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leonid [27]
3 years ago
11

If you change number of neutrons in an atom, you will also change its-

Chemistry
1 answer:
ikadub [295]3 years ago
5 0

Answer:

atomic mass. You will have created an isotope.

Explanation:

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What region of the atom contains most of the atoms mass?
dimulka [17.4K]

Answer:

Nucleus

Explanation: it is the center of the atom, and contains protons and nuetrons

7 0
3 years ago
Read 2 more answers
Which element would you expect to have properties similar to Chlorine (Cl)
jeyben [28]

Answer:

Iodine

Explanation:

It's in the same group as chlorine.

5 0
3 years ago
Please help
Molodets [167]

Answer:

A strip of magnesium metal is ignited using a lighter wand. The result is

an intensely glowing white light. As the burning of the metal subsides, a

white powder-like substance now appears replacing the smooth ribbon of

metal.

8 0
3 years ago
How many moles of oxygen will be produced from the decomposition of 3 moles of KClO3?
AlexFokin [52]

Answer:

4.5moles

Explanation:

First, let us balance the equation given from the question. This is illustrated below:

KClO3 —> KCl + O2

There are 2 atoms of O on the right side and 3 atoms on the left. It can be balance by putting 2 in front of KClO3 and 3 in of O2 as shown below

2KClO3 —> KCl + 3O2

Now, we have 2 atoms each of K and Cl on the left side and 1atom each of K and Cl on the right. It can be balance by putting 2 in front of KCl as shown below:

2KClO3 —> 2KCl + 3O2

Now the equation is balanced.

From the balanced equation,

2 moles of KClO3 produced 3 moles of O2.

Therefore, 3 moles of KClO3 will produce = (3 x 3) /2 = 4.5moles of O2.

Therefore 3 moles of KClO3 will produce 4.5 moles of O2

5 0
3 years ago
Which of the following equations represent redox reactions? For each redox reaction, determine which atom is oxidized and which
makkiz [27]

Answer:

c. H2(g) + CuO(s) → Cu(s) + H2O(l)

e. H2(g) + Cl2(g) → 2HCl(g)

Explanation:

A redox reaction is a reaction that involves a changes in oxidation number of the species involved in the reaction.

The oxidizing agent experiences a decrease in oxidation number while the reducing agent experiences an increase in oxidation number.

For H2(g) + CuO(s) → Cu(s) + H2O(l)

Copper is reduced from +2 to 0 while hydrogen is oxidized from 0 to +2 Hence hydrogen is the reducing agent while copper is the oxidizing agent.

For H2(g) + Cl2(g) → 2HCl(g)

Chlorine is reduced from 0 to -1 while hydrogen is oxidized from 0 to +1. Hence chlorine is the oxidizing agent while hydrogen is the reducing agent.

4 0
2 years ago
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