Help asap plzzzz 30 points

What is the scientific term for rocks formed from magma

gogolik [260]

The answer is Igneous rock. ^-^

7 0

3 years ago

The two naturally occurring isotopes of bromine are

ch4aika [34]

Answer:

The decreasing order of masses of for different BrCl molecules :

= $M_2$

= $113.887 amu ,115.884 amu ,115.885 amu ,117.882 amu$

Explanation:

The two naturally occurring isotopes of bromine are

81-Br (80.916 amu, 49.31%) 79-Br (78.918 amu, 50.69%).

The two naturally occurring isotopes of chlorine are

37-Cl (36.966 amu, 24.23%) and 35- Cl (34.969 amu, 75.77%).

Molar mass of BrCl molecule composed of 81-Br and 37-Cl.

Mass of 81-Br = 80.916 amu

Mass of 37-Cl = 36.966 amu

Molar mass of this BrCl molecule, $M_1$ = 80.916 amu + 36.966 amu

= 117.882 amu

Molar mass of BrCl molecule composed of 79-Br and 35-Cl.

Mass of 79-Br = 78.918 amu

Mass of 35-Cl = 34.969 amu

Molar mass of this BrCl molecule $M_2$ = 78.918 amu + 34.969 amu

= 113.887 amu

Molar mass of BrCl molecule composed of 81-Br and 35-Cl.

Mass of 81-Br = 80.916 amu

Mass of 35-Cl = 34.969 amu

Molar mass of this BrCl molecule, $M_3$ = 80.916 amu + 34.969 amu

= 115.885 amu

Molar mass of BrCl molecule composed of 79-Br and 37-Cl.

Mass of 79-Br = 78.918 amu

Mass of 37-Cl = 36.966 amu

Molar mass of this BrCl molecule, $M_4$ = 78.918 amu + 36.966 amu

= 115.884 amu

The decreasing order of masses of for different BrCl molecules :

= $M_2$

= $113.887 amu < 115.884 amu$

5 0

3 years ago

What is the coefficient of silver in the final, balanced equation for this reaction?

katovenus [111]

Answer: 3

Explanation:

An oxide-reduction reaction or, simply, redox reaction, is a chemical reaction in which one or more electrons are transferred between the reactants, causing a change in their oxidation states, which is the hypothetical electric charge that the atom would have if all its links with different elements were 100% ionic.

For there to be a reduction-oxidation reaction, in the system there must be an element that yields electrons and another that accepts them:

The oxidizing agent picks up electrons and remains with a state of oxidation inferior to that which it had, that is, it is reduced.
The reducing agent supplies electrons from its chemical structure to the medium, increasing its oxidation state, ie, being oxidized.

To balance a redox equation you must identify the elements that are oxidized and reduced and the amount of electrons that they release or capture, respectively.

In the reaction that arises in the question the silver (Ag) is reduced because it decreases its oxidation state from +1 to 0 and the aluminum (Al) is oxidized because its oxidation state increases from 0 to +3, releasing 3 electrons (e⁻). Then we can raise two half-reactions:

Ag⁺ + e⁻ → Ag⁰

Al⁰ → Al⁺³ + 3e⁻

In order to obtain the balanced equation, we must multiply the first half-reaction by 3 so that, when both half-reactions are added, the electrons are canceled. In this way:

(Ag⁺ + e⁻ → Ag⁰ ) x3

Al⁰ → Al⁺³ + 3e⁻ +

-------------------------------------

3Ag⁺ + Al⁰ → 3Ag⁰ + Al⁺³

So, the coefficient of silver in the final balanced equation is 3.

5 0

4 years ago

A solution is a ____________a liquid____________ mixture.

Tamiku [17]

it is a solute and a solvent

8 0

4 years ago