Grade 11 : Chemistry - Thermodynamics (Set 4)

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Grade 11 : Chemistry - Thermodynamics (Set 4)— Questions & Detailed Solutions

A sample of ideal gas in a cylinder fitted with a frictionless piston expands from 2.0 L to 6.0 L against a constant external pressure of 2.0 atm. During this expansion, the gas absorbs 500 J of heat from the surroundings. ($1\text{ L}\cdot\text{atm} = 101.3\text{ J}$).
What is the change in internal energy ($\Delta U$) of the gas system?

(A)

+310.4 J

(B)

-310.4 J

(C)

-1310.4 J

(D)

+1310.4 J

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:Work done $w = -P_{ext}\Delta V = -2.0 \times (6.0 - 2.0) = -8.0\text{ L}\cdot\text{atm}$. Converting work to Joules: $w = -8.0 \times 101.3 = -810.4\text{ J}$. By the First Law of Thermodynamics: $\Delta U = q + w = +500\text{ J} + (-810.4\text{ J}) = -310.4\text{ J}$.

Consider the gaseous reaction: $\text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g)$ occurring at 298 K. The internal energy change for the reaction is $\Delta U = -88.0\text{ kJ}$. ($R = 8.314\text{ J K}^{-1}\text{ mol}^{-1}$).
Calculate the enthalpy change ($\Delta H$) for the reaction under standard conditions.

(A)

-92.95 kJ

(B)

-83.05 kJ

(C)

+92.95 kJ

(D)

-88.00 kJ

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:$\Delta n_g = 2 - (1 + 3) = -2\text{ mol}$. Using $\Delta H = \Delta U + \Delta n_g RT$: $\Delta H = -88.0\text{ kJ} + (-2 \times 8.314 \times 10^{-3} \times 298)\text{ kJ} = -88.0 - 4.95 = -92.95\text{ kJ}$.

Thermochemical Reaction $\Delta H^\circ\text{ (kJ)}$
(1) $\text{C}(s) + \text{O}_2(g) \rightarrow \text{CO}_2(g)$ -393.5
(2) $\text{CO}(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{CO}_2(g)$ -283.0
Using Hess's Law and the table above, determine $\Delta H^\circ$ for the partial oxidation of carbon: $\text{C}(s) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{CO}(g)$.

Thermochemical Reaction	$\Delta H^\circ\text{ (kJ)}$
(1) $\text{C}(s) + \text{O}_2(g) \rightarrow \text{CO}_2(g)$	-393.5
(2) $\text{CO}(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{CO}_2(g)$	-283.0

(A)

-676.5 kJ

(B)

+110.5 kJ

(C)

-110.5 kJ

(D)

-283.0 kJ

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:Subtract reaction (2) from reaction (1): $\text{C}(s) + \text{O}_2(g) - [\text{CO}(g) + \frac{1}{2}\text{O}_2(g)] \rightarrow \text{CO}_2(g) - \text{CO}_2(g)$, which gives $\text{C}(s) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{CO}(g)$. Thus, $\Delta H^\circ = -393.5 - (-283.0) = -110.5\text{ kJ}$.

A 0.50 g sample of benzoic acid is combusted in a bomb calorimeter with a total heat capacity of 2.50 kJ/K. The observed temperature rise is 5.00 K. The molar mass of benzoic acid is 122 g/mol.
Calculate the molar internal energy of combustion ($\Delta U_{comb}$) for benzoic acid.

(A)

-3050 kJ/mol

(B)

-1525 kJ/mol

(C)

-6100 kJ/mol

(D)

+3050 kJ/mol

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:Heat released $q = C \Delta T = 2.50\text{ kJ/K} \times 5.00\text{ K} = 12.5\text{ kJ}$. Moles of benzoic acid $n = \frac{0.50g}{122\text{ g/mol}} = 0.004098\text{ mol}$. $\Delta U_{comb} = -\frac{12.5\text{ kJ}}{0.004098\text{ mol}} \approx -3050\text{ kJ/mol}$.

A 2.0 mol sample of an ideal gas expands isothermally and reversibly from an initial volume of 10.0 L to a final volume of 100.0 L at 300 K. ($R = 8.314\text{ J K}^{-1}\text{ mol}^{-1}$, $\ln(10) = 2.303$).
What is the total work done ($w$) by the gas during this process?

