Post-Module Assess. #14

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Grace Lee 3G
Posts: 19
Joined: Fri Sep 29, 2017 7:07 am

Post-Module Assess. #14

Postby Grace Lee 3G » Mon Nov 06, 2017 9:30 pm

339.20 g of a cobalt metal is reacted with fluorine gas to produce 996.08 g of a compound. What is the empirical formula of the new compound?

How do I solve this?

sandros
Posts: 19
Joined: Fri Sep 29, 2017 7:07 am

Re: Post-Module Assess. #14

Postby sandros » Mon Nov 06, 2017 9:40 pm

First you find the mass percentage of each element given that you already have the total mass

Then you imagine that the sample mass is 100g and you can then transform your percentages into actual masses (in grams)

Once you transform these percentages, you divide the mass of each atom by its molar mass so that you can obtain the number of mole(s) of each atom

Then you divide all of these numbers by the smallest number

Finally multiply them all by a number that you have to figure out on your own in order to have whole numbers of atoms (approximately).

Grace Lee 3G
Posts: 19
Joined: Fri Sep 29, 2017 7:07 am

Re: Post-Module Assess. #14

Postby Grace Lee 3G » Mon Nov 06, 2017 11:07 pm

Thanks!


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