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Calculate the heat of combustion $(kJ)$ of propane, $C_{3} H_{8}$ using the listed standard enthalpy of reaction data:

$C_{3} H_{8} (g) + 5 O_{2} (g) \to 3 {CO}_{2} (g) + 4 H_{2} O (g)$

$3 C (s) + 4 H_{2} (g) \to C_{3} H_{8} (g)$ $∆ H ° / KJ = - 103.8$

$C (s) + O_{2} (g) \to {CO}_{2} (g)$ $∆ H ° / KJ = - 393.5$

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (g)$ $∆ H ° / KJ = - 241.8$

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Important Questions on Thermodynamics

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JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 21

Calculate the value of $∆ H ° / kJ$ for the following reaction using the listed thermochemical equations:

$2 C (s) + H_{2} (g) \to C_{2} H_{2} (g)$

$2 C_{2} H_{2} (g) + 5 O_{2} (g) \to 4 {CO}_{2} (g) + 2 H_{2} O (l)$ $∆ H ° / kJ = - 2600 kJ$

$C (s) + O_{2} (g) \to {CO}_{2} (g)$ $∆ H ° / kJ = - 390 kJ$

$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$ $∆ H ° / kJ = - 572 kJ$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 22

Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

$C_{2} H_{5} OH (l) + 3 O_{2} (g) \to 2 {CO}_{2} (g) + 3 H_{2} O (g)$

$∆ H_{f}^{°} C_{2} H_{5} OH (l) = - 277.7 kJ / mole$

$∆ H_{f}^{°} {CO}_{2} (g) = - 393.5 kJ / mol$

$∆ H_{f}^{°} H_{2} O (g) = - 241.8 kJ / mole$

MEDIUM

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 23

Calculate $∆ H ° / kJ$ for the following reaction using the listed standard enthalpy of reaction data:

$2 N_{2} (g) + 5 O_{2} (g) \to 2 N_{2} O_{5} (s)$

$N_{2} (g) + 3 O_{2} (g) + H_{2} (g) \to 2 {HNO}_{3} (aq)$ $∆ H ° / kJ = - 414.0$

$N_{2} (g) + 3 O_{2} (g) + H_{2} (g) \to 2 {HNO}_{3} (aq)$ $∆ H ° / kJ = - 86.0$

$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$ $∆ H ° / kJ = - 571.6$

MEDIUM

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 24

Determine $∆ H ° / kJ$ for the following reaction using the listed enthalpies of reaction:

$4 CO (g) + 8 H_{2} (g) \to 3 {CH}_{4} (g) + {CO}_{2} (g) + 2 H_{2} O (l)$

$C (graphite) + \frac{1}{2} O_{2} (g) \to CO (g)$ $∆ H ° / kJ = - 110.5 kJ$

$CO (g) + \frac{1}{2} O_{2} (g) \to {CO}_{2} (g)$ $∆ H ° / kJ = - 282.9 kJ$

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l)$ $∆ H ° / kJ = - 285.8 kJ$

$C (graphite) + 2 H_{2} (g) \to {CH}_{4} (g)$ $∆ H ° / kJ = - 74.8 kJ$

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 25

Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

$2 LiOH (s) + {CO}_{2} (g) \to {Li}_{2} {CO}_{3} (s) + H_{2} O (l)$

$∆ H_{f}^{°} LiOH (s) = - 487.23 kJ / mole$

$∆ H_{f}^{°} {Li}_{2} {CO}_{3} (s) = - 1215.6 kJ / mole$

$∆ H_{f}^{°} H_{2} O (l) = - 285.85 kJ / mole$

$∆ H_{f}^{°} {CO}_{2} (g) = - 393.5 kJ / mole$

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JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 26

Given:

${NH}_{3} (g) + 3 {Cl}_{2} (g) ⇌ {NCl}_{3} (g) + 3 HCl (g); - ∆ H_{1} N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g); - ∆ H_{2} H_{2} (g) + {Cl}_{2} (g) ⇌ 2 HCl (g); ∆ H_{3}$

The heat of formation of ${NCl}_{3} (g)$ in terms of $∆ H_{1}$ , $∆ H_{2}$ ,and $∆ H_{3}$ is

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 27

Determine $∆ H °$ of the following reaction using the listed heats of formation:

$4 {HNO}_{3} (l) + P_{4} O_{10} (s) \to 2 N_{2} O_{5} (s) + 4 {HPO}_{3} (s)$

$∆ H_{f}^{°} {HNO}_{3} (l) = - 174.2 kJ / mole$

$∆ H_{f}^{°} N_{2} O_{5} (s) = - 43.1 kJ / mole$

$∆ H_{f}^{°} P_{4} O_{10} (s) = - 2984.0 kJ / mole$

$∆ H_{f}^{°} {HPO}_{3} (s) = - 948.5 kJ / mole$

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 28

x_{1}, x_{2}

and

x_{3}

are enthalpies of

H - H, O = O

and

O - H

bonds respectively, and

x_{4}

is the enthalpy of vaporization of water, estimate the standard enthalpy of combustion of hydrogen.

Calculate the heat of combustion kJ of propane, C3H8 using the listed standard enthalpy of reaction data: C3H8g+5O2g→3CO2g+4H2Og 3Cs+4H2g→C3H8g ∆H°/KJ=-103.8 Cs+O2g→CO2g ∆H°/KJ=-393.5 H2g+12O2g→H2Og ∆H°/KJ=-241.8

Important Questions on Thermodynamics

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