(A)

+11.49 kJ

(B)

-11.49 kJ

(C)

-5.74 kJ

(D)

-22.98 kJ

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:For isothermal reversible expansion: $w = -2.303 n R T \log_{10}(V_2/V_1) = -2.303 \times 2.0 \times 8.314 \times 300 \times \log_{10}(100/10) = -11488\text{ J} = -11.49\text{ kJ}$.

A certain chemical reaction has an enthalpy change $\Delta H = -40.0\text{ kJ/mol}$ and an entropy change $\Delta S = -100.0\text{ J K}^{-1}\text{ mol}^{-1}$.
At what temperature range will this reaction be spontaneous under standard conditions?

(A)

$T > 400\text{ K}$

(B)

$T < 400\text{ K}$

(C)

Spontaneous at all temperatures

(D)

Non-spontaneous at all temperatures

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:For spontaneity, $\Delta G = \Delta H - T\Delta S < 0$. $-40000\text{ J} - T(-100.0\text{ J/K}) < 0 \implies 100 T < 40000 \implies T < 400\text{ K}$. Thus, the reaction is spontaneous at temperatures below 400 K.

The molar heat of vaporization of liquid water at its boiling point ($100^\circ\text{C}$ / 373 K) is 40.66 kJ/mol.
Calculate the standard molar entropy of vaporization ($\Delta S_{vap}$) of water.

(A)

$+109.0\text{ J K}^{-1}\text{ mol}^{-1}$

(B)

$-109.0\text{ J K}^{-1}\text{ mol}^{-1}$

(C)

$+40.66\text{ J K}^{-1}\text{ mol}^{-1}$

(D)

$+0.109\text{ J K}^{-1}\text{ mol}^{-1}$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:At phase transition equilibrium, $\Delta S_{vap} = \frac{\Delta H_{vap}}{T_{b}} = \frac{40660\text{ J/mol}}{373\text{ K}} = +109.0\text{ J K}^{-1}\text{ mol}^{-1}$.

Chemical Bond Mean Bond Dissociation Enthalpy (kJ/mol)
C-H 414
Cl-Cl 243
C-Cl 330
H-Cl 431
Using the bond enthalpy table above, calculate $\Delta H$ for the chlorination of methane: $\text{CH}_4(g) + \text{Cl}_2(g) \rightarrow \text{CH}_3\text{Cl}(g) + \text{HCl}(g)$.

Chemical Bond	Mean Bond Dissociation Enthalpy (kJ/mol)
C-H	414
Cl-Cl	243
C-Cl	330
H-Cl	431

(A)

+104 kJ/mol

(B)

-104 kJ/mol

(C)

-208 kJ/mol

(D)

+657 kJ/mol

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:$\Delta H = \sum BE(\text{reactants}) - \sum BE(\text{products}) = [4(414) + 243] - [3(414) + 330 + 431] = (414 + 243) - (330 + 431) = 657 - 761 = -104\text{ kJ/mol}$.

Statement I: Internal energy ($U$) and Enthalpy ($H$) are state functions.
Statement II: Heat ($q$) and Work ($w$) are path functions.
Statement III: The sum $(q + w)$ depends on the path taken between states.
Evaluate the statements above and select the correct combination.

(A)

Statements I, II, and III are all correct.

(B)

Statements I and II are correct, but Statement III is incorrect.

(C)

Statements II and III are correct, but Statement I is incorrect.

(D)

Only Statement I is correct.

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:Statements I and II are correct. Statement III is false because $q + w = \Delta U$, which is a state function independent of the path taken.

Q10

A gas undergoes a cyclic process (A -> B -> C -> D -> A):
- Step A -> B: Isobaric expansion at $P = 4.0\text{ atm}$ from $V = 1.0\text{ L}$ to $V = 4.0\text{ L}$.
- Step B -> C: Isochoric cooling at $V = 4.0\text{ L}$ from $P = 4.0\text{ atm}$ to $P = 1.0\text{ atm}$.
- Step C -> D: Isobaric compression at $P = 1.0\text{ atm}$ from $V = 4.0\text{ L}$ to $V = 1.0\text{ L}$.
- Step D -> A: Isochoric heating at $V = 1.0\text{ L}$ back to $P = 4.0\text{ atm}$.
Calculate the net work done by the system per cycle. ($1\text{ L}\cdot\text{atm} = 101.3\text{ J}$).

