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Earn 100

$0.16 g$ of methane was subjected to combustion at $27^{°} C$ in a bomb calorimeter. The temperature of calorimeter system (including water) was found to rise by $0 . 5^{°} C$ . Calculate the heat of combustion of methane at constant pressure (in $kJ {mol}^{- 1}$ ).
The thermal capacity of calorimeter system is $17.7 kJ K^{- 1}$ . $(R = 8.313 {mol}^{- 1} K^{- 1})$

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Important Questions on Thermodynamics

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IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-3>Q 50

When

1.0 g

of fructose

C_{6} H_{12} O_{6} (s)

is burnt in oxygen in a bomb calorimeter, the temperature of the calorimeter water increases by

1 . 56^{°} C

. If the heat capacity of the calorimeter and its contents is

10.0 kJ /^{°} C

. Calculate the enthalpy of combustion of fructose at

298 K

. (in

kJ {mol}^{- 1}

)

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-3>Q 51

The enthalpy of dissociation of

{PH}_{3}

954 kJ / mol

and that of

P_{2} H_{4}

1.485 M J {mol}^{- 1}

. What is the bond enthalpy of the

P - P

bond? (in

kJ {mol}^{- 1}

)

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-3>Q 52

Using the bond enthalpy data given below, calculate the enthalpy change for the reaction, (in

kJ {mol}^{- 1}

)

$C_{2} H_{4} (g) + H_{2} (g) \to C_{2} H_{6} (g)$

Data :

Bond	$C - C$	$C = C$	$C - H$	$H - H$
Bond Enthalpy	$336.81 kJ / mol$	$606.68 kJ / mol$	$410.87 kJ / mol$	$431.79 kJ / mol$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-3>Q 53

The enthalpy change for the following process at

25^{°} C

and under constant pressure at

1 atm

are as follows :

${CH}_{4} (g) \to C (g) + 4 H (g)$ $∆_{f} H = 396 kcal / mole$

$C_{2} H_{6} (g) \to 2 C (g) + 6 H (g)$

$∆_{f} H = 676 kcal / mole$

Calculate $C - C$ bond energy in $C_{2} H_{6}$ (in $kcal {mol}^{- 1}$ )

Given : $∆_{sub} C (s) = 171.8 kcal / mole$

$B . E . (H - H) = 104.1 kcal / mole$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-3>Q 54

Find the enthalpy of

S - S

bond (in

kJ {mol}^{- 1}

) from the following data.

(i) $C_{2} H_{5} - S - C_{2} H_{5} (g) ∆ H_{f}^{°} = + 147.2 kJ / mol$

(ii) $C_{2} H_{5} - S - S - C_{2} H_{2} (g) ∆ H_{f}^{°} = + 201.9 kJ / mol$

(iii) $S (g) ∆ H_{f}^{°} = + 222.8 kJ / mol$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-3>Q 55

Calculate the electron affinity of fluorine atom (in

kJ {mol}^{- 1}

) using the following data. Make Born-Haber's cycle. All the values are in

kJ {mol}^{- 1}

25^{°} C, ∆ H_{diss} (F_{2}) = 160 kJ {mol}^{- 1}, ∆ H_{f}^{°} (NaF (s)) = - 571 kJ {mol}^{- 1} . I . E . [Na (g)] = 494 kJ {mol}^{- 1}

∆ H_{vap} = [Na (s)] = 101 kJ {mol}^{- 1}

. Lattice energy of

NaF (s) = - 894

kJ {mol}^{- 1}

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-3>Q 56

Cesium chloride is formed according to the following equation :

$Cs (s) + 0.5 {Cl}_{2} (g) \to CsCl (s)$ .

The enthalpy of sublimation of $Cs$ , enthalpy of dissociation of chloride, ionization energy of $Cs$ & electron affinity of chlorine are $81.2, 243.0, 375, 7$ and $- 348.3 kJ {mol}^{- 1}$ . The energy change involved in the formation of $CsCl$ is $- 388.6 kJ {mol}^{- 1}$ . Calculate the lattice energy of $CsCl$ . (in $kJ {mol}^{- 1}$ ) enolved.

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-3>Q 57

The enthalpy of formation of ethane, ethylene and benzene from the gaseous atom are

- 2839.2, - 2275.2

and

- 5506 kJ {mol}^{- 1}

respectively. Calculate the modulus of resonance energy of benzene (in

kJ {mol}^{- 1}

). The bond enthalpy of

C - H

bond is given as equal to

+ 410.87 kJ / mol

Important Questions on Thermodynamics

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