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ओक्सीकरण में इलेक्ट्रॉन की हानि होती है।
False
रिडक्शन में इलेक्ट्रॉन प्राप्ति के समर्थन का अर्थ होता है।
False
एलेक्ट्रोकैमिस्ट्री में, एक पूरे रासायनिक-विद्युत प्रक्रिया में, दो समाधानों के प्रतिपक्ष होते हैं।
False
गैल्वेनिक सेल में, एक अंतर्गत बैटरी प्राणित होती है।
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एलेक्ट्रोलिटिक सेल में, एक बाह्य वोल्टेज स्रोत लागू होता है।
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फैरेडे का नियम विद्युत से भार और मात्रा का संबंध स्थापित करता है।
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इलेक्ट्रोकेमिस्ट्री के क्षेत्र में बैटरी, करोड़ संरक्षण, सेंसर्स, ईंधन सेल्स, और इलेक्ट्रोप्लेटिंग के अनुप्रयोग होते हैं।
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मैटेरियल साइंस और इंजीनियरिंग में हुए विकास से इलेक्ट्रोकेमिस्ट्री के संदर्भ में कोई सीमाएँ रही हैं।
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साइक्लिक वोल्टामेट्री, पोटेंशिओमेट्रिक टाइट्रेशन, और इम्पीडेंस स्पेक्ट्रोस्कोपी के माध्यम से पर्यावरण शोध, कला संरक्षण, और पारमाध्यानिक विश्लेषण में महत्वपूर्ण भूमिका है।
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मौर्खता, किनेटिक्स, और इंटरफेसिअल प्रक्रियाओं के संकेतन में कुछ महत्ापूप्ुपुन््पु पि््ुपुप्ुप्ुप्ुप्ुप््ुप्ुप्ुप्ुप्ुप्ुप्ुप्ुप्ुप्ुक्, 'नि््ुन्'्पुप्ुन्।
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Study Notes
Rasayan Shastra Class 12: Exploring Electrochemistry
The final year of secondary education in India, commonly known as class 12, introduces students to advanced sciences, one of which is Rasayan Shastras encompassing chemistry. This comprehensive section delves into electrochemistry—the interdisciplinary science focused on electrical energy conversion through chemical redox reactions.
Fundamentals of Redox Reactions
Electrochemical processes often involve reduction and oxidation reactions (redox) occurring simultaneously when electrons flow between two half-reactions driven by an external electric potential difference. Oxidation is defined as a loss of electrons while reduction refers to gaining electrons; these processes must occur together during redox reactions, with the sum of their balanced equations equaling zero.
Half-Reactions and Cell Potentials
In an electrochemical cell, there exist two half-cells, each containing its own half-reaction. These half-reactions have standard cell potentials associated with them, determined using the Nernst equation and standard conditions. A galvanic cell results from combining both half-cells' reaction products to form a complete chemical-electrical process resulting in current production. Conversely, an electrolytic cell applies an external voltage source causing non-spontaneous redox reactions to proceed.
Faraday’s Law and Stoichiometry
Faraday's law relates electricity to mass and establishes the relationship between current and the amount of substance undergoing redox reactions. This concept allows us to calculate quantities like moles of electrons transferred (called charge), limiting current, and efficiency of electrochemical devices.
Applications of Electrochemistry
Electrochemistry finds applications in various fields such as batteries, corrosion protection, sensors, fuel cells, and electroplating due to its ability to facilitate practical large-scale energy storage, conversion, and utilization technologies. Additionally, it plays vital roles in environmental remediation, art conservation, and biochemical analysis through techniques such as cyclic voltammetry, potentiometric titrations, and impedance spectroscopy.
Challenges and Future Prospects
Despite significant progress made in recent decades, gaps still remain in our fundamental understanding of some critical aspects of electrochemistry, including charge transfer mechanisms, kinetics, and interfacial phenomena. Developments in materials science and engineering will undoubtedly contribute to overcoming these challenges and drive innovation in new electrochemical systems for efficient and sustainable energy supply solutions.
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Description
Explore the intricate world of electrochemistry in this quiz focused on redox reactions, half-reactions, cell potentials, Faraday's law, and applications of electrochemistry. Dive into the fundamentals and challenges of this interdisciplinary field.