(A)

-911.7 J

(B)

+911.7 J

(C)

-303.9 J

(D)

0 J

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:Area of the closed cycle = $\Delta P \times \Delta V = (4.0 - 1.0)\text{ atm} \times (4.0 - 1.0)\text{ L} = 9.0\text{ L}\cdot\text{atm}$. Converting to Joules: $9.0 \times 101.3\text{ J} = 911.7\text{ J}$. Since the cycle is clockwise, work is done by system: $w = -911.7\text{ J}$.

Q11

For 1.0 mol of a monoatomic ideal gas, the molar heat capacity at constant volume is $C_v = \frac{3}{2} R$. Using Mayer's relation ($C_p - C_v = R$).
What is the heat capacity ratio $\gamma = \frac{C_p}{C_v}$ for this gas?

(A)

1.40

(B)

1.67

(C)

1.33

(D)

2.50

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:$C_p = C_v + R = \frac{3}{2}R + R = \frac{5}{2}R$. Therefore, $\gamma = \frac{C_p}{C_v} = \frac{\frac{5}{2}R}{\frac{3}{2}R} = \frac{5}{3} \approx 1.67$.

Q12

In a neutralization experiment, 100 mL of 0.5 M HCl is mixed with 100 mL of 0.5 M NaOH in a coffee-cup calorimeter. The standard enthalpy of neutralization for strong acid and strong base is -57.1 kJ/mol.
Calculate the heat released ($q$) during this reaction.

(A)

57.1 kJ

(B)

2.855 kJ

(C)

5.71 kJ

(D)

1.428 kJ

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:Moles of $\text{H}^+$ reacted = $0.100\text{ L} \times 0.5m = 0.05\text{ mol}$. Heat released $q = 0.05\text{ mol} \times 57.1\text{ kJ/mol} = 2.855\text{ kJ}$.

Q13

Which of the following statements correctly expresses the Third Law of Thermodynamics?

(A)

Energy can neither be created nor destroyed in an isolated system.

(B)

The entropy of a perfectly crystalline substance approaches zero as temperature approaches absolute zero (0 K).

(C)

The total entropy of the universe increases in any spontaneous process.

(D)

Heat cannot flow spontaneously from a cooler body to a warmer body.

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✓ Correct Option: (B)

Explanation:The Third Law of Thermodynamics states that the entropy of a pure, perfectly crystalline substance is zero at absolute zero temperature (0 K).

Q14

Substance Standard Enthalpy of Combustion $\Delta H_c^\circ\text{ (kJ/mol)}$
$\text{C}(s)$ -393.5
$\text{H}_2(g)$ -285.8
$\text{CH}_4(g)$ -890.3
Determine the standard enthalpy of formation ($\Delta H_f^\circ$) of methane gas: $\text{C}(s) + 2\text{H}_2(g) \rightarrow \text{CH}_4(g)$.

Substance	Standard Enthalpy of Combustion $\Delta H_c^\circ\text{ (kJ/mol)}$
$\text{C}(s)$	-393.5
$\text{H}_2(g)$	-285.8
$\text{CH}_4(g)$	-890.3

(A)

-74.8 kJ/mol

(B)

+74.8 kJ/mol

(C)

-1569.6 kJ/mol

(D)

-211.0 kJ/mol

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:$\Delta H_f^\circ(\text{CH}_4) = \Delta H_c^\circ(\text{C}) + 2\Delta H_c^\circ(\text{H}_2) - \Delta H_c^\circ(\text{CH}_4) = -393.5 + 2(-285.8) - (-890.3) = -393.5 - 571.6 + 890.3 = -74.8\text{ kJ/mol}$.

Q15

An ideal gas expands adiabatically into an evacuated chamber (free expansion, $P_{ext} = 0$).
What are the values of heat transferred ($q$), work done ($w$), and internal energy change ($\Delta U$) for this process?

