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Q. No.If bond enthalpies of \(C-C,C-H,O=O,C=O \) and \(O-H \) are
a, b, c, d, and e respectively, then the heat of combustion of ethane will be:
1. \(6 b+\frac{7}{2} c+a-2 d-3e \)
2. \(b+c+a-4 d-3e \)
3. \(6 b+\frac{7}{2} c+a-4 d-6e \)
4. \(6 b+7 c+a-4 d-6e \)
Subtopic: Thermochemistry |
77%
From NCERT
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| Statement I: | ∆S total i.e., ∆Ssys + ∆Ssurr is zero for the irreversible process. |
| Statement II: | Total entropy change for the system and surrounding of a spontaneous process is zero. |
| 1. | Statement I is False but Statement II is True. |
| 2. | Both Statement I and Statement II are True. |
| 3. | Both Statement I and Statement II are False. |
| 4. | Statement I is True but Statement II is False. |
Subtopic: Spontaneity & Entropy |
54%
From NCERT
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1 mol of monoatomic ideal gas expanded adiabatically against a constant pressure of 2 atm from 10L to 20L. The correct option for the above process is:
1. q = 20 L-atm
2. \(\Delta U = 0 \)
3. \(\Delta U = -20 ~\text L~\text {atm} \)
4. \(\text w = 10 ~\text L~ \text {atm} \)
1. q = 20 L-atm
2. \(\Delta U = 0 \)
3. \(\Delta U = -20 ~\text L~\text {atm} \)
4. \(\text w = 10 ~\text L~ \text {atm} \)
Subtopic: First Law of Thermodynamics |
82%
From NCERT
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A system is taken from state \(a\) to state \(c\) by two paths \(adc\) and \(abc\) as shown in the figure. The internal energy at \(a\) is \({U}_{a}=10~\text{J}.\) Along the path \(adc\) the amount of heat absorbed \(\delta Q_1=50~\text{J}\) and the work obtained \(\delta W_1=20~\text{J}\) whereas along the path \(abc\) the heat absorbed \(\delta Q_2 = 36~\text{J}.\) The amount of work along the path \(abc\) is:
| 1. | \(10~\text{J}\) | 2. | \(12~\text{J}\) |
| 3. | \(36~\text{J}\) | 4. | \(6~\text{J}\) |
Subtopic: First Law of Thermodynamics |
81%
From NCERT
NEET - 2013
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Which of the following relations does not give the equation of an adiabatic process, where terms have their usual meaning?
1. \({P}^{1-\gamma}{T}^{\gamma}= \text{constant}\)
2. \({PV}^{\gamma}=\text{constant}\)
3. \({TV}^{\gamma-1}= \text{constant}\)
4. \({P}^{\gamma} {T}^{1-\gamma}=\text{constant}\)
1. \({P}^{1-\gamma}{T}^{\gamma}= \text{constant}\)
2. \({PV}^{\gamma}=\text{constant}\)
3. \({TV}^{\gamma-1}= \text{constant}\)
4. \({P}^{\gamma} {T}^{1-\gamma}=\text{constant}\)
Subtopic: Types of Processes |
77%
From NCERT
NEET - 2013
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For \(\Delta G <0 \) , a reaction is spontaneous only if :
| 1. | Pressure is constant. |
| 2. | Temperature is constant. |
| 3. | Both pressure and temperature are constant. |
| 4. | Both temperature and volume are constant. |
Subtopic: Spontaneity & Entropy |
57%
From NCERT
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3 moles of helium gas at 1 bar is compressed reversibly and isothermally at 400 K to 10 bar pressure. The work done (in J) on the system is: (Given: \(R= 8.314 ~J K^{-1}~ mol^{-1}\) )
| 1. | \(2.29 \times 10^4 \) | 2. | \(2.29 \times 10^{-4} \) |
| 3. | \(-2.29 \times 10^4 \) | 4. | \(-2.29 \times 10^{-4} \) |
Subtopic: First Law of Thermodynamics |
58%
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An ideal gas follows a process described by the equation \(PV^2=C\) from the initial \((P_1, V_1, T_1)\) to final \((P_2, V_2, T_2)\) thermodynamics states, where \(C\) is a constant. Then:
| 1. | \(\text{If}~P_1>P_2~\text{then}~T_1<T_2\) |
| 2. | \(\text{If}~V_2>V_1~\text{then}~T_2>T_1\) |
| 3. | \(\text{If}~V_2>V_1~\text{then}~T_2<T_1\) |
| 4. | \(\text{If}~P_1>P_2~\text{then}~V_1>V_2\) |
Subtopic: Types of Processes |
From NCERT
NEET - 2022
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Identify correct match using Column I & Column II
| Column I | Column II | ||
| (i) | Spontaneous process | (a) | Isothermal and isobaric process |
| (ii) | \(\Delta H^\circ\) | (b) | \(\Delta H<0 \) |
| (iii) | \(\Delta T=0, \Delta P=0 \) | (c) | \(\Delta G<0 \) |
| (iv) | Exothermic process | (d) | (Bond energy of reactant) - (Bond energy of product) |
| I | II | III | IV | |
| 1. | c | d | a | b |
| 2. | b | a | c | d |
| 3. | d | b | c | d |
| 4. | a | d | b | c |
Subtopic: First Law of Thermodynamics | Spontaneity & Entropy | Gibbs Energy Change |
94%
From NCERT
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An ideal gas undergoes four different processes from the same initial state as shown in the figure below. Those processes are adiabatic, isothermal, isobaric, and isochoric. The curve which represents the adiabatic process among \(1,\) \(2,\) \(3\) and \(4\) is:
| 1. | \(4\) | 2. | \(1\) |
| 3. | \(2\) | 4. | \(3\) |
Subtopic: Types of Processes |
78%
From NCERT
NEET - 2022
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