Chemical Kinetics

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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

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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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The energy possessed by the reacting species increases as the temperature rises, the pace of a reaction increases. This raises the temperature and raises the average kinetic energy of the reactant molecules

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The reaction's activation energy is relatively high at room temperature and not readily available, the reaction is highly viable. H₂ (g) and O₂ (g)bond break and clash, allowing particles to pass across the energy barrier.

2H_2&n

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A. The reaction has a zero order. The concentration of the reactants does not change with time in a zero order reaction, and the rate of concentration remains constant

B. Slope of the curve is  - k

C. The rate constant's uni

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The concentration of the reactants does not change with time in a zero -order reaction, and the rate of concentration remains constant. The molecularity of a reaction cannot be 0 because it indicates the number of reactants involved

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When the Threshold energy is less than the energy of the molecules and the orientation of the molecules is proper for the effective collision, the reaction happens. As a result, the reaction is slow, and the number of effective coll

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The number of ions or atoms that collide to react is known as molecularity in an elementary reaction. The order of reaction about B should be 1 if this is an elementary reaction, however the rate law given is $\frac{3}{2}$

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The concentration of the reactants does not change with time in a zero- order reaction, and the rate of concentration remains constant.

R= [R]₀ – Kt

Kt = [R]₀

t = $\frac{\left. [\mathrm{R}\right]{}_0}{\mathrm{K}}$