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oksian1 [2.3K]
3 years ago
9

A standard galvanic cell is constructed so that the overall cell reaction is as given below where M is an unknown metal. 2 Al3+(

aq) + 3 M(s) 3 M2+(aq) + 2 Al(s) If ΔG° = -411 kJ for the overall cell reaction, identify the metal used to construct the standard cell.
Chemistry
1 answer:
jasenka [17]3 years ago
5 0

Answer:

magnesium metal

Explanation:

According to the redox reaction equation, six electrons were transferred hence n=6 and F= Faraday's constant 96500C. ∆G° is given hence E°cell can easily be calculated as follows:

From ∆G°= -nFE°cell

E°cell= -∆G°/nF= -(-411×10^3/96500×6)

E°cell= 0.7098V

But for Al3+(aq)/Al(s) half cell, E°= -1.66V from standard table of reduction potentials.

E°cell= E°cathode- E°anode but Al3+(aq)/Al(s) half cell is the cathode

Hence

E°anode=E°cathode - E°cell

E°anode= -1.66-0.7098= -2.37V

This is the reduction potential of Mg hence the anode material was magnesium metal

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After the reaction of mixture is worked-up Washing three times the organic  with sodium carbonate helps to decrease the solubility of the organic layer into the aqueous layer. This allows the organic layer to be separated more easily.

And then the reaction washed by saturated NACL we have The bulk of the water can often be removed by shaking or "washing" the organic layer with saturated aqueous sodium chloride (otherwise known as brine). The salt water works to pull the water from the organic layer to the water layer.

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3 years ago
Which of the following is a pure substance? Choose all that apply.
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A. Solution, Colloid, Suspension

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3 years ago
Which two terms relate and why? Compound, ion, proton
Lerok [7]

ion, proton

Explanation:

Ions and protons have profound relationships.

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5 0
3 years ago
How much CuSO4*5H2O and Na2CO3 is needed to obtain 5g of CuCO3?
Svetllana [295]
I think the reaction that is occurring is CuSO₄(aq)+Na₂CO₃(aq)⇒CuCO₃(s)+Na₂SO₄(aq).  Water in the hydrate will just become part of water in solution so it does not really matter for this question.  
SInce we now know the balanced chemical equation, you can use stoichiometry to find the amount of reactants needed to produce 5g CuCO₃.  
The first step to any stoichiometry question is to convert the mass given into moles.  To do this you have to divide the mass by the molar mass of the compound the mass is referring to.  The molar mass of CuCO₃ is 123.5g/mol so you have to divide 5g by 123.5g/mol to get 0.04047 moles of CuCO₃.
The next step in this qustoin is to find the number of moles of each reactant using the moles of product we found in the first step.  To do this, we need go back and look at the equation to find the molar ratios which is shown through the coefficients.  Since all of the coeficients in the chemical equation is 1, we know the molar ratios are all `1 to 1 and therefore the number of moels of each reactant is equal to the number of moles of the product found in step one.  This means that you started off with 0.04047 moles of both CuSO₄ and Na₂CO₃.
The final step is to multiply the number moles of each reactant by its molar mass.  the molar mass of CuSO₄ is 159.6g/mol and the molar mass of Na₂CO₃ is 106g/mol.  When you multiply 0.04047mol by 159.6g/mol you get 6.4g and when you multiply 0.04047mol by 106g/mol you get 4.29g.
Therefore you started with 6.4g of CuSO₄ and 4.29g of Na₂CO₃.
I hope this helps.
5 0
3 years ago
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