Question

calculate the moles of oxygen (atoms) in 10.0 g of aluminum sulfate. then calculate the oxygen atoms in 10.0 g of aluminum sulfate. the molar mass was calculated as 342.15 g first convert 10.0 g into moles as we did previously: (10.0 g as)(1 mol as/_2_g as) = _1_mol as then convert moles as into moles of o using the formula al₂(so₄)₃ that gives 1 mol as = 12 mol o (_4_mol as)(_3_mol o/_6_mol as) = _5_mol o finally convert moles of oxygen into atoms of oxygen using 1 mol = 6.022 x 10²³ things (_8_mol o)(_7_atoms o/_10_mol o) = _9_atoms a. 0 b. 1 c. 2 d. 3 e. 4 f. 342.15 g. 10.0 h. 12 i. 56.1 j. 0.0292274 k. 0.350728 l. 6.022 x 10²³ m 1.76 x 10²³ n 4.85 x 10²⁶ o 1.76 x 10²⁴ p 2.11 x 10²³

Explanation:

Step1: Convert grams to moles

Using the formula \(n=\frac{m}{M}\), where \(n\) is the number of moles, \(m\) is the mass, and \(M\) is the molar mass. For converting \(10.0\) g of aluminum sulfate (\(AS\)) to moles: \((10.0\space g\space AS)\times(\frac{1\space mol\space AS}{342.15\space g\space AS})\). So, blank 1 is \(J(0.0292274)\) (since \(n=\frac{10.0}{342.15}\approx0.0292274\)), blank 2 is \(F(342.15)\).

Step2: Convert moles of \(AS\) to moles of \(O\)

Given \(1\space mol\space AS = 12\space mol\space O\). So, \((0.0292274\space mol\space AS)\times(\frac{12\space mol\space O}{1\space mol\space AS})\). Blank 3 is \(H(12)\), blank 4 is \(J(0.0292274)\), blank 5 is \(K(0.350728)\) (since \(0.0292274\times12 = 0.3507288\approx0.350728\)), blank 6 is \(B(1)\).

Step3: Convert moles of \(O\) to atoms of \(O\)

Using \(N = n\times N_{A}\), where \(N\) is the number of atoms, \(n\) is the number of moles, and \(N_{A}=6.022\times 10^{23}\space mol^{- 1}\). So, \((0.350728\space mol\space O)\times(\frac{6.022\times 10^{23}\space atoms\space O}{1\space mol\space O})\). Blank 7 is \(L(6.022\times 10^{23})\), blank 8 is \(K(0.350728)\), blank 9 is \(M(2.11\times 10^{23})\) (since \(0.350728\times6.022\times 10^{23}\approx2.11\times 10^{23}\)), blank 10 is \(B(1)\).

Answer:

1. \(J.0.0292274\)
2. \(F.342.15\)
3. \(H.12\)
4. \(J.0.0292274\)
5. \(K.0.350728\)
6. \(B.1\)
7. \(L.6.022\times 10^{23}\)
8. \(K.0.350728\)
9. \(M.2.11\times 10^{23}\)
10. \(B.1\)