(A)

$q = 0, w < 0, \Delta U < 0$

(B)

$q = 0, w = 0, \Delta U = 0$

(C)

$q > 0, w < 0, \Delta U = 0$

(D)

$q = 0, w > 0, \Delta U > 0$

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:For adiabatic process, $q = 0$. For expansion into vacuum, $P_{ext} = 0 \implies w = 0$. By First Law, $\Delta U = q + w = 0 + 0 = 0$.

Q16

Reaction Case Enthalpy Change ($\Delta H$) Entropy Change ($\Delta S$)
Case 1 Negative ($\Delta H < 0$) Positive ($\Delta S > 0$)
Case 2 Positive ($\Delta H > 0$) Negative ($\Delta S < 0$)
Case 3 Positive ($\Delta H > 0$) Positive ($\Delta S > 0$)
Case 4 Negative ($\Delta H < 0$) Negative ($\Delta S < 0$)
Which case represents a reaction that is non-spontaneous at low temperatures but becomes spontaneous ONLY at high temperatures?

Reaction Case	Enthalpy Change ($\Delta H$)	Entropy Change ($\Delta S$)
Case 1	Negative ($\Delta H < 0$)	Positive ($\Delta S > 0$)
Case 2	Positive ($\Delta H > 0$)	Negative ($\Delta S < 0$)
Case 3	Positive ($\Delta H > 0$)	Positive ($\Delta S > 0$)
Case 4	Negative ($\Delta H < 0$)	Negative ($\Delta S < 0$)

(A)

Case 1

(B)

Case 2

(C)

Case 3

(D)

Case 4

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation:$\Delta G = \Delta H - T\Delta S$. For Case 3, both $\Delta H$ and $\Delta S$ are positive. At low temperatures, $T\Delta S < \Delta H$ so $\Delta G > 0$ (non-spontaneous). At high temperatures, $T\Delta S > \Delta H$, making $\Delta G < 0$ (spontaneous).

Q17

A system absorbs 3000 J of heat reversibly from a constant thermal reservoir at 600 K.
What are the entropy changes of the system ($\Delta S_{sys}$) and the reservoir ($\Delta S_{res}$)?

(A)

$\Delta S_{sys} = +5\text{ J/K}, \Delta S_{res} = -5\text{ J/K}$

(B)

$\Delta S_{sys} = -5\text{ J/K}, \Delta S_{res} = +5\text{ J/K}$

(C)

$\Delta S_{sys} = +5\text{ J/K}, \Delta S_{res} = +5\text{ J/K}$

(D)

$\Delta S_{sys} = 0\text{ J/K}, \Delta S_{res} = 0\text{ J/K}$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:$\Delta S_{sys} = +\frac{q_{rev}}{T} = +\frac{3000\text{ J}}{600\text{ K}} = +5\text{ J/K}$. Heat lost by reservoir = -3000 J, so $\Delta S_{res} = -\frac{3000\text{ J}}{600\text{ K}} = -5\text{ J/K}$.

Q18

Thermodynamic Process Step $\Delta H^\circ\text{ (kJ/mol)}$
Sublimation of $\text{Na}(s)$ +108
Dissociation of $\frac{1}{2}\text{Cl}_2(g)$ +121
First Ionization Energy of $\text{Na}(g)$ +496
Electron Gain Enthalpy of $\text{Cl}(g)$ -349
Lattice Enthalpy of $\text{NaCl}(s)$ -788
Calculate the standard enthalpy of formation ($\Delta H_f^\circ$) of $\text{NaCl}(s)$ using the Born-Haber cycle data above.

Thermodynamic Process Step	$\Delta H^\circ\text{ (kJ/mol)}$
Sublimation of $\text{Na}(s)$	+108
Dissociation of $\frac{1}{2}\text{Cl}_2(g)$	+121
First Ionization Energy of $\text{Na}(g)$	+496
Electron Gain Enthalpy of $\text{Cl}(g)$	-349
Lattice Enthalpy of $\text{NaCl}(s)$	-788

(A)

-412 kJ/mol

(B)

+412 kJ/mol

(C)

-788 kJ/mol

(D)

-550 kJ/mol

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:By Born-Haber cycle: $\Delta H_f^\circ = \Delta H_{sub} + \frac{1}{2}\Delta H_{diss} + IE_1 + EA_1 + U_L = 108 + 121 + 496 + (-349) + (-788) = 725 - 1137 = -412\text{ kJ/mol}$.

