When 1 mole of an ideal gas to 20 atm pressure and 15 L volume expands such that the final pressure becomes 10 atm and the final volume become 60 L. Calculate entropy change for the reaction (Cp.m = 30.96)

1. 80.2 J k-1mol-1

2. 62.42 J k-1mol-1

3. 120×102 J k-1mol-1

4. 27.22 J k-1mol-1

Subtopic:  Spontaneity & Entropy |
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NEET 2023 - Target Batch - Aryan Raj Singh
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If a process is both endothermic and spontaneous, then :

1. S>0

2. S<0

3. H<0

4. G>0

Subtopic:  Gibbs Energy Change |
 78%
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The bond energies of C=C and C-C at 298 K are 590 and 331 kJ mol-1 respectively. The enthalpy of polymerization per mole of ethylene is

1. -70 kJ

2. -72 kJ

3. 72 kJ

4. -68 kJ

Subtopic:  Thermochemistry |
 70%
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1 mole of NH3 gas at 27C is expanded adaibatic condition to make volume 8 times (γ=1.33). Final temperature and work done respectively are-

1. 150 K, 900 cal

2. 150 K, 400 cal

3. 250 K, 1000 cal

4. 200 K, 800 cal

Subtopic:  Cp & Cv |
 63%
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Which of the following statements is correct with regard to G of a cell reaction and EMF of the cell (E) in which the reaction occurs ?

(1) Both G and E are extensive properties

(2) G is an intensive property but E is an extensive property

(3) G is an extensive property and E is an intensive property

(4) Both G and E are intensive properties.

Subtopic:  Classification of System, Extensive & Intensive Properties |
 56%
From NCERT
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Temperature of 1 mol of a gas is increased by 1 at constant pressure. Work done is-

1. -R

2. 2R

3. R/2

4. 3R

Subtopic:  First Law of Thermodynamics |
 77%
From NCERT
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When 0.16 g of glucose was burnt in a bomb calorimeter, the temperature rose by 4 deg. Calculate the calorimeter constant (water equivalent of the calorimeter) given that H=-2.8×106 J mol-1. [molar enthalpy of combustion]. Molar mass of glucose = 180 mol-1.

1. 5.73×102 J/deg

2. 7.53×102 J/deg

3. 6.22×102 J/deg

4. 3.57×102 J/deg

Subtopic:  Thermochemistry |
 51%
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The C-Cl bond energy can be calculated from :

1. HfCCl4, l only

2. fCCl4, l and Cl2

3. HfCCl4, l Cl2

4. HfCCl4, l Cl2, HfC, g and HvapCCl4

Subtopic:  Thermochemistry |
 63%
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Given Hf of DyCl3 (s) = -994.30 kJ mol-1

12H2g+12Cl2g+aqHClaq. 4 M;              H=-158.31 kJ mol-1
DyCl3sHClaqDyCl3aq. 4 M HCl;                H=-180.06 kJ mol-1
Dysaq. 4 M+3 HClDyCl3aq. 4 M HCl+32H2g;   H=x, calculate x.

1. -966.5 kJ/mol

2. -699.43 kJ/mol

3. -596.6 kJ/mol

4. -569.6 kJ/mol

Subtopic:  Thermochemistry |
 67%
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When 1 g H2 gas at S.T.P is expanded to twice its initial volume, then the work done is:

1. 22.4 L atm
2. 5.6 L atm
3. 11.2 L atm
4. 44.8 L atm

Subtopic:  First Law of Thermodynamics |
 56%
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