The forward reaction is exothermic because ΔH = −94 kJ/mol, meaning heat is released during the formation of SO₃.
Increasing temperature shifts the equilibrium towards SO₂ and O₂, reducing the equilibrium constant Kp.
According to Le Chatelier’s principle, increasing pressure shifts the equilibrium towards SO₃ because the product side has fewer moles of gas (2 moles) than the reactant side (3 moles).
A catalyst speeds up both forward and reverse reactions equally.
It does not change the equilibrium constant or the equilibrium yield of SO₃.
اس بیان کے مطابق کہ ہائیڈروجن سے اوپر موجود الیکٹروڈز کا پوٹینشل منفی ہوتا ہے اور وہ ہائیڈروجن کے مقابلے میں الیکٹران زیادہ آسانی سے خارج کرتے ہیں، ہائیڈروجن کس طرح کام کرتی ہے؟
Metals above hydrogen in the electrochemical series generally have more negative standard reduction potentials and tend to lose electrons more readily than hydrogen.
Hydrogen acts as the cathode when it gains electrons and undergoes reduction in a galvanic cell where such a metal acts as the anode.
The metal above hydrogen acts as the anode and as the reducing agent because it loses electrons and reduces another substance.
Electrochemistry is the branch of chemistry that studies the relationship between electrical energy and chemical energy, including their interconversion.
It deals with electrochemical cells, batteries, electrolysis, and oxidation-reduction (redox) reactions.
Galvanic cells convert chemical energy into electrical energy.
Electrolytic cells use electrical energy to drive chemical reactions.
