Chemistry - Thermodynamics - Quiz-4

Point out the wrong statement in relation to enthalpy

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It is a state function
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It is an intensive property
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It is independent of the path followed for the change
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Its value depends upon the amount of substance in the system

Which of the following is zero for an isochoric process

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dP
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dV
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dT
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dE

Mark the correct statement

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For a chemical reaction to be feasible, ΔG should be zero
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Entropy is a measure of order in a system
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For a chemical reaction to be feasible, ΔG should be positive
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The total energy of an isolated system is constant

Internal energy is an example of [Pb. PMT 2000]

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Path function
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State function
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Both (1) and (2)
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None of these

The intensive property among these quantities is

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Enthalpy
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Mass/volume
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Mass
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Volume

Which of the following is not a state function?

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ΔS
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ΔG
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ΔH
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ΔQ

Which of the following is true for an adiabatic process [DCE 2002; MP PET 1995, 98, 2004; CPMT 1990; MP PMT 1998, 2002]

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ΔH = 0
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ΔW = 0
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ΔQ = 0
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ΔV = 0

Which of the following is not a state function

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Internal energy
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Enthalpy
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Work
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Entropy

Among them, intensive property is [AFMC 2004]

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Mass
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Volume
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Surface tension
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Enthalpy

First law of thermodynamics is the law of conservation of=

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Mass
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Linear momentum
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Energy
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Angular momentum

A mixture of two moles of carbon monoxide and one mole of oxygen, in a closed vessel is ignited to convert the carbon monoxide to carbon dioxide. If ΔH is the enthalpy change and ΔE is the change in internal energy, then

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ΔH > ΔE
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ΔH < ΔE
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ΔH = ΔE
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The relationship depends on the capacity of the vessel

The relation between ΔE and ΔH is [MP PET 1992; MP PMT 1996; MP PET/PMT 1998]

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$ΔH = ΔE - P ΔV$
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$ΔH = ΔE + P ΔV$
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$ΔE = ΔV + ΔH$
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$ΔE = ΔH + P ΔV$

At constant T and P, which one of the following statements is correct for the reaction, $CO (g) + \frac{1}{2} O_{2} (g) \to {CO}_{2} (g)$

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ΔH is independent of the physical state of the reactants of that compound
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ΔH > ΔE
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ΔH < ΔE
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ΔH = ΔE

For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter, ΔU and w correspond to

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$Δ U <0, w =0$
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$Δ U = 0, w < 0$
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$Δ U > 0, w = 0$
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$Δ U < 0, w > 0$

If ΔH is the change in enthalpy and ΔE the change in internal energy accompanying a gaseous reaction

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ΔH is always greater than ΔE
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ΔH < ΔE only if the number of moles of the products is greater than the number of the reactants
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ΔH is always less than ΔE
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ΔH < ΔE only if the number of moles of the products is less than the number of moles of the reactants

Enthalpy for the reaction C + O₂ → CO₂ is-

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Positive
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Negative
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Zero
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None

The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 liters to 20 liters at 25°C is -

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$- 2 .303 \times 298 \times 0 .082 \log 2$
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$- 298 \times 10^{7} \times 8 .31 \times 2 .303 \log 2$
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$2 .303 \times 298 \times 0 .082 \log 0 .5$
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$- 8 .31 \times 10^{7} \times 298 - 2 .303 \log 0 .5$

In a reversible isothermal process, the change in internal energy is-

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Zero
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Positive
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Negative
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None of the above

The enthalpy of neutralization of which of the following acids and bases is nearly –13.6 Kcal [Roorkee 1999]

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HCN and NaOH
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HCl and KOH
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HCl and HCN
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HCl and NH₄OH

Work done during isothermal expansion of one mole of an ideal gas from 10 atm to 1 atm at 300 K is (Gas constant = 2)

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938.8 cal.
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1138.8 cal.
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1381.8 cal.
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1581.8 cal.

Joule-Thomson expansion is [JIPMER 2000]

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Isobaric
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Isoenthalpic
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Isothermal
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None of these

In an adiabatic expansion of an ideal gas-

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W = –ΔE
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W = ΔE
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ΔE = 0
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W = 0

For the reaction

$C H_{3} C O O H (l) + 2 O_{2} (g) ⇌ 2 C O_{2} (g) + 2 H_{2} O (l)$

at 25°C and 1 atm. pressure, ΔH = –874 kJ. The change in internal energy (ΔE) is -

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– 874 kJ
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– 971.53 kJ
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+ 971.53 kJ
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+ 874 kJ

One mole of an ideal gas is allowed to expand freely and adiabatically into a vacuum until its volume has doubled. A statement that is not true concerning this expression is [Pb. PMT 1998]

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ΔH = 0
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ΔS = 0
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ΔE = 0
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W = 0

At 27°C, one mole of an ideal gas is compressed isothermally and reversibly from a pressure of 2 atm to 10 atm. The values of ΔE and q are (R = 2)

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0, – 965.84 cal
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– 965.84 cal, + 965.84 cal
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+ 865.58 cal, – 865.58 cal
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– 865.58 cal, – 865.58 cal

ΔE° of combustion of isobutylene is –X kJ mol^–1. The value of ΔH° is [DCE 2004]

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= ΔE°
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> ΔE°
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= 0
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< ΔE°

An ideal gas expands in volume from 1 × 10^–3 m³ to 1 × 10^–2 m³ at 300 K against a constant pressure of 1 × 10⁵ Nm^–2. The work done is [AIEEE 2004]

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270 kJ
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–900 kJ
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–900 J
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900 kJ

The spontaneous flow of heat is always

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From low to high pressure
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From high to high pressure
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Unidirectional from lower temperature to higher temperature
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Unidirectional from the higher to lower temperature

The mixing of non-reacting gases is generally accompanied by

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Decrease in entropy
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Increase in entropy
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Change in enthalpy
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Change in free energy

An irreversible process occuring isothermally in an isolated system leads to

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Zero entropy
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An increase in the total entropy of the system
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A decrease in the total entropy of the system
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None of these

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Practice Chemistry Quiz Questions and Answers

0:0:1

Practice Chemistry Quiz Questions and Answers

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