SO2+O2 SO3 how many moles of O2 needed to combust 100.0g of sulfur dioxide

Chemistry

1 answer:

Oksanka [162]3 years ago

6 0

2SO2 + O2 ------> 2SO3

1) M(SO2)= 32.0 + 2*16.0 = 64 g/mol

2) 100.0 g SO2 * 1 mol SO2/64 g SO2 = 1.5625 mol SO2

3) 2SO2 + O2 ------> 2SO3

2 mol 1 mol

1.5625 mol x mol

x= 1.5625/2=0.78125 ≈ 0.7813 mol O2

Answer: 0.7813 mol O2.

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Answer:

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Answer:

$\rm S^{2-}$ .

Explanation:

Based on the electron configuration of this ion, count the number of electrons in this ion in total:

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Each electron has a charge of $(-1)$ .

Atoms are neutral and have $0$ charge. However, when an atom gains one extra electron, it becomes an ion with a charge of $(-1)$ . Likewise, when that ion gains another electron, the charge on this ion would become $(-2)$ .

The ion in this question has a charge of $(-2)$ . In other words, this ion is formed after its corresponding atom gains two extra electrons. This ion has $18$ electrons in total. Therefore, the atom would have initially contained $18 - 2 = 16$ electrons. The atomic number of this atom would be $16$ .

Refer to a modern copy of the periodic table. The element with an atomic number of $16$ is sulphur with atomic symbol $\rm S$ . To denote the ion, place the charge written backwards (" $2-$ " for a charge of $(-2)$ ) as the superscript of the atomic symbol: