Thermodynamics Test

Question 1
1 / -0

Calculate $${ \Delta H }/{ kJ }$$ for the following reaction using the listed standard enthalpy of reaction data.
$$2{ N }_{ 2 }\left( g \right) +5{ O }_{ 2 }\left( g \right) \longrightarrow 2{ N }_{ 2 }{ O }_{ 5 }\left( s \right) $$

$${ N }_{ 2 }\left( g \right) +3{ O }_{ 2 }\left( g \right) +{ H }_{ 2 }\left( g \right) \longrightarrow 2HN{ O }_{ 3 }\left( aq \right) ; \ { \Delta H }/{ kJ }=-414.0$$

$${ N }_{ 2 }{ O }_{ 5 }\left( s \right) +{ H }_{ 2 }O\left( l \right) \longrightarrow 2HN{ O }_{ 3 }\left( aq \right) ; \ { \Delta H }/{ kJ }=-86.0$$

$$2{ H }_{ 2 }\left( g \right) +{ O }_{ 2 }\left( g \right) \longrightarrow 2{ H }_{ 2 }O\left( l \right) ; \ { \Delta H }/{ kJ }=-571.6$$

A
-84.4

B
-243.6

C
-71.2

D
-121.8

Question 2
1 / -0

Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:
$${ C }_{ 2 }{ H }_{ 5 }OH\left( l\right) +3{ O }_{ 2 }\left( g \right) \longrightarrow 2C{ O }_{ 2 }\left( g \right) +3{ H }_{ 2 }O\left( g \right) $$
$$\Delta { H }_{ f }^{ }{ C }_{ 2 }{ H }_{ 5 }OH\left( l \right) =-277.7{ kJ }/{ mole }$$
$$\Delta { H }_{ f }^{ }C{ O }_{ 2 }\left( g \right) =-393.5{ kJ }/{ mole }$$
$$\Delta { H }_{ f }^{ }{ H }_{ 2 }O\left( g \right) =-241.8{ kJ }/{ mole }$$

A
-1456.3

B
-1234.7

C
-1034.0

D
-1119.4

Question 3
1 / -0

0.16 g of methane was subjected to combustion at $$27^{\circ}C$$ in a bomb calorimeter. The temperature of the calorimeter system (including water) was found to rise by $$0.5^{\circ}C$$.
Calculate the heat of combustion of methane at constant pressure. The thermal capacity of the calorimeter system is $$17.7 \: kJ \: K^{-1}$$.
$$[R = 8.314 \: JK^{-1}\: mol^{-1}]$$.

A
-890

B
890

C
-750

D
None of these

Question 4
1 / -0

The enthalpy change for the following process at $${25}^{o}C$$ and under constant pressure at $$1$$ atm are as follows:
$${CH}_{4}(g)\longrightarrow C(g)+4H(g)$$ $${\Delta}_{r}H=396kcal/mole$$
$${C}_{2}{H}_{6}(g)\longrightarrow 2C(g)+6H(g)$$ $${\Delta}_{r}H=676kcal/mole$$

Calculate $$C-C$$ bond energy in $${C}_{2}{H}_{6}$$ and heat formation of $${C}_{2}{H}_{6}(g)$$.

[Given: $${\Delta}_{sub}C(s)=171.8kcal/mole$$ $$B.E(H-H)=104.1kcal/mole$$]

A
$$B.E(C-C)=82kcal/mol, {\Delta}_{f}H[{C}_{2}{H}_{6}(g)]=-20.1kcal/mol$$

B
$$B.E(C-C)=-82kcal/mol, {\Delta}_{f}H[{C}_{2}{H}_{6}(g)]=-20.1kcal/mol$$

C
$$B.E(C-C)=82kcal/mol, {\Delta}_{f}H[{C}_{2}{H}_{6}(g)]=+20.1kcal/mol$$

D
None of these

Question 5
1 / -0

Use the given bond enthalpy data to estimate the $$\Delta H\left( kJ \right) $$ for the following reaction.
$$\left( C - H = 414 kJ, H - Cl = 431 kJ, Cl - Cl = 243 kJ, C - Cl = 331 kJ \right) $$.
$$C{ H }_{ 4 }\left( g \right) + 4{ Cl }_{ 2 }\left( g \right) \longrightarrow C{ Cl }_{ 4 }\left( g \right) + 4HCl\left( g \right) $$

A
620

B
330

C
420

D
105

Question 6
1 / -0

Caesium chloride is formed according to the following equation:

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

The enthalpy of sublimation of $$Cs$$, enthalpy of dissociation of chlorine, ionization energy of $$Cs$$ and electron affinity of chlorine are $$81.2, 243.0, 375.7$$ and $$-348.3kJ$$ $${ol}^{-1}$$. The energy change involved in the formation of $$CsCl$$ is $$388.6\ kJ.{mol}^{-1}$$. Calculate the lattice energy of $$CsCl$$.

