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Anna35 [415]
3 years ago
9

What is the overall voltage for the nonspontaneous redox reaction involving

Chemistry
2 answers:
Ann [662]3 years ago
6 0

Answer:

Answer D => E°(Mg°/Cu⁺²) = 0.34 + 2.37 = 2.71v

Explanation:

(Oxidation) =>  Mg°(s) => Mg⁺²(aq) + 2e⁻    E°(Mg°/Mg⁺²) = -2.37 v

(Reduction) => Cu⁺²(aq) + 2e⁻ => Cu°(s)     E°(Cu⁺²/Cu°) = +0.34 v

________________________________________________

Net Rxn => Mg°(s) + Cu⁺²(aq) => Mg⁺²(aq) + Cu°(s)

Std Cell Potential (25°C/1Atm) = E°(Redn) = E°(Oxidn) = +0.34v - (-2.37v)

= 0.34v + 2.37v = 2.72v

Margarita [4]3 years ago
3 0

Answer: B -2.37 -0.34

Explanation: A P E X

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Answer:

7.99 mol

Explanation:

Step 1: Given data

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Step 2: Calculate how many moles of chlorine gas corresponds to 4.81 × 10²⁴ molecules of chlorine gas

In order to convert molecules to moles, we will use Avogadro's number: there are 6.02 × 10²³ molecules of chlorine gas in 1 mole of molecules of chlorine gas.

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3 years ago
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City A is located along the shore of an ocean. City B is at the same latitude and altitude, but it is located
arlik [135]

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A In the summer, the daytime temperature in City A is typically lower than the daytime temperature  in City B.

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5 0
2 years ago
What mass of zinc (molar mass 65.4 g moll) does it take to produce 0.50 mole of H2(g)?
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32.7 g of Zn

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Next, we shall determine the number of mole of Zn required to produce 0.5 mole of H₂. This can be obtained as follow:

From the balanced equation above,

1 mole of Zn reacted to produce 1 mole of H₂.

Therefore, 0.5 mole of Zn will also react to produce to 0.5 mole of H₂.

Thus, 0.5 mole of Zn is required.

Finally, we shall determine the mass of 0.5 mole of Zn. This can be obtained as follow:

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Mass of Zn = 32.7 g

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2 years ago
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3 years ago
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