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3 years ago

Toxic Cr(VI) can be precipitated from an aqueous solution by bubbling SO2 through the

Chemistry

1 answer:

gavmur [86]3 years ago

3 0

Answer:

2.48 × 10⁴ mol

Explanation:

Step 1: Write the balanced equation

2 CrO₄²⁻ + 3 SO₂ + 4 H⁺ ⇒ Cr₂(SO₄)₃ + 2 H₂O

Step 2: Calculate the reacting moles of CrO₄²⁻

3.00 × 10⁸ L of 5.50 × 10⁻² mM CrO₄²⁻ react. The reacting moles are:

3.00 × 10⁸ L × 5.50 × 10⁻² × 10⁻³ mol/L = 1.65 × 10⁴ mol

Step 3: Calculate the reacting moles of SO₂

The molar ratio of CrO₄²⁻ to SO₂ is 2:3. The reacting moles of SO₂ are 3/2 × 1.65 × 10⁴ mol = 2.48 × 10⁴ mol.

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3 years ago

6. What is the oxidation number for the atom indicated in the following compounds.

Hatshy [7]

Answer:

a. +6;

b. +5;

c. +3.

Explanation:

Start with elements with well-known oxidation states.

The oxidation state on oxygen O in compounds is mostly -2. Common exceptions include:

-1 in peroxides and
positive when oxygen bonds to fluorine.

The oxidation state on group 1 metals (Li, Na, K, etc.) in compounds is mostly +1.

The oxidation state on group 2 metals (Be, Mg, Ca, etc.) in compounds is mostly +2.

Barium Ba is a group 2 metal. The oxidation state on Ba in the compound BaSO₄ is expected to be +2.

The oxidation state on hydrogen H in compounds is mostly +1. The oxidation state on H might be negative when it is bonded to metals.

The oxidation state on halogens (F, Cl, Br, etc.) is mostly -1. The oxidation state may vary when the halogen is bonded to oxygen or another halogen element.

Compounds are neutral. The oxidation state on all atoms in a compound shall add up to 0. Both BaSO₄ and HClO₂ are neutral.

Oxidation states:

Ba: +2;
The oxidation state on sulfur S is to be determined;
O: -2.

Let the oxidation state on S be x.

2 + x + 4 × (-2) = 0;

x = 6.

Hence, the oxidation state on S in BaSO₄ is +6.

Oxidation states:

H: +1;
Cl here is bonded to oxygen. The oxidation state on chlorine Cl is to be determined;
O: -2.

Let the oxidation state on Cl be x.

<em>Refer to the equation in BaSO₄ as an example. Try setting up the equation on your own. </em>

x = 3.

Hence, the oxidation state on Cl is +3.

Ions carry charge. Oxidation states on atoms in an ion shall add up to the charge of the ion. The superscript of an ion shows its charge. The superscript 3- in the phosphate ion shows that the ion carries a charge of -3.

Oxidation states:

The oxidation state on P is to be found;
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Let the oxidation state on P be x.

x + 4 × (-2) = -3;

x = 5.

Hence, the oxidation state on P is +5.

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3 years ago