Use the bond dissociation energies of H2 (435 kJ/mol) and of a typical carbon–carbon bond (347 kJ/mol) to decide which bond is stronger. Explain your reasoning.

H2 bond is stronger

Explanation:

In this question, we are trying to make a connection between bond dissociation energy and the strength of a bond.

First of all, we must know that any bond that is quite stable must have a large bond dissociation energy. This means that more energy is supplied in order to cleave the bond.

A high bond dissociation energy actually implies that a bond is of low energy and consequently stable.

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally