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1 answer:
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Answer:
Explanation:
1. Write the equation for the reaction.
M_r: 24.30
MgCl₂ ⟶ Mg + Cl₂
m/g: 60.0
2. Calculate the moles of Mg
Moles of Mg = 60.0 g Mg × (1 mol Mg/ 24.30 g Mg) = 2.469 mol Mg
3. Calculate the moles of electrons
Moles of electrons = 2.469 mol Mg × (2 mol electrons/1 mol Mg)
= 4.938 mol electrons
4. Calculate the number of coulombs
Q = 4.938 mol electrons × (96 485 C/1 mol electrons) = 476 500 C
5. Calculate the current required
Q = It
I = Q/t
t = 2.00 h × (60 min/1h) × (60 s/1 min) = 7200 s
I = 476 500 C/7600 s= 66.2 C/s = 66.2 A
You need a current of .
Answer: The correct formula is
Explanation:
For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.
Here magnesium is having an oxidation state of +2 called as cation and bromine
is an anion with oxidation state of -1. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral
.
The cations and anions being oppositely charged attract each other through strong coloumbic forces and form an ionic bond.