Thermodynamics Test

Question 1
1 / -0

Born-Haber cycle can be used to estimate :

A
Lattice energy of ionic crystals

B
Electron gain enthalpy

C
Electronegativity

D
Both (A) and (B)

Question 2
1 / -0

Which one of the following gases possesses the largest internal energy?

A
2 moles of helium occupying $$1m^{3}$$ at 300 K

B
56 kg of nitrogen at 107$$Nm^{-2}$$ and 300 K

C
8 grams of oxygen at 8 atm and 300 K

D
$$6\times 10^{26}$$ molecules of argon occupying $$4m^{3}$$ at 900 K

Question 3
1 / -0

Which of the following relationship is not correct for the relation between $$\Delta H$$ and $$\Delta U$$?

A
When $$\Delta n_{g} = 0$$ then $$\Delta H = \Delta U$$

B
When $$\Delta n_{g} > 0$$ then $$\Delta H > \Delta U$$

C
When $$\Delta n_{g} < 0$$ then $$\Delta H < \Delta U$$

D
When $$\Delta n_{g} = 0$$ then $$\Delta H > \Delta U$$

Question 4
1 / -0

For the electrochemical cell, $$ \mathrm{M} | \mathrm{M}^{+} \| \mathrm{X}^{-} \mid \mathrm{X}, $$
$$ E_{M}^{o}+/ M=0 \cdot 44 V $$ and $$ E_{x / x^-}^{\circ}=0 \cdot 33 V $$From these data one can deduce that

A
$$ M+X \rightarrow M^{+}+X^{-} $$ is the spontaneous reaction

B
$$ M^{+}+X^{-} \rightarrow M+X $$ is the spontaneous reaction

C
$$ E_{c e l l}=0 \cdot 77 V $$

D
$$ \mathrm{E}_{\mathrm{cell}}=-0.77 \mathrm{V} $$

Question 5
1 / -0

Hess's law is applicable for the determination of heat of

A
transition

B
formation

C
reaction

D
all of these

Question 6
1 / -0

The relationship between enthalpy and internal energy change is

A
$$\Delta E=\Delta H+P\Delta V$$

B
$$\Delta H=\Delta E+P\Delta V$$

C
$$\Delta H=-\Delta E-P\Delta V$$

D
$$P\Delta V=\Delta E+\Delta H$$

Question 7
1 / -0

Consider the following processes.
$$\Delta H (kJ/mol)$$
$$1/2A\rightarrow B$$ +150
$$3B\rightarrow 2C+D$$ -125
$$E+A\rightarrow 2D$$ +350
For $$B+D\rightarrow E+2C, \Delta H$$ will be:

A
325 kJ/mol

B
525 kJ/mol

C
-175 kJ.mol

D
-325 kJ/mol

Question 8
1 / -0

The data given below are for vapour phase reactions at constant pressure.
$$C_{2}H_{6}\rightarrow \overset{\bullet} C_{2}H_{5}+ \overset{\bullet}{H};\ \Delta H=420\ kJ\ mol^{-1}$$
$$\overset{\bullet}{C}_{2}H_{5}\rightarrow C_{2}H_{4}+\overset{\bullet}{H};\ \Delta H=168\ kJ\ mol^{-1}$$
The enthalpy change for the reaction for the given reaction is :
$$2\overset{\bullet}{C}_{2}H_{5}\rightarrow C_{2}H_{6}+C_{2}H_{4}$$

A
$$+ 250$$ kJ mol$$^{-1}$$

B
$$+ 588$$ kJ mol$$^{-1}$$

C
$$- 252$$ kJ mol$$^{-1}$$

D
$$- 588$$ kJ mol$$^{-1}$$

Question 9
1 / -0

Assertion (A): At equilibrium $$\Delta G$$ becomes zero.
Reason (R): At equilibrium the two tendencies $$\Delta H$$and $$T\Delta S$$ become equal.

A
Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

B
Both Assertion and Reason are true but Reason is not the correct explanation of Assertion.

C
Assertion is true but Reason is false.

D
Assertion is false and Reason is true.

Question 10
1 / -0

Match the list -I with list - II.
List-I List - II
A) Hess law is not applicable for 1) is not a state function
B) All combustion reactions are 2) Heat of dilution
C) Work 3) Exothermic
D) Difference between two integral 4) Nuclear reaction
heats of solutions

A
A-1, B-2, C-3, D-4

B
A-4, B-3, C-1, D-2

C
A-3, B-2, C-4, D-1

D
A-2, B-1, C-4, D-3

Submit Test

	$$\Delta H (kJ/mol)$$
$$1/2A\rightarrow B$$	+150
$$3B\rightarrow 2C+D$$	-125
$$E+A\rightarrow 2D$$	+350

Thermodynamics ...

Question 1

Lattice energy of ionic crystals

Electron gain enthalpy

Electronegativity

Both (A) and (B)

Question 2

2 moles of helium occupying $$1m^{3}$$ at 300 K

56 kg of nitrogen at 107$$Nm^{-2}$$ and 300 K

8 grams of oxygen at 8 atm and 300 K

$$6\times 10^{26}$$ molecules of argon occupying $$4m^{3}$$ at 900 K

Question 3

When $$\Delta n_{g} = 0$$ then $$\Delta H = \Delta U$$

When $$\Delta n_{g} > 0$$ then $$\Delta H > \Delta U$$

When $$\Delta n_{g} < 0$$ then $$\Delta H < \Delta U$$

When $$\Delta n_{g} = 0$$ then $$\Delta H > \Delta U$$

Question 4

$$ M+X \rightarrow M^{+}+X^{-} $$ is the spontaneous reaction

$$ M^{+}+X^{-} \rightarrow M+X $$ is the spontaneous reaction

$$ E_{c e l l}=0 \cdot 77 V $$

$$ \mathrm{E}_{\mathrm{cell}}=-0.77 \mathrm{V} $$

Question 5

transition

formation

reaction

all of these

Question 6

$$\Delta E=\Delta H+P\Delta V$$

$$\Delta H=\Delta E+P\Delta V$$

$$\Delta H=-\Delta E-P\Delta V$$

$$P\Delta V=\Delta E+\Delta H$$

Question 7

325 kJ/mol

525 kJ/mol

-175 kJ.mol

-325 kJ/mol

Question 8

$$+ 250$$ kJ mol$$^{-1}$$

$$+ 588$$ kJ mol$$^{-1}$$

$$- 252$$ kJ mol$$^{-1}$$

$$- 588$$ kJ mol$$^{-1}$$

Question 9

Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

Both Assertion and Reason are true but Reason is not the correct explanation of Assertion.

Assertion is true but Reason is false.

Assertion is false and Reason is true.

Question 10

A-1, B-2, C-3, D-4

A-4, B-3, C-1, D-2

A-3, B-2, C-4, D-1

A-2, B-1, C-4, D-3

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