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The atomic mass of carbon can be calculated using the following information: Natural carbon is a mixture of three isotopes: 12^C, 13^C and 14^C. The carbon atoms are 98.59% of the isotope: 12^C, 1.11% of the isotope 13^C and <0.01% of the isotope 14^C. It has been decided that the atomic mass of the lightest carbon isotope should be exactly 12 u. Then the atomic masses of the two other isotopes will be 13.0034 u and 14.0032 u respectively. To calculate the atomic mass of carbon, we need to determine the total mass of 10,000 atoms of natural carbon. To do this, we can use the following steps: 1. Calculate the mass of 10,000 atoms of the 12^C isotope: Since the 12^C isotope is the most abundant isotope in natural carbon, we can calculate its mass by multiplying the mass of a single atom of 12^C by the number of atoms present: (12 u) x (10,000 atoms) = 120,000 u. 2. Calculate the mass of 10,000 atoms of the 13^C isotope: We can do this in a similar way, by multiplying the mass...

The C--O bond in phenol is shorter than the C--O bond in ethanol due to the presence of the aromatic ring in phenol. In an aromatic compound such as phenol, the electrons in the aromatic ring are delocalized, meaning that they are spread out over the entire ring rather than being concentrated in a single bond. This delocalization of electrons allows the atoms in the aromatic ring to be more stable, resulting in a shorter bond length. In contrast, the C--O bond in ethanol is a regular covalent bond, with the electrons concentrated in the bond between the carbon and oxygen atoms. As a result, the C--O bond in ethanol is longer than the C--O bond in phenol. The shorter bond length of the C--O bond in phenol has important implications for the chemical properties of the compound. For example, the shorter bond length allows the oxygen atom in phenol to form stronger hydrogen bonds with other molecules, which contributes to the high solubility of phenol in water. In summary, the C--O bond in ...