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11th Chemistry Monthly Test - 1 ( Thermodynamics )

MABS Institution

11th Chemistry Monthly Test - 1 ( Thermodynamics )-Aug 2020

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

Molar heat capacity at constant volume is------

\({ \left( \frac { dH }{ dT } \right) }_{ V }\)
\({ \left( \frac { dU }{ dT } \right) }_{ V }\)
\({ \left( \frac { dq }{ dT } \right) }_{ V }\)
\({ \left( \frac { dV}{ dT } \right) }_{ V }\)

For a given reaction \(\triangle\)G obtained was having positive sign convention. State whether the reaction was spontaneous or non-spontaneous.

spontaneous
non-spontaneous
reversible
equilibrium

All naturally occurring processes are ----- process

reversible
irreversible
cyclic process
isochoric process

The enthalpies of all elements in their standard states are ____

1
0
<0
different for each elements

The temperature of the system, decreases in an ---------

Isothermal expansion
Isothermal Compression
adiabatic expansion
adiabatic compression

The SI unit of entropy is ______

JK
JK^-1
KJ K^-1
KJ / mole

The process in which volume of the system remains constant is called ------ process

isobaric
cyclic
isothermal
isochoric

-----is an intensive property

internal energy
volume
temperature
mass

--------is an example for closed system.

Solution ofCuSO₄ in a beaker
A gas contained in a cylinder fitted with piston
Hot water contained in a thermos flask
Tea in a cup

When 15.68 litres of a gas mixture of methane and propane are fully combusted at 0° C and 1 atmosphere, 32 litres of oxygen at the same temperature and pressure are consumed. The amount of heat of released from this combustion in KJ is (ΔH_c (CH₄) = - 890 KJ mol^-1and ΔH_c(C₃H₈ = - 2220 KJ mol^-1)

- 889 K.Jmol^-1
- 1390 K.Jmol^-1
- 3180 K.Jmol^-1
- 635.47 K.Jmol^-1

Part - B

Generic 2 - Answer All Question

Define enthalpy of combustion.

Define molar heat capacity. Give its unit

Identify the state and path function out of the following: a) Enthalpy b) Entropy c) Heat d) Temperature e) Work f) Free energy.

Define Gibb's free energy.

Define the calorific value of food. What is the unit of calorific value?
Define Hess's law of constant heat summation. (or) State Hess's law.

Predict the feasibility of a reaction when
(i) both ΔH and ΔS positive
(ii) both ΔH and ΔS negative
(iii) ΔH decreases but ΔS increases

What is lattice energy?

State the first law of thermodynamics.

Explain intensive properties with two examples

Part - C

Generic 3 - Answer All Question

Explain the relationship between free energy and equilibrium constant.

Answer the following questions with respect to I law of thermodynamics.
(i) State the law
(ii) Give its mathematical expression.
(iii) List out its Umitations

Heat is considered as a path function, but in an endothermic process, the heat absorbed by the system under certain specific conditions is independent of path. What are those conditions?

State the various statements of second law of thermodynamics.

Define the Molar Heat of Vapourisation

Bring out the differences between extensive and intensive properties.
Define standard entropy change.

Find out the value of equilibrium constant for the following reaction at 298K; 2NH_3(g)+ CO_2(g) \(\leftrightharpoons\)

NH₂CONH_2(aq) + H₂O(I) Standard Gibbs energy change, \(\Delta G_{r}^{o}\) at the given temperature is -13.6 kJ mol^-1.

State zeroth law of thermodynamics.

Which law of thermodynamics deals with equivalence of different forms of energies?

Part - D

Generic 5 - Answer All Question

For the equilibrium \({ PCl }_{ 5 }\rightleftharpoons { PCl }_{ 3(g) }+{ Cl }_{ 2(g) }\) at 298 K, K is 1.8 x 10^-7. What is the ΔG⁰ for the reaction?

Show that the reaction \(CO+\frac { 1 }{ 2 } { O }_{ 2 }\longrightarrow { CO }_{ 2 }\) at 300K is spontaneous. The standard Gibbs free energies of formation of CO₂ and CO are -394.4 and -137.2 KJ mole^-1 respectively.

Calculate the enthalpy change for the reaction
Fe₂O₃ + 3CO ⟶ 2Fe + 3CO₂ from the following data.
2Fe +\(\frac{3}{2}\)O₂ ⟶ Fe₂O₃; ΔH = -741 kJ
C +\(\frac{1}{2}\)O₂ ⟶ CO; ΔH = -137 kJ
C + O₂ ⟶ CO₂; ΔH = - 394.5 kJ

Suggest and explain an indirect method to calculate lattice enthalpy of sodium chloride crystal

Define the following terms
(a) isothermal process (b) adiabatic process
(c) isobaric process (d) isochoric process

What is the equilibrium constant Keq for the following reaction at 400K.
2NOCI_(g)\(\leftrightharpoons\) 2NO_(g) + Cl_2(g)
given that ΔH^o = 77.2kJ mol^-1
and ΔS^o= 122JK^-1mol^-1
At 333K, N₂O₄ is fifty percent dissociated. Calculate the standard free energy change at this temperature and at one atmosphere.

Calculate the standard entropy of formation \(\Delta { S }_{ f }^{ o }\) of CO_2(g). Given the standard entropies of CO_2(g), C_(s), O_2(g) as 218.8, 8.740 and 205.60 Jk^-1 respectively.

In the reaction N_2(g) + O_2(g) ⟶ 2NO_(g), ΔH⁰_reaction is 179.9 KJ mol^-1 and ΔS⁰_reaction=78.09 JK-1mol^-1. Calculate ΔG⁰_reaction at 300 K.

Calculate the standard free energy change \(({ \Delta G }^{ o })\) of the following reaction and say whether it is feasible at 373 K or not.\(\frac{1}{2}H_{2(g)}+\frac{1}{2}I_{2(g)} \rightarrow HI_{(g)}\) \({ \Delta H }_{ r }^{ o }\) is + 25.95 kJ mol^-1 standard entropies of HI_(g) H_2(g) and I_2(g) are 206.3,140.6 and 118.7 Jk^-1 mol-1.

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