Daily Practice Problems
NEET Chemistry
Thermodynamics
NEET Chemistry
Thermodynamics
Question 1.
Which of the following statement obeyed third law of thermodynamics?
[Level: Moderate]
(a) The entropy of 1 mole of solid HCl at 0K is zero while entropy of one mole of solid CO is 5J/K.
(b) Entropy of an isolated system can never decrease over time
(c) Conservation of energy
(d) None of these
Question 2.
At equilibrium, value of free energy change is [Level: Easy]
(a) +ve
(b) -ve
(c) zero
(d) A & B both
Question 3.
Equilibrium constant for a reaction is e-2then ∆G0 is – [Level: Moderate]
(a) -2 J/Mol
(b) 2 J/Mol
(c) -4.606 J/Mol
(d) e J/Mol
Question 4.
Calculate W and ∆E for the conversion of 1 mole of water into 1 Mole of steam at a temperature of 1000C and at a pressure of 1 atmosphere latent heat of vaporisation of water is 9720 cal/mol. [Level: Difficult]
(a) 8979 cal
(b) 8000 cal
(c) 89.2 KJ
(d) 90 J
Question 5.
The net internal energy change in reversible cyclic process is –[Level: Difficult]
(a) 
RT
(b) Zero
(c) Greater than zero
(d) Less than Zero
Question 6.
Calculate the temperature at which 32g of O2 will occupy a volume of 10.0 L at 3.16 atm. [Level: Easy]
(a) 273.1k
(b) 384.8K
(c) 348.6K
(d) 1170C
Question 6.
During a thermodynamic process, 93 KJ of heat flows into the system and work done by the system is 47KJ. The increase in internal energy of the system is – [Level: Moderate]
(a) Ammonia < Methane
(b) Ammonia > Methane
(c) +52KJ
(d) Diffusion will not take place
Question 7.
If the standard enthalpies of formation (∆H0f) for CO2, CO, H2O are -453.5,-217.3 and -141.8 KJmol-1respectively than what will be the change in enthalpy for the reaction – [Level: Easy]
(a) +194.4kJ
(b) +94.4kJ
(c) +84.4kJ
(d) -94.4kJ
Question 8.
Plants and living being are the example of –
(a) Adiabatic system
(b) Isolated system
(c) Open system
(d) Closed system
Question 9.
In a fuel cell (Device used for producing electricity directly from a chemical reaction) methanol is used as fuel and oxygen gas is used as an oxidizer. The standard enthalpy of combustion of methanol is -726 KJmol-1. The standard free enthalpy of formation of CH3OH(l),CO2(g) and H2O(l) are -126.3,-434.4 and -257.1 KJmol-1 Respectively then find the standard free energy for the reaction. [Level: Moderate]
(a) 9 dm3
(b) 3 dm3
(c) 4 dm3
(d) 5 dm3
Question 10.
The efficiency of the fuel cell will be:
(Hint: Use value of standard free energy from Q.9) [Level: Easy]
(a) 96.7%
(b) 66.2%
(c) 41.3%
(d) 85.1%
Question 11.
29 ml of pure water takes 90 sec to evaporate from a vessel and heater connected to an electric source which delivers 716 watt. The ∆Hvap of water is: –[Level: Moderate]
(b) 40000 J/m Approx
(c) 31.901 KJ/m Approx
(d) 45.104 KJ/m Approx
Question 12.
Calculate the work performed when 3 moles of hydrogen expand isothermally and reversibly at 270C from 35 to 70 L – [Level: Moderate]
(a) - 1247.7 cal
(b) - 1247.7 erg
(c) – 12.47 cal
(d) - 1247.7 J
Question 13.
4 mole of NH3(Υ = 1.33) gas at 307K is expanded under adiabatic condition to increase the volume 0.5 times then what will be the temperature and the value of work done – [Level: Difficult]
(a) T2 = 614, W= -1.268
(b) T2 = 614, W= -7008
(c) T2 = 641, W= -8765
Question 14.
Five moles of gas is put through a series of changes as shown graphically in cycle process
The process AàB, B àC and CàA are respectively [Level: Easy]
(a) Isochoric, Isobaric, Isothermal
(b) Isobaric, Isochoric, Isothermal
(c) Isochoric, Isothermal, Isobaric
(d) Isobaric, Isothermal, Isochoric
Question 15.
For the gas phase reaction:
PCl5 ⇌ PCl3 + Cl2
Which of the following conditions are correct [Level: Moderate]
(a) ∆H < 0, ∆S < 0
(b) ∆H > 0, ∆S < 0
(c) ∆H = 0, ∆S < 0
(d) ∆H > 0, ∆S > 0
Question 16.
Find ∆Sf0 at 250C for PCl5(g) If ∆Hf0 is -396.9 KJ/mole and ∆G0f is -315 KJ/mol. [Level: Easy]
(a) ∆S0 = -0.274.8 KJ/mol K
(b) ∆S0 = -274.8 J/mol K
(c) ∆S0 = -274.8 x 107 erg/mol K
(d) All of these
Question 17.
What will be the pressure of 5 mol of an ideal gas at 314K having volume 11.8 L? [Level: Easy]
(a) 1 atm
(b) 2.12 atm
(c) 9.0 atm
(d) 11 atm
Question 18.
Calculate the entropy change involved in the conversion of one mole of water at 396K to vapour at the same temperature. (Latent heat of vaporization of Water = 2.257KJg-1) : [Level: Easy]
(c) ∆SV = 10.5JK-1Mol-1
(d) ∆SV = 201.5JK-1Mol-1
Question 19.
Calculate ∆H at 457K for reaction
Fe2O3(S) + 3H2(g) à 2Fe + 3H2O(l)
Given that ∆H298 = -33.29 Kj Mol-1 and Cp for Fe2O3(s), Fe(s), H2O(l) and H2(g) are 98.8, 29.1, 64.3 and 18.7 J/K mole
(a) -18.3291 KJ/mol
(b) -183291 KJ/mol
(c) 18.3291 KJ/mol
(d) 18.3291 J/mol
Question 20.
At a given temperature, the energy of activation of two reaction is same if [Level: Easy]
(a) The specific rate constant for the two reaction is the same
(b) The temperature coefficient for the specific rate constant for the two reaction is same
(c) ∆H for the two reaction is the same but not Zero
(d) ∆H for the two reactant is zero
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