Q19

Which of the following sets contains ONLY intensive thermodynamic properties?

(A)

Volume ($V$), Enthalpy ($H$), Molar Heat Capacity ($C_m$)

(B)

Temperature ($T$), Density ($d$), Molar Heat Capacity ($C_m$)

(C)

Temperature ($T$), Volume ($V$), Density ($d$)

(D)

Enthalpy ($H$), Density ($d$), Molar Heat Capacity ($C_m$)

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation:Intensive properties are independent of sample size: Temperature ($T$), Density ($d$), and Molar Heat Capacity ($C_m$) are intensive. Volume ($V$) and Enthalpy ($H$) are extensive.

Q20

A 50.0 g sample of a metal heated to $100.0^\circ\text{C}$ is placed into 100.0 g of water initially at $20.0^\circ\text{C}$ inside a insulated calorimeter. The system reaches a final equilibrium temperature of $25.0^\circ\text{C}$. ($c_{water} = 4.184\text{ J g}^{-1}{^\circ\text{C}}^{-1}$).
Calculate the specific heat capacity ($c_{metal}$) of the metal.

(A)

$0.558\text{ J g}^{-1}{^\circ\text{C}}^{-1}$

(B)

$0.279\text{ J g}^{-1}{^\circ\text{C}}^{-1}$

(C)

$1.116\text{ J g}^{-1}{^\circ\text{C}}^{-1}$

(D)

$0.418\text{ J g}^{-1}{^\circ\text{C}}^{-1}$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation:Heat gained by water = $m_w c_w \Delta T_w = 100.0 \times 4.184 \times (25.0 - 20.0) = 2092\text{ J}$. Heat lost by metal = $m_m c_m \Delta T_m = 50.0 \times c_m \times (100.0 - 25.0) = 3750 c_m$. Setting $3750 c_m = 2092 \implies c_m = 0.558\text{ J g}^{-1}{^\circ\text{C}}^{-1}$.

Grade 11 : Chemistry - Thermodynamics (Set 4)

Grade 11 : Chemistry - Thermodynamics (Set 4)— Questions & Detailed Solutions

A 0.50 g sample of benzoic acid is combusted in a bomb calorimeter with a total heat capacity of 2.50 kJ/K. The observed temperature rise is 5.00 K. The molar mass of benzoic acid is 122 g/mol.
Calculate the molar internal energy of combustion ($\Delta U_{comb}$) for benzoic acid.

A 2.0 mol sample of an ideal gas expands isothermally and reversibly from an initial volume of 10.0 L to a final volume of 100.0 L at 300 K. ($R = 8.314\text{ J K}^{-1}\text{ mol}^{-1}$, $\ln(10) = 2.303$).
What is the total work done ($w$) by the gas during this process?

A certain chemical reaction has an enthalpy change $\Delta H = -40.0\text{ kJ/mol}$ and an entropy change $\Delta S = -100.0\text{ J K}^{-1}\text{ mol}^{-1}$.
At what temperature range will this reaction be spontaneous under standard conditions?

The molar heat of vaporization of liquid water at its boiling point ($100^\circ\text{C}$ / 373 K) is 40.66 kJ/mol.
Calculate the standard molar entropy of vaporization ($\Delta S_{vap}$) of water.

Chemical Bond Mean Bond Dissociation Enthalpy (kJ/mol)
C-H 414
Cl-Cl 243
C-Cl 330
H-Cl 431
Using the bond enthalpy table above, calculate $\Delta H$ for the chlorination of methane: $\text{CH}_4(g) + \text{Cl}_2(g) \rightarrow \text{CH}_3\text{Cl}(g) + \text{HCl}(g)$.

Statement I: Internal energy ($U$) and Enthalpy ($H$) are state functions.
Statement II: Heat ($q$) and Work ($w$) are path functions.
Statement III: The sum $(q + w)$ depends on the path taken between states.
Evaluate the statements above and select the correct combination.

