At 25°C (298 K), (2.303RT/F) = (2.303 × 8.314 × 298)/96485 ≈ 0.0592 V. This is commonly used in half-cell potential calculations.
All colligative properties (boiling point elevation, freezing point depression, osmotic pressure, and vapor pressure lowering) depend only on the number of solute particles, not their nature.
In a galvanic cell, the anode is where oxidation occurs and is the negative electrode. Electrons flow from anode to cathode through the external circuit.
pH = -log[H⁺] = -log(10⁻⁴) = 4. At 25°C, pH + pOH = 14, so pOH = 14 - 4 = 10.
A catalyst speeds up both forward and reverse reactions equally, so it does not change the position of equilibrium. It only helps the system reach equilibrium faster.
Equivalent moles of strong acid and strong base neutralize completely. The salt NaCl formed doesn't hydrolyze. pH = 7
For first-order reaction: t₁/₂ = 0.693/k = 0.693/0.693 = 1 min
Using Charles's Law: V₁/T₁ = V₂/T₂ → V₂ = V₁ × (T₂/T₁) = 22.4 × (546/273) = 44.8 L
Daniell cell is a primary cell (non-rechargeable). Others are secondary (rechargeable) cells.
Increasing pressure favors the side with fewer moles of gas. 1 mole N₂O₄ ⇌ 2 moles NO₂. Equilibrium shifts left.