11th Chemistry Monthly Test - 4 ( Thermodynamics )

MABS Institution

11th Chemistry Monthly Test - 4 ( Thermodynamics )-Aug 2020

Time : 2.00 Hours

Part - A

Generic 5 - Answer All Question

Calculate the lattice energy of MgBr₂ from the given data

1 mole of an ideal gas is maintained at 4.1 atm and at a certain temperature absorbs 3710J heat and expands to 2 Iitres. Calculate the entropy change in expansion process.

ΔH and ΔS for the reaction
Ag2O(s) ➝ 2Ag(s)+\(\frac{1}{2}O_{2(g)}\) are 30.56 kJ mol^-1 and 66.0 Jk^-1 mol^-1 respectively. Calculate the temperature at which the free energy for this reaction will be zero. What will be the direction of reaction at this temperature and at temperature below this and why?
ΔH=30.56 kJ mol^-1=30560 J mol^-1
ΔS=66.0 JK^-1 mol^-1
ΔG=0

Calculate the entropy change during the melting of one mole of ice into water at 0°C and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol^-1.

Calculate the change of entropy for the process, water (liq)to water (vapor, 373 K) involving ΔH_vap = 40850J mort at 373 K.

Explain the measurement of heat change at constant pressure with a neat diagram.

Calculate the entropy change in the system, and in the surroundings and the total entropy change in the universe when during a process 75J of heat flow out of the system at 55°C to the surrounding at 20°C.

Calculate the entropy change of a process possessing ΔH_t = 2090 J mole^-1.

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

Discuss in detail about the variation of internal energy with respect to various thermodynamic processes

Write down the Born-Haber cycle for the formation of CaCl₂

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.

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11th Chemistry Monthly Test - 4 ( Thermodynamics )

MABS Institution

11th Chemistry Monthly Test - 4 ( Thermodynamics )-Aug 2020

Part - A

Generic 5 - Answer All Question

Calculate the lattice energy of MgBr2 from the given data

1 mole of an ideal gas is maintained at 4.1 atm and at a certain temperature absorbs 3710J heat and expands to 2 Iitres. Calculate the entropy change in expansion process.

Calculate the entropy change during the melting of one mole of ice into water at 0°C and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol-1.

Calculate the change of entropy for the process, water (liq)to water (vapor, 373 K) involving ΔHvap = 40850J mort at 373 K.

Explain the measurement of heat change at constant pressure with a neat diagram.

Calculate the entropy change in the system, and in the surroundings and the total entropy change in the universe when during a process 75J of heat flow out of the system at 55°C to the surrounding at 20°C.

Calculate the entropy change of a process possessing ΔHt = 2090 J mole-1.

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

Discuss in detail about the variation of internal energy with respect to various thermodynamic processes

Write down the Born-Haber cycle for the formation of CaCl2

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.

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Calculate the lattice energy of MgBr₂ from the given data

Calculate the entropy change during the melting of one mole of ice into water at 0°C and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol^-1.

Calculate the change of entropy for the process, water (liq)to water (vapor, 373 K) involving ΔH_vap = 40850J mort at 373 K.

Calculate the entropy change of a process possessing ΔH_t = 2090 J mole^-1.

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

Write down the Born-Haber cycle for the formation of CaCl₂

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.