Ncert Solutions Chemistry Class 12th

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The pace of any reaction is determined by the concentration of the reactants, the rate of any reaction generally declines during the reaction. As the reaction progresses, the reactant concentration declines, and the product concentration rises.

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Ans: Acetic acid is a weak electrolyte and the number of ions on dilution increases due to an increase in the degree of dissociation. In the case of strong electrolytes the number of ions remains the same but interionic attraction decreases.

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Ans: The cell reaction of a lead storage battery is as follows;

Pb + PbO₂ + 2H₂SO₄→2H₂SO₄ + 2H₂O

The density of electrolytes changes because water is formed and sulphuric acid is consumed as a product during discharge of the battery

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The chance of more than three molecules meeting at the same time is extremely minimal, reactions with molecularity more than three are extremely rare. Simultaneous collisions decrease as the number grows, the probability is very low, and more than three reactions with molecularity are uncommon.

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Ans: Primary batteries contain a limited amount of reactants and once consumed are discharged. Secondary batteries take a long time to recharge. Fuel cells run continuously as long as reactants are supplied to them and products are consumed

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The activation energy for fuel combustion reactions is very large, and because every substance or element requires an ignition temperature to function and excite to a higher temperature, oxygen in air does not combust to fire.

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Ans: The reactions taking place in the Daniel cell is as follows;

Zn⁺ + Cu²⁺ → Zn²⁺ + Cu

The number of electrons involved in two. The Nernst equation is as follows;

E_{cell =} E $°$ _cell - $\frac{-0.059}{2}$  log $\frac{\left[Z{n^2}^{+}\right]}{\left[C{u^2}^{+}\right]}$

From the above equation, we conclude that increasing the concentration of Zn^2+, E_cell will decrease.

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Ans: The given cell reaction consists of two half cell reactions represented below as follows;

At anode: Cu→Cu²⁺+ 2e⁻

At cathode: Cl² + 2e⁻ →2Cl⁻

Here oxidation of copper and reduction of chlorine is taking place