-0.0039 g
-0.16 g
-6.3 g
-250 g
I think it's 6.3 but i'm not sure..
thank you :)
Update:How many moles of chlorine (Cl) atoms are in a sample of 1.72 × 1022 atoms?
0.0286 mol Cl
35.0 mol Cl
1.03 × 1023 mol Cl
1.04 × 1046 mol Cl
I also am having problems with this one..
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Answers & Comments
Verified answer
Hello, Christina. Let's see if I can help you a bit with your questions.
#1). You are given a number of Argon atoms, 3.8x10^24 actually, and are told to determine their mass, in grams, but there isn't a balance. What to do?
You know a mole contains 6.022x10^23 atoms.
You know, from your Periodic Table, Ar has a mass of 39.948 g/mol.
You know you were given more than 1mol Ar, as, 3.8x10^24 > 6.022x10^23.
To solve this question divide 3.8x10^24 by 6.022x10^23 = 6.31 mols Ar are present. Multiply this 6.31 by 39.948 = 252.07188 grams Ar are in the sample. As the least precise, and only, measurement given contains 2 sigfigs the answer can only contain 2 digits. The correct answer is 250 grams.
#2). You can solve this in the same manner. As 1.72x10^22 atoms are less than the 6.022x10^23 required to constitute a mole the answer will be less than a mole. Divide 1.72x10^22 by 6.022x10^23 = 0.02856, in sigfigs 0.0286 mol Cl.
That wasn't so very difficult, Christina, now was it.
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divide 3.8 * 10^24 atoms by 6.022x10^23 (avogadro's number) to get moles and then multiply by the MM of Argon to get grams...
Part B
Divide 1.72 * 10^22 atoms by avogadro's number to get moles.