For molecules of comparable mass, why are dipole-dipole forces stronger than dispersion forces?

1 answer:

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Dispersion forces, otherwise known as induced dipole-induced dipole interactions, polarize a molecule slightly into weak negative and weak positive charges. Then coulombs law dictates their electrostatic attractions. However, in dipole-dipole, these molecules are already polarized permanently and typically of a much larger magnitude than an induced dipole for a molecule of the same molar mass. This means that the electrostatic attractions are significantly stronger than the London Dispersion force's.

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The second-order rate constant for the dimerization of a protein (P) P + P → P2 is 6.2 × 10−3/M · s at 25°C. Part 1 out of 2 If

siniylev [52]

Answer:

$r=1.59\times 10^{-10}\ M/s$

Explanation:

According to the law of mass action:-

The rate of the reaction is directly proportional to the active concentration of the reactant which each are raised to the experimentally determined coefficients which are known as orders. The rate is determined by the slowest step in the reaction mechanics.

Order of in the mass action law is the coefficient which is raised to the active concentration of the reactants. It is experimentally determined and can be zero, positive negative or fractional.

The order of the whole reaction is the sum of the order of each reactant which is raised to its power in the rate law.

From the reaction given that:-

$P+P\rightarrown P_2$