JEE Main Physical Chemistry — Energetics & Equilibrium – Topic Test
JEE Main Physical Chemistry — Energetics & Equilibrium – Topic Test is an online topic test in the JEE Main pattern, covering Physical Chemistry — Energetics & Equilibrium. Attempt it on SeatBeat with a timer like the real exam, then see a detailed solution for every question and your score and weak-topic analysis.
Topics in this test
| Topic | Questions |
|---|---|
| Physical Chemistry — Energetics & Equilibrium | 30 |
Difficulty: 15 medium · 15 hard
Physical Chemistry — Energetics & Equilibrium MCQ questions with answers
The first 3 of 30 questions. Unlock the series for the rest, each with a solution.
Q1. Which one of the following species does NOT have a standard enthalpy of formation equal to zero at 298 K?
निम्नलिखित में से किस एक स्पीशीज़ की 298 K पर मानक संभवन एन्थैल्पी शून्य के बराबर नहीं है?
- A. Br₂(l)
- B. Hg(l)
- C. Br₂(g)
- D. N₂(g)
Solution
The reference form of bromine at 298 K is liquid Br₂, so ΔfH° of Br₂(g) is not zero (it equals the enthalpy of vaporization, about +31 kJ mol⁻¹), whereas Br₂(l), Hg(l) and N₂(g) are the stable standard-state forms of their elements and are assigned zero.
298 K पर ब्रोमीन का संदर्भ रूप द्रव Br₂ है, अतः Br₂(g) की ΔfH° शून्य नहीं है (यह वाष्पन एन्थैल्पी के बराबर है, लगभग +31 kJ mol⁻¹), जबकि Br₂(l), Hg(l) और N₂(g) अपने तत्वों के स्थायी मानक-अवस्था रूप हैं और इन्हें शून्य मान दिया जाता है।
Q2. For a certain reaction ΔH = +30 kJ mol⁻¹ and ΔS = +100 J K⁻¹ mol⁻¹, both assumed independent of temperature. The reaction becomes spontaneous:
एक निश्चित अभिक्रिया के लिए ΔH = +30 kJ mol⁻¹ और ΔS = +100 J K⁻¹ mol⁻¹, दोनों को तापमान से स्वतंत्र माना गया है। यह अभिक्रिया स्वतः प्रवर्तित (spontaneous) हो जाती है:
- A. below 300 K / 300 K से नीचे
- B. at no temperature / किसी भी तापमान पर नहीं
- C. above 300 K / 300 K से ऊपर
- D. at all temperatures / सभी तापमानों पर
Solution
With ΔH > 0 and ΔS > 0, ΔG = ΔH − TΔS becomes negative only above T = ΔH/ΔS = 30000/100 = 300 K. Hence the reaction is spontaneous above 300 K.
ΔH > 0 और ΔS > 0 होने पर, ΔG = ΔH − TΔS केवल T = ΔH/ΔS = 30000/100 = 300 K से ऊपर ही ऋणात्मक होता है। अतः अभिक्रिया 300 K से ऊपर स्वतः प्रवर्तित होती है।
Q3. Among the following thermodynamic quantities, which one is the odd one out?
निम्नलिखित ऊष्मागतिक राशियों में से कौन-सी एक भिन्न (odd one out) है?
- A. Internal energy / आंतरिक ऊर्जा
- B. Enthalpy / एन्थैल्पी
- C. Heat / ऊष्मा
- D. Entropy / एन्ट्रॉपी
Solution
Internal energy, enthalpy and entropy are state functions (depend only on state). Heat is a path function, so it is the odd one out.
आंतरिक ऊर्जा, एन्थैल्पी और एन्ट्रॉपी अवस्था फलन (state function) हैं (केवल अवस्था पर निर्भर करती हैं)। ऊष्मा एक पथ फलन (path function) है, अतः यही भिन्न है।
Frequently asked questions
How many questions are in the JEE Main Physical Chemistry — Energetics & Equilibrium – Topic Test?
30 questions for 30 marks, to be answered in 30 minutes.
Is there negative marking in the JEE Main Physical Chemistry — Energetics & Equilibrium – Topic Test?
Yes — 0.25 marks are deducted for each wrong answer, as in the real exam pattern.
Which topics does the JEE Main Physical Chemistry — Energetics & Equilibrium – Topic Test cover?
Physical Chemistry — Energetics & Equilibrium (30 questions).
Is the JEE Main Physical Chemistry — Energetics & Equilibrium – Topic Test free?
It is part of the JEE Main 2027 Mock Test Series (104 tests, ₹299). You can first try Basic Concepts & Atomic Structure – Topic Test for free.
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