Explanation:
Reaction:
Cu + 2AgC₂H₃O₂ → Cu(C₂H₃O₂)₂ + 2Ag
The problem is to split the reaction into oxidation and reduction halves:
The oxidation half is the sub-reaction that undergoes oxidation
The reduction half is the one that undergoes reduction:
The ionic equation:
Cu + 2Ag⁺ + 2C₂H₃O₂⁻ → Cu²⁺ + 2C₂H₃O₂⁻ + 2Ag
Oxidation half:
Cu → Cu²⁺ + 2e⁻
Reduction half:
2Ag⁺ + 2e⁻ → 2Ag
C₂H₃O₂⁻ is neither oxidized nor reduced in the reaction.
learn more:
Oxidation state brainly.com/question/10017129
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The balanced chemical equation would be as follows:
<span>AlCl3(aq) + 3AgC2H3O2(aq) -> 3AgCl(s) + Al(C2H3O2)3(aq)
</span>
We are given the concentrations of the reactants. We use these values to calculate for the volume of aluminum chloride needed. We do as follows:
0.500 mol/L AgC2H3O2 (0.020 L) ( 1 mol AlCl3 / 3 mol AgC2H3O2 ) ( 1 L / 0.250 AlCl3 ) = 0.0133 L or 13.3 mL of AlCl3 solution is needed
Because they don’t have the same elements i guess, what is question 1?
Answer:
We have to add 14 mL of water to dilute the alcohol solution from 13% to 6%
Explanation:
Step 1: Data given
Original solution has 12 mL of 13% alcohol
New volume has a concentration of 6%
Step 2: Determine how much pure alcohol you have in the solution.
0.13 * 12ml = 1.56 ml pure alcohol.
Step 3: Calculate ratio alcohol: total in volume
1.56 ml / 12 ml = .013
Step 4: add water to the total solution and set the desired percentage
1.56 ml / (12ml + x) = 0.06
1.56 = 0.06 (12 + x)
1.56 = 0.72 + 0.06x
0.84 = 0.06x
x = 14
We have to add 14 mL of water to dilute the alcohol solution from 13% to 6%
Answer: A.) 2 is the answer.
Explanation: