Thermodynamics – Chemistry | NEET Online Mock Test

Find the set of intensive properties from the following statements

1. Vapour pressure, specific heat and Dielectric constant
2. E⁰_cell, melting point and viscosity
3. Refractive index, surface tension and molarity
4. All of these

2 mole of an ideal gas at 27°C expands isothermally and reversibly from a volume of 4L to 40L. The workdone (in KJ) by the gas is -

Find the incorrect from the following

1. PCl₅(g) → PCl₃(g) + Cl₂(g) (△H = △E)
2. 2HI(g) → H₂(g) + l₂(g) (△H = △E)
3. C(s) + H₂O(g) → CO(g) + H₂(g) (△H > △E)
4. All of these

Which of the following is the correct option for free expansion of an ideal gas under adiabatic conditions?

1. q = 0, △T = 0, w ≠ 0
2. q = 0, △T = 0, w = 0
3. q ≠ 0, △T ≠ 0, w ≠ 0
4. q = 0, △T ≠ 0, w = 0

In which of the following reaction maximum amount of heat is evolved?

1. HNO₃(aq) + NaOH (aq)
2. CH₃COOH (aq) + NaOH (aq)
3. HCI (aq) + NH₄OH (aq)
4. HF (aq) + NaOH (aq)

If heat of formation (△H°) of C₂H₄ and C₂H₆ are x₁ and x₂ kcal mol-1 respectively, then heat of hydrogenation of C₂H₄ is

1. x₁ + x₂
2. x₁ - x₂
3. x₂ - x₁
4. x₁ + 2x₂

Calculate the C-H bond energy if heat of atomization of C₂H₆ is x kJ

Entropy decreases during

Find the correct statement about surface tension

1. SI unit is Nm^-1
2. The increase of temperature tends to decrease the surface tension
3. Work done per unit area is the surface energy
4. All of these

Select the incorrect statement

For the reaction, MCO₃(s) → MO(s) + CO₂(g); △H 82.8 kJ at 25°C, △E or △U at 25°C is

If 50 calories are added to a system and the system does work of 30 calories on surroundings then the change in internal energy of the system is

Find the incorrect relation for the irreversible adiabatic process from the following:

1. TV^Y-1 = constant
2. T^YP^1-Y- constant
3. PV^Y = constant
4. All of these

Bond dissociation enthalpy of H₂, Cl₂ and HCI are 434, 242 and 435 kJmol^-1 respectively. Enthalpy of formation of HCI is

1. 245 kJ mol^-1
2. 93 kJ mol^-1
3. -245 kJ mol^-1
4. -97 kJ mol^-1

Internal energy change (△U) when a monoatomic ideal gas is compressed reversibly from 16L to 2L at 300 K, is

The heat of formation of NH3(g) is - 46 kJ mol^-1 The AH (in kJ mol^-1) of the reaction 2NH₃(g) → N₂(g) + 3H₂(g) is

In reversible adiabatic expansion of an ideal gas

1. △S_sys = 0
2. △S_sys > 0
3. △S_sys < 0
4. Data insufficient

For vaporization of water at 1 atmospheric pressure, the values of △H and △S are 40.63 kJ mol^-1 and 108.8 JK-1mol^-1 respectively. The temperature, when Gibbs energy change (△G) for this transformation will be zero, is

The molar heat of formation of NH₄NO₃ (s) is - 367.5 kJ and those of N₂O(g) and H₂O(l) are +81.5 kJ and -286kJ respectively at 25°C and 1 atm. △U for decomposition of NH₄NO₃(s), into N₂O(g) and H₂O(l), is

The standard enthalpies of combustion of C₃H₆(l). C(graphite) and H₂(g) are respectively -3270, -394 and -286KJ respectively. The standard enthalpy of the formation of C₃H₆(l) in kJ mole^-1 is

For the reaction 2H₂ + O₂ → 2H₂O △H = -571 kJ mol^-1. Bond energies of H-H and O = O respectively are 435 and 498 kJ. Then average bond energy of the O-H bond will be (Approximately)

If 80 g NaOH reacts with 36.5 g HCI in dilute aqueous solution then the enthalpy of neutralisation is

What is the entropy change when 1 mole of a monoatomic ideal gas changes volume from 1L to 3L at constant temperature?

Which one of the following is a wrong statement?

1. △H_f^o for H⁺(aq) is taken as zero
2. The standard entropy of ethane is lower than that of methane
3. For same initial P, V, T, the final temperature is less in adiabatic reversible expansion as compared to adiabatic irreversible expansion considering the final volume as the same
4. For isothermal irreversible compression, △S_sys < 0

110J of heat are added to a gaseous system and its internal energy increases by 40J. The amount of workdone involved is

One mole of a monoatomic ideal gas at an initial temperature of T(K) does 6R joule of work adiabatically. The change in temperature is ((C_p/C_v) = 72)

The combustion of glucose takes place as
C₆H₁₂O₆ +6O₂ → 6CO₂+6H₂O, △H = x kcal mol^-1
The energy released by the combustion of 1.6g of glucose is -0.64 kcal. What is the value of x?

1. -80 kcal mol^-1
2. -72 kcal mol^-1
3. +72 kJ mol^-1
4. -108 kcal mol^-1

Heat of hydrogenation of cyclohexene is -x KJ. If the heat of hydrogenation of benzene is -z then what would be the resonance energy of benzene?

Calculate amount of work done when 2 mole of an ideal gas present in a vessel of 2L capacity at 1 atm pressure is allowed to enter into an evacuated vessel of 10L capacity

One mole of ideal gas is adiabatically and reversibly compressed to 1/4th of its original volume. Change in temperature of the gas if initial temperature is 27°C (given γ = 1.66)

Calculate the enthalpy change for the following reaction
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l)
Given enthalpies of formation of CH₄, CO₂ and H₂O are -74.8 kJ/mole, -393.5 kJ/mole and -286.2 kJ/mole respectively

On combustion carbon forms two oxide CO and CO₂ Heat of formation of CO₂ is -94.3 Kcal and that of CO is -26.0 Kcal. Heat of combustion of carbon is

For which of the following AH, is not zero ?

1. Br₂(e)
2. P₄(white)
3. C(diamond)
4. S₈(Rhombic)

The temperature at which the reaction
Ag₂O(s) 2Ag(s) + 1/2 O₂(g)
is at equilibrium is (Given, △H° 30.5 kJ/mole △S° 0.066 kJ/mole K^-1)

Which of the following statement is/are correct regarding third law of thermodynamics?

1. Third law of thermodynamics deals with entropy of perfect crystalline substance which is taken as zero at absolute zero temperature
2. The entropy of solid or liquid approaches zero at 0^oC
3. The residual entropy of CO is 5 JK^-1 mol^-1

The enthalpy of dissociation of CH₄(g) and C₂H₆(g) are 360 kcal and 620 kcal respectively. The bond energy of the C-C bond is

The difference between heat of reaction at constant pressure and constant volume for the reaction,
C(s) + 1/2O₂(g) --> CO₂(g) at 300 K is energies Given: R = 0.002 Kcal

A thin evacuated glass bulb of 100 mL capacity was there inside a 2-litre container at 27°C and 800 mm Hg pressure. If the bulb is broken isothermally, The new pressure in the container is

A gas at a pressure of 6 bar is heated from 0°C to 546°C and simultaneously compressed to half of its original volume. Final pressure is

The standard molar heat of formation of ethane, CO₂ (g) and H₂O(l), is respectively -21.1, -94.1 and-68.3 kcal mol^-1. The standard molar heat of , combustion (in kcal mol^-1) of ethane will be

If the standard heat of hydrogenation of but 1-ene is - x kJ/mole and that of Buta -1, 3-diene is -y kJ/mole, then the resonance energy of Buta-1, 3- diene is

The total entropy change for a reversible cyclic process

If a gas is contracted at constant temperature

One mole of gas occupying 2dm³ expands against a constant external pressure of 1.5 atm to a volume of 12 dm³. The work done is

1. -10 atm dm³
2. -15 atm dm³
3. -5 atm dm³
4. -18 atm dm³

Which of the following is correct for an ideal gas undergoing adiabatic expansion in a vacuum?

1. △U = 0
2. △T = 0
3. W = 0
4. All of these

The bond dissociation energy of C-H bond in CH₄ from given equation is
C(g) + 4H(g) → CH₄(g), △H = -397.8 kcal

Which of the following is correct for the adiabatic reversible process?

1. △S_sys = 0
2. △S_{sys >} 0
3. △S_{sys <} 0
4. △S_sys = 1

Select extensive property from the following

The enthalpy of combustion of solid benzoic acid at constant volume is - x kJ at 27°C, Its enthalpy of combustion (in kJ) at constant pressure will be

If 84 J of heat energy is given to a system and work done by the system is 5 cal, then the amount of internal energy change for the system will be