A compound containing xenon and fluorine was prepared by shining sunlight on a mixture of Xe (0.526 g) and excess F2 gas. If you isolate 0.678 g of the new compound, what is its empirical formula

In this case, according the law of conservation of mass, we can see that, since the total mass of the Xe-F compound is 0.678 g and that of xenon is 0.526 g, we have 0.152 g as the mass of reactants equal the mass of the products. It means that we can compute the moles of each atom in the compound as shown below:

[tex]n_{Xe}=0.526g/131.3g/mol=0.004mol\\\\n_F=0.152g/19.0g/mol=0.008mol[/tex]

Now we divide the moles of both reactants by the moles of xenon as those are the fewest ones in order to find their subscripts in the empirical formula:

[tex]Xe=0.004/0.004=1\\\\F=0.008/0.004=2[/tex]

Thus, the empirical formula is:

[tex]XeF_2[/tex]

Best regards!

bratislava bratislava · Answer 2 · 2022-01-20T12:03:02+01:00

The case kf the compound which consist of the xenon and the fluoride was made by shining the sunlight on a mixture of Xe and F2 gas.

As per the law of conservation of the mass, we can see that, as the total mass of the Xe-F compound is 0.678 g and that of xenon is 0.526 g,

Thus the 0.152 g as the mass of reactants equal the mass of the products. It means that we can compute the moles of each atom in the compound.

Learn more about the xenon and fluorine was prepared by.

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