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Svetach [21]
3 years ago
14

What is an example of inert elements​

Chemistry
2 answers:
solmaris [256]3 years ago
8 0
Neon, Helium, Krypton, Xenon, Argon
marusya05 [52]3 years ago
8 0
Inert gases helium argon neon krypton xenon and radón another noble gas element does not occur naturally.
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HELP NEED HELP PLEASE !!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
Goshia [24]

Answer: B) 4.2 M

Explanation:

Molarity = moles of solute/litre of solution

1560mL/1000 = 1.56 litres

6.5/1.56 = x/1

x = 4.2

M of solution = 4.2

3 0
3 years ago
An aqueous solution of potassium carbonate combine with a solution of calcium nitrate. What are the total and net ionic equation
romanna [79]
<span><span>K_2</span>C<span>O_3</span>(aq)+Ca(N<span>O_3</span><span>)_2</span>(aq)→ ?</span>
If we break these two reactants up into their respective ions, we get...<span><span>
K^+ </span>+ C<span>O^2_3 </span>+ C<span>a^<span>2+ </span></span>+ N<span>O_−3</span></span>
If we combine the anion of one reactant with the cation of the other and vice-versa, we get...<span>
CaC<span>O_3 </span>+ KN<span>O_3</span></span>

Now we need to ask ourselves if either of these is soluble in water. Based on solubility rules, we know that all nitrates are soluble, so the potassium nitrate is. Alternatively, we know that all carbonates are insoluble except those of sodium, potassium, and ammonium; therefore, this calcium carbonate is insoluble. This is good. It means we have a driving force for the reaction! That driving force is that a precipitate will form. In such a case, a precipitation reaction will occur, and the total equation will be...<span><span>
K_2</span>C<span>O_3</span>(aq) + Ca(N<span>O_3</span><span>)_2</span>(aq) → CaC<span>O_3</span>(s) + 2KN<span>O_3</span>(aq)</span>

To determine the net ionic equation, we need to remove all ions that appear on both sides of the equation in aqueous solution -- these ions are called spectator ions, and do not actually undergo any chemical reaction. To determine the net ionic equation, let's first rewrite the equation in terms of ions...
2K^+(aq) + CO_3^{2-}(aq) + Ca^{2+}(aq) + 2NO_3^{-}(aq) → Ca^{2+}(s) + CO_3^{2-}(s) + 2K^+(aq) + 2NO_3^-(aq)

The species that appear in aqueous solution on both sides of the equation (spectator ions) are... <span>
2K^+,NO_3^-</span>
If we remove these spectator ions from the total equation, we will get the net ionic equation...
CO_3^{2-}(aq) + Ca^{2+}(aq) <span>→</span> CaCO_3(s)
5 0
3 years ago
what mass of Fe2O3 is produced in the reaction in the table above mass of reactants= 223.4 g Fe+96.0 g O2. and mass of products=
Ganezh [65]

Answer:

AS ACCORDING TO THE LAW OF MASS CONSERVATION

REACTANTS =PRODUCTS

THEREFORE,

223.4+96=MASS OF FE2O3

=319.4 FE203

4 0
3 years ago
Write a balanced half-cell equation for the reaction occurring at the anode. ignore phases in the reaction.
r-ruslan [8.4K]

The balanced half-cell equation for the reaction occurring at the anode is  H2 ---> 2H(+) + 2e(-)

E<u>xplanation:</u>

  • The balanced half-cell equation taking place at the anode is explained below
  • The product produced in the reaction in the fuel cell is water.
  • H2 ---> 2H(+) + 2e(-)
  • In the above reaction, the oxidation state of hydrogen switches from 0 to +1.
  • It is becoming oxidized by delivering two electrons at the anode.
  • In the fuel cell, hydrogen molecules get oxidized to hydronium ions.Thus half-reaction is the oxidation reaction.

<u />

7 0
3 years ago
Sodium metal reacts vigorously with water
Sphinxa [80]
This is a true statement.
7 0
4 years ago
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