The outer electron in magnesium is excited by absorbing the heat energy from the N=1 stage to higher energy levels when it starts to drop back down to the N=2 level it losses energy in the form of visible light this is part of the Balmer series
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Answer:
0.0658 M
Explanation:
The reaction that takes place is:
Na₂SO₄(aq) + BaCl₂(aq) ↔ BaSO₄(s) + 2NaCl(aq)
First we <u>calculate the number of Na₂SO₄ moles</u>:
- 0.4000 g sample * 96.4/100 = 0.3856 g Na₂SO₄
- 0.3856 g Na₂SO₄ ÷ 142.04 g/mol = 2.715x10⁻³ mol Na₂SO₄
Now we <u>convert to moles of BaCl₂</u>:
- 2.715x10⁻³ mol Na₂SO₄ * 1 molBaCl₂/1 molNa₂SO₄ = 2.715x10⁻³ mol BaCl₂
Finally we divide by the volume to <u>calculate the molarity</u>:
- 41.25 mL ⇒ 41.25 / 1000 = 0.04125 L
- 2.715x10⁻³ mol BaCl₂ / 0.04125 L = 0.0658 M
The latest one in Hawaii would be one but since this question is from 2016, None at all is the correct answer
Answer:
The Group 2 metals become more reactive towards the water as you go down the Group.
Explanation:
These all react with cold water with increasing vigour to give the metal hydroxide and hydrogen. ... You get less precipitate as you go down the Group because more of the hydroxide dissolves in the water. Summary of the trend in reactivity.
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