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lana66690 [7]
4 years ago
13

A non example of a protron

Chemistry
1 answer:
konstantin123 [22]4 years ago
3 0
A neutron is the opposite
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There are 3 naturally occurring isotopes of hydrogen and 2
DedPeter [7]

Answer:

True

Explanation:

Hydrogen has three naturally occuring isotopes and copper has two.

3 0
3 years ago
28. Explain the difference between the processes of melting and freezing?
natali 33 [55]
Freezing something makes it solid and melting something makes it a liquid
4 0
4 years ago
Read 2 more answers
HELP PLZ ASAP<br> will give brainliest
horrorfan [7]

Answer:

I believe that it would be the third option down.

Explanation:

The thermal energy is in constant motion in the COOLER room, and when the desired temperature in the room is reached, it stops.

8 0
3 years ago
Balancee las ecuaciones químicas por el método de tanteo e identifique que tipo de reacción es: 1.1.- Cloruro férrico acuoso rea
lakkis [162]

Respuesta:

2 FeCl₃(aq) + 3 Na₂CO₃(s) ⇒ Fe₂(CO₃)₃(s) + 6 NaCl(aq)

Explicación:

Consideremos la ecuación no balanceada que ocurre cuando cloruro férrico acuoso reacciona con carbonato de sodio sólido para formar carbonato férrico sólido y cloruro de sodio acuoso. Esta es una reacción de doble desplazamiento.

FeCl₃(aq) + Na₂CO₃(s) ⇒ Fe₂(CO₃)₃(s) + NaCl(aq)

Vamos a usar el método de tanteo. Empezaremos balanceando los átomos de C, multiplicando Na₂CO₃ por 3.

FeCl₃(aq) + 3 Na₂CO₃(s) ⇒ Fe₂(CO₃)₃(s) + NaCl(aq)

Luego, balancearemos los átomos de Fe, multiplicando FeCl₃ por 2.

2 FeCl₃(aq) + 3 Na₂CO₃(s) ⇒ Fe₂(CO₃)₃(s) + NaCl(aq)

Finalmente, obtendremos la ecuación balanceada, multiplicando NaCl por 6.

2 FeCl₃(aq) + 3 Na₂CO₃(s) ⇒ Fe₂(CO₃)₃(s) + 6 NaCl(aq)

4 0
3 years ago
xidation in redox reactions involves a. a loss of electrons and an increase in the oxidation number b. a gain of electrons and a
Strike441 [17]

Answer:

Option a is the right one

Explanation:

Redox reactions are defined as the reactions where one element is oxidized (so the oxidation state is increased); and another element is reduced (oxidation state decreases). These changes in the oxidations states are defined by a transference of electrons.

When the oxidation state decrease → reduction → the element gains electrons

When the oxidation state increase → oxidation → the element release electrons

4 0
3 years ago
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