Acarbonatomhasarelativeatomicmassof13.2.60%ofthecarbonatomhasamassnumberof12.4.30%ofthecarbonatomshaveamassnumberof13.7,whilsttheremaining10%haveamassnumberwhichisnotknown.Calculatethemassnumberofthecarbonisotopewhichis10%oftheCarbon13.2atom.Giveyouranswerto1decimalplace,ifneeded.

The question seems to be asking for the mass number of the carbon isotope that makes up 10% of the carbon atom, given that the relative atomic mass of the carbon atom is 13.2, 60% of the carbon atom has a mass number of 12.4, and 30% of the carbon atom has a mass number of 13.7. The mass number of the remaining 10% is unknown and is what we're trying to find.

Here's how you can calculate it:

1. First, understand that the relative atomic mass of an element is the weighted average of the mass numbers of its isotopes. The weights are the relative abundances of the isotopes.

2. The relative atomic mass of the carbon atom is given as 13.2. This is calculated as follows:

   (0.60 * 12.4) + (0.30 * 13.7) + (0.10 * x) = 13.2

   where x is the mass number of the unknown isotope.

3. You can now solve this equation for x:

   7.44 + 4.11 + 0.10x = 13.2 0.10x = 13.2 - 7.44 - 4.11 0.10x = 1.65 x = 1.65 / 0.10 x = 16.5

So, the mass number of the carbon isotope that makes up 10% of the carbon atom is 16.5.