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antiseptic1488 [7]
3 years ago
10

Write the nuclear equation for the alpha decay of:

Chemistry
1 answer:
Agata [3.3K]3 years ago
6 0

Answer:

The answer to your question is below

Explanation:

Alpha decay occurs when a radioactive atm emits an alpha particle (Helium atom).

a)      ²⁵⁶Ra      ⇒      ²⁵²₈₄ Po  +   ⁴₂He

b)     ²¹⁹Rn       ⇒      ²¹⁵₈₂Pb    +   ⁴₂He

c)      ²¹¹Po      ⇒      ²⁰⁷₈₀Hg    +   ⁴₂Hg

d)      ²¹⁰Pb     ⇒     ²⁰⁶₇₈Pt      +   ⁴₂Hg

e)      ²³⁸U      ⇒     ²³⁴₈₈U       +   ⁴₂Hg

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A hydrogen bond can occur between:
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Explanation:

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3 years ago
145.8g of Mg contains how many moles?
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8 0
3 years ago
Write the balanced NET IONIC equation for the reaction that occurs when ammonium nitrate and potassium hydroxide are combined. N
vova2212 [387]

Answer:

Net Ionic equation

NH₄⁺ + OH⁻ → NH₃ + H₂O

Option B is correct.

Weak Acid Strong Base

Check Explanation for the extent of the reaction.

Explanation:

Ammonium nitrate = NH₄NO₃

Potassium Hydroxide = KOH

Ammonium salts combine with alkalis to liberate NH₃ and form water.

The two reactants combine to give

NH₄NO₃ + KOH → KNO₃ + NH₃ + H₂O

In ionic form,

- NH₄NO₃ exists as NH₄⁺ and NO₃⁻

- KOH exists as K⁺ and OH⁻

- KNO₃ as K⁺ and NO₃⁻

And NH₃ and H₂O stay as they are, as per covalent compounds.

So, we have

NH₄⁺ + NO₃⁻ + K⁺ + OH⁻ → K⁺ + NO₃⁻ + NH₃ + H₂O

Eliminating the ions that exist on both sides, we have the net ionic equation to be

NH₄⁺ + OH⁻ → NH₃ + H₂O

which shows that this reaction is essentially a neutralization reaction in which the Bronsted Lowry acid, NH₄⁺, loses its proton to the base, OH⁻ and gives conjugate base, NH₃ and conjugate acid, H₂O.

This reaction is classified as a Weak acid versus Strong Base reaction as NH₄⁺ is from a Weak acid and OH⁻ is from a strong base.

Since this reaction is between a Weak base and a strong acid, the ionization isn't expected to be 100%, Hence, the extent of this reaction will be any option that is not 100%, a couple pieces of information might be required for the correct estimate, but above 50% seems correct.

Hope this Helps!!!

8 0
3 years ago
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