# what is the name for the compound with the formula as2o5?

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## What is the name for the compound with the formula As2O5?

**Arsenic**

All compounds containing arsenic (Ar) are toxic to humans. In high concentrations, arsenic can cause damage to internal organs, blood vessels, and the nervous system. Lower concentrations over a long period of time can cause various types of cancer.

## Formula of ARSENIC PENTOXIDE (As2O5)

The ARSENIC PENTOXIDE molecule contains a total of 7 atom(s). There are 5 Oxygen atom(s). A chemical formula of ARSENIC PENTOXIDE can therefore be written as:

**As2O5**

The chemical formula of ARSENIC PENTOXIDE shown above is based on the molecular formula indicating the numbers of each type of atom in a molecule without structural information, which is different from the empirical formula which provides the numerical proportions of atoms of each type.

The above chemical formula is the basis of stoichiometry in chemical equations, i.e., the calculation of relative quantities of reactants and products in chemical reactions. The law of conservation of mass dictates that the quantity of each element given in the chemical formula does not change in a chemical reaction. Thus, each side of the chemical equation must represent the same quantity of any particular element based on the chemical formula.

## What is the compound name for As2O5?

ARSENIC PENTOXIDE

Arsenic pentoxide

PubChem CID | 14771 |
---|---|

Chemical Safety | Laboratory Chemical Safety Summary (LCSS) Datasheet |

Molecular Formula | As2O5 |

Synonyms | ARSENIC PENTOXIDE Arsenic(V) oxide 1303-28-2 Arsenic(V) pentoxide Arsenic acid anhydride More… |

Molecular Weight | 229.84 |

## What is the molecular formula for As2O5?

As2O5

Arsenic pentoxide/Formula

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## how to balance as2o5?

* Step 1. Write down the unbalanced equation* (‘skeleton equation’) of the chemical reaction. All reactants and products must be known. For a better result write the reaction in ionic form.

_{3}

^{–}→ As

_{2}O

_{5}+ NO

* Step 2. Separate the process into half reactions.* A redox reaction is nothing but both oxidation and reduction reactions taking place simultaneously.

* a) Assign oxidation numbers* for each atom in the equation. Oxidation number (also called oxidation state) is a measure of the degree of oxidation of an atom in a substance.

_{3}

^{–}→ As+5

_{2}O-2

_{5}+ N+2O-2

* b) Identify and write out all redox couples in reaction.* Identify which reactants are being oxidized (the oxidation number increases when it reacts) and which are being reduced (the oxidation number goes down). Write down the transfer of electrons. Carefully, insert coefficients, if necessary, to make the numbers of oxidized and reduced atoms equal on the two sides of each redox couples.

**O:**

_{2}O-2

_{5}+ 10e

^{–}

**R:**

_{3}

^{–}+ 3e

^{–}→ N+2O-2

* c) Combine these redox couples into two half-reactions:* one for the oxidation, and one for the reduction .

**O:**

_{2}O-2

_{5}+ 10e

^{–}

**R:**

_{3}

^{–}+ 3e

^{–}→ N+2O-2

* Step 3. Balance the atoms in each half reaction.* A chemical equation must have the same number of atoms of each element on both sides of the equation. Add appropriate coefficients (stoichiometric coefficients) in front of the chemical formulas to balance the number of atoms. Never change any formulas.

* a) Balance all other atoms except hydrogen and oxygen.* We can use any of the species that appear in the skeleton equations for this purpose. Keep in mind that reactants should be added only to the left side of the equation and products to the right.

**O:**

_{2}O-2

_{5}+ 10e

^{–}

**R:**

_{3}

^{–}+ 3e

^{–}→ N+2O-2

* b) Balance the charge.* For reactions in an acidic solution, balance the charge so that both sides have the same total charge by adding a H

^{+}ion to the side deficient in positive charge.

**O:**

_{2}O-2

_{5}+ 10e

^{–}+ 10H

^{+}

**R:**

_{3}

^{–}+ 3e

^{–}+ 4H

^{+}→ N+2O-2

* c) Balance the oxygen atoms.* Check if there are the same numbers of oxygen atoms on the left and right side, if they aren’t equilibrate these atoms by adding water molecules.

**O:**

_{2}O → As+5

_{2}O-2

_{5}+ 10e

^{–}+ 10H

^{+}

**R:**

_{3}

^{–}+ 3e

^{–}+ 4H

^{+}→ N+2O-2 + 2H

_{2}O

Balanced half-reactions are well tabulated in handbooks and on the web in a ‘Tables of standard electrode potentials’. These tables, by convention, contain the half-cell potentials for reduction. To make the oxidation reaction, simply reverse the reduction reaction and change the sign on the E_{1/2} value.

* Step 4. Make electron gain equivalent to electron lost.* The electrons lost in the oxidation half-reaction must be equal the electrons gained in the reduction half-reaction. To make the two equal, multiply the coefficients of all species by integers producing the lowest common multiple between the half-reactions.

**O:**

_{2}O → As+5

_{2}O-2

_{5}+ 10e

^{–}+ 10H

^{+}

**R:**

_{3}

^{–}+ 3e

^{–}+ 4H

^{+}→ N+2O-2 + 2H

_{2}O

**O:**

_{2}O → 3As+5

_{2}O-2

_{5}+ 30e

^{–}+ 30H

^{+}

**R:**

_{3}

^{–}+ 30e

^{–}+ 40H

^{+}→ 10N+2O-2 + 20H

_{2}O

* Step 5. Add the half-reactions together.* The two half-reactions can be combined just like two algebraic equations, with the arrow serving as the equals sign. Recombine the two half-reactions by adding all the reactants together on one side and all of the products together on the other side.

_{3}

^{–}+ 15H

_{2}O + 30e

^{–}+ 40H

^{+}→ 3As+5

_{2}O-2

_{5}+ 10N+2O-2 + 30e

^{–}+ 20H

_{2}O + 30H

^{+}

* Step 6. Simplify the equation.* The same species on opposite sides of the arrow can be canceled. Write the equation so that the coefficients are the smallest set of integers possible.

_{3}

^{–}+ 10H

^{+}→ 3As+5

_{2}O-2

_{5}+ 10N+2O-2 + 5H

_{2}O

* Finally, always check to see that the equation is balanced.* First, verify that the equation contains the same type and number of atoms on both sides of the equation.