Answer:
B => Mg° => Mg⁺² + 2e⁻
Explanation:
2Mg° + O₂ => 2MgO rewrite => Mg° + 1/2O₂ => 2MgO
Oxidation Half Rxn => Mg° => Mg⁺² + 2e⁻
Reduction Half Rxn => 1/2O₂ + 2e⁻ => 2O⁻
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FYI Note => For half-reactions one always finds the electrons listed on the product side of the reaction for oxidation reactions and for reduction reactions on the reactant side.
Volume of H₂O added = 175 ml
<h3>Further explanation</h3>
Given
100 gm of a 55% (M/M) and 20% (M/M) nitric acid solution
Required
waters added
Solution
starting solution
mass H₂O = 45%=45 g
%mass of H₂O in new solution = 100%-20%=80%
Can be formulated for %mass H₂O :
For water mass=volume(density = 1 g/ml)
So volume added = 175 ml
830 mL. A 2.3 mol/L solution of CaCl2 has a volume of 830 mL
I am guessing that the concentration of your solution is 2.3 mol/L.
a) Moles of CaCl2
MM of CaCl2 = 110.98 g/mol
Moles of CaCl2 = 212 g CaCl2 x (1 mol CaCl2/110.98 g CaCl2)
= 1.910 mol CaCl2
b) Volume of solution
V = 1.910 mol CaCl2 x (1 L solution/2.3 mol CaCl2) = 0.83 L solution
= 830 mL solution
<h3>
Answer:</h3>
Ag⁺(aq) +Cl⁻(aq) → AgCl(s)
<h3>
Explanation:</h3>
The questions requires we write the net ionic equation for the reaction between aqueous potassium chloride and aqueous silver nitrate.
<h3>Step 1: Writing a balanced equation for the reaction.</h3>
- The balanced equation for the reaction between aqueous potassium chloride and aqueous silver nitrate will be given by;
KCl(aq) + AgNO₃(aq) → KNO₃(aq) +AgCl(s)
- AgCl is the precipitate formed by the reaction.
<h3>Step 2: Write the complete ionic equation.</h3>
- The complete ionic equation for the reaction is given by showing all the ions involved in the reaction.
K⁺(aq)Cl⁻(aq) + Ag⁺(aq)NO₃⁻(aq) → K⁺(aq)NO₃⁻(aq) +AgCl(s)
- Only ionic compounds are split into ions.
<h3>Step 3: Write the net ionic equation for the reaction.</h3>
- The net ionic equation for a reactions only the ions that fully participated in the reaction and omits the ions that did not participate in the reaction.
- The ions that are not involved directly in the reaction are known as spectator ions and are not included while writing net ionic equation.
Ag⁺(aq) +Cl⁻(aq) → AgCl(s)
