What is the mass of #7.83 * 10^23# atoms Cl?

Answer 1

Slightly over 35.5 grams.

I inevitably have 35.45 g of chlorine if I know Avogadro's number of chlorine atoms.

Here we have a number that is in excess of Avogadro's number, #6.022xx10^(23)# #=# #N_A#.

Since I know that if I have #6.022xx10^(23)# atoms of chlorine I have a mass of #35.45# #g# of chlorine, then all I have to do is give the product, #35.45*g# #xx(7.83xx10^(23))/(6.022xx10^(23))# #=# #??# #g#.

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Answer 2

Naomi Aronson

To find the mass of 7.83 * 10^23 atoms of Cl, you can use the molar mass of chlorine, which is approximately 35.45 g/mol. Multiply the number of atoms by the molar mass to get the mass:

(7.83 \times 10^{23} \text{ atoms} \times \frac{1 \text{ mol}}{6.022 \times 10^{23} \text{ atoms}} \times 35.45 \text{ g/mol} = 456.63 \text{ grams})

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.