 kJ 
E)  None of the above

Question 18

An exothermic reaction causes the surroundings to

Accepted Answer

A)  increase in temperature 
B)  decrease in temperature. 
C)  become acidic. 
D)  release CO2. 
E)  expand. 
A)  increase in temperature 
B)  decrease in temperature. 
C)  become acidic. 
D)  release CO2. 
E)  expand.

Question 19

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 butane must be burned to release 1.00 * 104 kJ of heat

Accepted Answer

A)  30.9 g 
B)  61.8 g 
C)  109 g 
D)  153 g 
E)  219 g 
A)  30.9 g 
B)  61.8 g 
C)  109 g 
D)  153 g 
E)  219 g

Question 20

Octane (C8H18) undergoes combustion according to the following thermochemical equation: 2C8H18(l) + 25O2(g) $\rarr$ 16CO2(g) + 18H2O(l), $\Delta$H$\circ$rxn = -11,020 kJ/mol.Given that $\Delta$H$\circ$f[CO2(g)] = -393.5 kJ/mol and $\Delta$H$\circ$f[H2O(l)] = -285.8 kJ/mol, calculate the standard enthalpy of formation of octane.

Accepted Answer

A)  -210 kJ/mol 
B)  -11,230 kJ/mol 
C)  22,040 kJ/mol 
D)  -420 kJ/mol 
E)  420 kJ/mol 
A)  -210 kJ/mol 
B)  -11,230 kJ/mol 
C)  22,040 kJ/mol 
D)  -420 kJ/mol 
E)  420 kJ/mol

Exam 6: Thermochemistry

A 22.0 g block of copper at 45 ∘\circ∘ C absorbs 2.50 kJ of heat. Given the specific heat of Cu is 0.385 J/g· ∘\circ∘ C what will be the final temperature of the Cu

The heat absorbed by a system at constant pressure is equal to DE - PDV.

Calculate the amount of heat necessary to raise the temperature of 135.0 g of water from 50.4 ∘\circ∘ F to 85.0 ∘\circ∘ F. The specific heat of water = 4.184 J/g· ∘\circ∘ C.

How much heat is required to raise the temperature of 1.5 x 103 g of water from 45 ∘\circ∘ F to 130. ∘\circ∘ F The specific heat of water is 4.184 J/g· ∘\circ∘ C.

Determine the heat given off to the surroundings when 9.0 g of aluminum reacts according to the equation 2Al + Fe2O3 →\rarr→ Al2O3 + 2Fe, Δ\DeltaΔ H ∘\circ∘ rxn= -849 kJ/mol.

An endothermic reaction causes the surroundings to

How many grams of ethylene (C2H4) would have to be burned to produce 450 kJ of heat C2H4(g) + 3O2(g) →\rarr→ 2CO2(g) + H2O(l) Δ\DeltaΔ H ∘\circ∘ rxn = -1411 kJ/mol

Which of the following processes always results in an increase in the energy of a system

Aluminum metal has a specific heat of 0.900 J/g· ∘\circ∘ C. Calculate the amount of heat required to raise the temperature of 10.5 moles of Al from 30.5 ∘\circ∘ C to 225 ∘\circ∘ C.

Given the specific heat for aluminum is 0.900 J/g· ∘\circ∘ C, how much heat is released when a 3.8 g sample of Al cools from 450.0 ∘\circ∘ C to 25 ∘\circ∘ C

The reaction that represents the standard enthalpy of formation for acetone (CH3COCH3), a common ingredient in nail polish remover is:

Radiant energy is

The heat of neutralization of HCl by NaOH is Δ\DeltaΔ H ∘\circ∘ rxn = -56.2 kJ/mol. How much heat is released when 125 mL of 1.750 M HCl is mixed with 195 mL of 0.667 M NaOH

An exothermic reaction causes the surroundings to

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 butane must be burned to release 1.00 * 104 kJ of heat

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A 22.0 g block of copper at 45^$\circ$C absorbs 2.50 kJ of heat. Given the specific heat of Cu is 0.385 J/g·^$\circ$C what will be the final temperature of the Cu

Calculate the amount of heat necessary to raise the temperature of 135.0 g of water from 50.4^$\circ$F to 85.0^$\circ$F. The specific heat of water = 4.184 J/g·^$\circ$C.

How much heat is required to raise the temperature of 1.5 x 10³ g of water from 45^$\circ$F to 130.^$\circ$F The specific heat of water is 4.184 J/g·^$\circ$C.

Determine the heat given off to the surroundings when 9.0 g of aluminum reacts according to the equation 2Al + Fe₂O₃ $\rarr$ Al₂O₃ + 2Fe, $\Delta$ H^$\circ$_rxn= -849 kJ/mol.

How many grams of ethylene (C₂H₄) would have to be burned to produce 450 kJ of heat C₂H₄(g) + 3O₂(g) $\rarr$ 2CO₂(g) + H₂O(l) $\Delta$ H^$\circ$_rxn = -1411 kJ/mol

Aluminum metal has a specific heat of 0.900 J/g·^$\circ$C. Calculate the amount of heat required to raise the temperature of 10.5 moles of Al from 30.5 ^$\circ$C to 225^$\circ$C.

Given the specific heat for aluminum is 0.900 J/g·^$\circ$C, how much heat is released when a 3.8 g sample of Al cools from 450.0^$\circ$C to 25^$\circ$C

The reaction that represents the standard enthalpy of formation for acetone (CH₃COCH₃), a common ingredient in nail polish remover is:

The heat of neutralization of HCl by NaOH is $\Delta$ H^$\circ$_rxn = -56.2 kJ/mol. How much heat is released when 125 mL of 1.750 M HCl is mixed with 195 mL of 0.667 M NaOH

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 butane must be burned to release 1.00 * 10⁴ kJ of heat