A
$$-618.7\ kJ{mol}^{-1}$$

B
$$+618.7\ kJ{mol}^{-1}$$

C
$$1315.2\ kJ{mol}^{-1}$$

D
None of these

Question 7
1 / -0

Using the data (all values are in $$kJ/mol$$ at $${25}^{o}C$$) given below:

(i) Enthalpy of polymerization of ethylene$$=-72$$
(ii) Enthalpy of formation of benzene $$(l)=49$$
(iii) Enthalpy of vaporization of benzene $$(l)=30$$
(iv) Resonance energy of benzene $$(l)=-152$$
(v) Heat of formation of gaseous atoms from the elements in their standard states $$H=218, C=715$$.

Average bond energy of $$C-H=415$$. Calculate the $$B.E$$ of $$C-C$$ and $$C=C$$.

A
$$C-C=343.67$$, $$C=C=615.33$$

B
$$C-C=615.33$$, $$C=C=342.67$$

C
$$C-C=343.67$$, $$C=C=959$$

D
None of these

Question 8
1 / -0

Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction: $$TiCL_4(g)+2\:H_2O(g)\rightarrow TiO_2(g)+4\:HCl(g)$$

$$\Delta H^{\circ}_f\:TiCL_4(g)=-763.2\:kJ/mol$$
$$\Delta H^{\circ}_f\:TiO_2(g)=-944.7\:kJ/mol$$
$$\Delta H^{\circ}_f\:H_2O(g)=-241.8\:kJ/mol$$
$$\Delta H^{\circ}_f\:HCl(g)=-92.3\:kJ/mol$$

A
$$-\:278.1$$

B
$$+\:369.2$$

C
$$+\:67.1$$

D
$$-\:67.1$$

Question 9
1 / -0

A piston filled with 0.04 mole of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 37.0°C. As it does so, it absorbs 207 J of heat. The values of q and W for the process will be :
[Take : R = 8.314 J / mol K, In 7.5 = 2.01]

A
q = +207, W = -207

B
q = -207, W = -207

C
q = -207, W = +207

D
q = +207, W = +207

Question 10
1 / -0

A swimmer coming out from a pool is covered with a film of water weighing about 18 g. Calculate the internal energy of vaporisation at 100°C.
[$$\Delta H_{vap}^o$$ for water at 373 K = 40.66 kJ/mol ]

The correct option is:

A
35.67 kJ

B
36.64 kJ

C
37.56 kJ

D
None of the above

Submit Test

Thermodynamics ...

Question 1

-84.4

-243.6

-71.2

-121.8

Question 2

-1456.3

-1234.7

-1034.0

-1119.4

Question 3

-890

890

-750

None of these

Question 4

$$B.E(C-C)=82kcal/mol, {\Delta}_{f}H[{C}_{2}{H}_{6}(g)]=-20.1kcal/mol$$

$$B.E(C-C)=-82kcal/mol, {\Delta}_{f}H[{C}_{2}{H}_{6}(g)]=-20.1kcal/mol$$

$$B.E(C-C)=82kcal/mol, {\Delta}_{f}H[{C}_{2}{H}_{6}(g)]=+20.1kcal/mol$$

None of these

Question 5

620

330

420

105

Question 6

$$-618.7\ kJ{mol}^{-1}$$

$$+618.7\ kJ{mol}^{-1}$$

$$1315.2\ kJ{mol}^{-1}$$

None of these

Question 7

$$C-C=343.67$$, $$C=C=615.33$$

$$C-C=615.33$$, $$C=C=342.67$$

$$C-C=343.67$$, $$C=C=959$$

None of these

Question 8

$$-\:278.1$$

$$+\:369.2$$

$$+\:67.1$$

$$-\:67.1$$

Question 9

q = +207, W = -207

q = -207, W = -207

q = -207, W = +207

q = +207, W = +207

Question 10

35.67 kJ

36.64 kJ

37.56 kJ

None of the above

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