For 1.0 mol of a monoatomic ideal gas, the molar heat capacity at constant volume is $C_v = \frac{3}{2} R$. Using Mayer's relation ($C_p - C_v = R$).
What is the heat capacity ratio $\gamma = \frac{C_p}{C_v}$ for this gas?

In a neutralization experiment, 100 mL of 0.5 M HCl is mixed with 100 mL of 0.5 M NaOH in a coffee-cup calorimeter. The standard enthalpy of neutralization for strong acid and strong base is -57.1 kJ/mol.
Calculate the heat released ($q$) during this reaction.

Which of the following statements correctly expresses the Third Law of Thermodynamics?

Substance Standard Enthalpy of Combustion $\Delta H_c^\circ\text{ (kJ/mol)}$
$\text{C}(s)$ -393.5
$\text{H}_2(g)$ -285.8
$\text{CH}_4(g)$ -890.3
Determine the standard enthalpy of formation ($\Delta H_f^\circ$) of methane gas: $\text{C}(s) + 2\text{H}_2(g) \rightarrow \text{CH}_4(g)$.

An ideal gas expands adiabatically into an evacuated chamber (free expansion, $P_{ext} = 0$).
What are the values of heat transferred ($q$), work done ($w$), and internal energy change ($\Delta U$) for this process?

A system absorbs 3000 J of heat reversibly from a constant thermal reservoir at 600 K.
What are the entropy changes of the system ($\Delta S_{sys}$) and the reservoir ($\Delta S_{res}$)?

Which of the following sets contains ONLY intensive thermodynamic properties?

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Grade 11 : Chemistry - Thermodynamics (Set 4)

Grade 11 : Chemistry - Thermodynamics (Set 4)— Questions & Detailed Solutions

A 0.50 g sample of benzoic acid is combusted in a bomb calorimeter with a total heat capacity of 2.50 kJ/K. The observed temperature rise is 5.00 K. The molar mass of benzoic acid is 122 g/mol.Calculate the molar internal energy of combustion ($\Delta U_{comb}$) for benzoic acid.

A 2.0 mol sample of an ideal gas expands isothermally and reversibly from an initial volume of 10.0 L to a final volume of 100.0 L at 300 K. ($R = 8.314\text{ J K}^{-1}\text{ mol}^{-1}$, $\ln(10) = 2.303$).What is the total work done ($w$) by the gas during this process?

A certain chemical reaction has an enthalpy change $\Delta H = -40.0\text{ kJ/mol}$ and an entropy change $\Delta S = -100.0\text{ J K}^{-1}\text{ mol}^{-1}$.At what temperature range will this reaction be spontaneous under standard conditions?

The molar heat of vaporization of liquid water at its boiling point ($100^\circ\text{C}$ / 373 K) is 40.66 kJ/mol.Calculate the standard molar entropy of vaporization ($\Delta S_{vap}$) of water.

Chemical BondMean Bond Dissociation Enthalpy (kJ/mol)C-H414Cl-Cl243C-Cl330H-Cl431Using the bond enthalpy table above, calculate $\Delta H$ for the chlorination of methane: $\text{CH}_4(g) + \text{Cl}_2(g) \rightarrow \text{CH}_3\text{Cl}(g) + \text{HCl}(g)$.

Statement I: Internal energy ($U$) and Enthalpy ($H$) are state functions.Statement II: Heat ($q$) and Work ($w$) are path functions.Statement III: The sum $(q + w)$ depends on the path taken between states.Evaluate the statements above and select the correct combination.

For 1.0 mol of a monoatomic ideal gas, the molar heat capacity at constant volume is $C_v = \frac{3}{2} R$. Using Mayer's relation ($C_p - C_v = R$).What is the heat capacity ratio $\gamma = \frac{C_p}{C_v}$ for this gas?

In a neutralization experiment, 100 mL of 0.5 M HCl is mixed with 100 mL of 0.5 M NaOH in a coffee-cup calorimeter. The standard enthalpy of neutralization for strong acid and strong base is -57.1 kJ/mol.Calculate the heat released ($q$) during this reaction.

Which of the following statements correctly expresses the Third Law of Thermodynamics?

