MCQ (Practice) - Thermodynamics (Level 1) Part -1 - Class 11 MCQ

Based on the first law of thermodynamics, which one of the following is correct? 

One mole of ideal gas is allowed to expand reversibly and adiabatically from a temperature of 27°C. If the work done by the gas in the process is 3 kJ, the final temperature will be equal to (C_v = 20 J/K mol)

What is the change in internal energy when a gas contracts from 377 ml to 177 ml under a constant pressure of 1520 torr, while at the same time being cooled by removing 124 J heat ? [Take : (1 L atm) = 100 J]

The heat capacity of liquid water is 75.6 J/mol K, while the enthalpy of fusion of ice is 6.0 kJ/mol. What is the smallest number of ice cubes at 0°C, each containing 9.0 g of water, needed to cool 500 g of liquid water from 20°C to 0°C?

An ideal gas is taken around the cycle ABCDA as shown in figure. The net work done during the cycle is equal to :

Molar heat capacity of water in equilibrium with ice at costant pressure is

A cyclic process ABCD is shown in PV diagram for an ideal gas. Which of the following diagram represents the same process ?

A diatomic ideal gas initially at 273 K is given 100 cal heat due to which system did 209 J work. Molar heat capcity (C_m) of gas for the process is :

One mole of an ideal monoatomic gas expanded irreversibly in two stage expansion.

State-1 (8.0 bar, 4.0 litre, 300 K)

State-2 (2.0 bar, 16 litre, 300 K)

State-3 (1.0 bar, 32 litre, 300 K)

Total heat absorbed by the gas in the process is :

For an ideal monoatomic gas during any process T = kV, find out the molar heat capacity of the gas during the process. (Assume vibrational degree of freedom to be active)

A gas (C_v,m = ) behaving ideally was allowed to expand reversibly and adiabaticaly from 1 litre to 32 litre. It's initial temperature was 327°C. The molar enthalpy change (in J/mole) for the process is

The bond energy (in kcal mol^–1) of a C—C single bond is approximately 

Two moles of an ideal gas (C_v = ) was compressed adiabatically against constant pressure of 2 atm. Which was initially at 350 K and 1 atm pressure. The work involve in the process is equal to

An insulated container of gas has two chambers separated by an insulating partition. One of the chambers has volume V₁ and contains ideal gas at pressure P₁ and temperature T₁. The other chambers has volume v₂ and contains ideal gas at pressure P₂ and temperature T₂. If the partion is removed without doing any work on the gas, the final equilibrium temperature of the gas in the container will be

The maximum efficiency of a heat engine operating between 100°C and 25°C is

A heat engine operating between 227°C and 27°C absorbs 2 Kcal of heat from the 227°C reservoir reversibly per cycle. The amount of work done in one cycle is :

A reversible heat engine A (based on carnot cycle) absorbs heat from a reservoir at 1000 K and rejects heat to a reservoir at T₂. A second reversible engine B absorbs, the same amount of heat as rejected by the engine A, from the reservoir at T₂ and rejects energy to a reservoir at 360 K. If the efficiencies of engines A and B are the same then the temperautre T₂ is

For the reaction at 300 K

A(g) + B(g) → C(g) DE = -3.0 kcal ; ΔS = -10.0 cal/K

value of ΔG is

The entropy change when two moles of ideal monoatomic gas is heated from 200 to 300°C reversibly and isochorically

What is the free energy change (ΔG) when 1.0 mole of water at 100° C and 1 pressure is converted into steam at 100°C and 1 atm pressure ?

What if the free energy change (ΔG) when 1.0 mole of water at 100°C and 1 atm pressure is converted into steam at 100°C and 2 atm pressure ?

What can be concluded about the values of ΔH and ΔS from this graph ?

If DH_vaporisation of substance X (l) (molar mass : 30 g/mol) is 300 J/g at it's boiling point 300 K, then molar entropy change for revesible condensation process is

Pressure of 10 moles of an ideal gas is changed from 2 atm to 1 at against constant external pressure without change in temperature. If surrounding temperature (300K) and pressure (1 atm) always remains constant then calculate total entropy change (ΔS_system + ΔS_surrounding) for given process.

The enthalpy of tetramerization of X in gas phase (4X(g) → X₄(g)) is _100 kJ/mol at 300 K. The enthalpy of vaporisation for liquid X and X₄ are respectively 30 kJ/mol and 72 kJ/mol respectively. ΔS for tetramerization of X in liquid phase is –125 J/K mole at 300 K. What is the ΔG at 300 K for tetramerization of x in liquid phase.

The change in entropy of 2 moles of an ideal gas upon iosthermal expansion at 243.6 K from 20 litre until the pressure becomes 1 atm, is :

Standard entropy of X₂, Y₂ and XY₃ are 60, 40 and 50 JK^-1 mol^-1, respectively. For the reaction,  , ΔH = –30 kJ to be at equilibrium, the temperature will be