SubstanceStandard Enthalpy of Combustion $\Delta H_c^\circ\text{ (kJ/mol)}$$\text{C}(s)$-393.5$\text{H}_2(g)$-285.8$\text{CH}_4(g)$-890.3Determine the standard enthalpy of formation ($\Delta H_f^\circ$) of methane gas: $\text{C}(s) + 2\text{H}_2(g) \rightarrow \text{CH}_4(g)$.

An ideal gas expands adiabatically into an evacuated chamber (free expansion, $P_{ext} = 0$).What are the values of heat transferred ($q$), work done ($w$), and internal energy change ($\Delta U$) for this process?

A system absorbs 3000 J of heat reversibly from a constant thermal reservoir at 600 K.What are the entropy changes of the system ($\Delta S_{sys}$) and the reservoir ($\Delta S_{res}$)?

Which of the following sets contains ONLY intensive thermodynamic properties?

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A 0.50 g sample of benzoic acid is combusted in a bomb calorimeter with a total heat capacity of 2.50 kJ/K. The observed temperature rise is 5.00 K. The molar mass of benzoic acid is 122 g/mol.
Calculate the molar internal energy of combustion ($\Delta U_{comb}$) for benzoic acid.

A 2.0 mol sample of an ideal gas expands isothermally and reversibly from an initial volume of 10.0 L to a final volume of 100.0 L at 300 K. ($R = 8.314\text{ J K}^{-1}\text{ mol}^{-1}$, $\ln(10) = 2.303$).
What is the total work done ($w$) by the gas during this process?

A certain chemical reaction has an enthalpy change $\Delta H = -40.0\text{ kJ/mol}$ and an entropy change $\Delta S = -100.0\text{ J K}^{-1}\text{ mol}^{-1}$.
At what temperature range will this reaction be spontaneous under standard conditions?

The molar heat of vaporization of liquid water at its boiling point ($100^\circ\text{C}$ / 373 K) is 40.66 kJ/mol.
Calculate the standard molar entropy of vaporization ($\Delta S_{vap}$) of water.

Chemical Bond Mean Bond Dissociation Enthalpy (kJ/mol)
C-H 414
Cl-Cl 243
C-Cl 330
H-Cl 431
Using the bond enthalpy table above, calculate $\Delta H$ for the chlorination of methane: $\text{CH}_4(g) + \text{Cl}_2(g) \rightarrow \text{CH}_3\text{Cl}(g) + \text{HCl}(g)$.

Statement I: Internal energy ($U$) and Enthalpy ($H$) are state functions.
Statement II: Heat ($q$) and Work ($w$) are path functions.
Statement III: The sum $(q + w)$ depends on the path taken between states.
Evaluate the statements above and select the correct combination.

For 1.0 mol of a monoatomic ideal gas, the molar heat capacity at constant volume is $C_v = \frac{3}{2} R$. Using Mayer's relation ($C_p - C_v = R$).
What is the heat capacity ratio $\gamma = \frac{C_p}{C_v}$ for this gas?

In a neutralization experiment, 100 mL of 0.5 M HCl is mixed with 100 mL of 0.5 M NaOH in a coffee-cup calorimeter. The standard enthalpy of neutralization for strong acid and strong base is -57.1 kJ/mol.
Calculate the heat released ($q$) during this reaction.

Substance Standard Enthalpy of Combustion $\Delta H_c^\circ\text{ (kJ/mol)}$
$\text{C}(s)$ -393.5
$\text{H}_2(g)$ -285.8
$\text{CH}_4(g)$ -890.3
Determine the standard enthalpy of formation ($\Delta H_f^\circ$) of methane gas: $\text{C}(s) + 2\text{H}_2(g) \rightarrow \text{CH}_4(g)$.

An ideal gas expands adiabatically into an evacuated chamber (free expansion, $P_{ext} = 0$).
What are the values of heat transferred ($q$), work done ($w$), and internal energy change ($\Delta U$) for this process?

A system absorbs 3000 J of heat reversibly from a constant thermal reservoir at 600 K.
What are the entropy changes of the system ($\Delta S_{sys}$) and the reservoir ($\Delta S_{res}$)?