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dlinn [17]
3 years ago
5

What are the half-reactions for a galvanic cell with Zn and Mg electrodes?

Chemistry
1 answer:
Alona [7]3 years ago
7 0

the half-reactions

cathode : Zn²⁺ (aq) + 2e⁻ ---> Zn (s)  

anode : Mg (s) → Mg²⁺ (aq) + 2e−

a balanced cell reaction

Zn²⁺(aq) + Mg(s)→ Zn(s) + Mg²⁺ (aq)

<h3 /><h3>Further explanation</h3>

Given

Zn and Mg electrodes

Required

The half-reactions for a galvanic cell

Solution

To determine the reaction of a voltaic cell, we must determine the metal that serves as the anode and the metal that serves as the cathode.

To determine this, we can either know from the standard potential value of the cell or use the voltaic series

1. voltaic series

<em>Li-K-Ba-Ca-Na-Mg-Al-Mn- (H2O) -Zn-Cr-Fe-Cd-Co-Ni-Sn-Pb- (H) -Cu-Hg-Ag-Pt-Au </em>

The more to the left, the metal is more reactive (easily release electrons) and the stronger reducing agent

So the metal on the left will easily undergo oxidation and function as anode

Since Mg is located to the left of Zn, then Mg functions as anode and Zn as a cathode

2. Standard potentials cell of Mg and Zn metals :

Mg2+ + 2e– → Mg E° = -2,35 V

Zn2+ + 2e– → Zn E° = -0,78 V

The anode has a smaller E°, then Mg is the anode and Zn is the cathode.

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Ammonia (NH3) reacts with oxygen to form nitric oxide (NO) and water vapor: 4NH3 + 502 4NO + 6H2O b) When 20.0 g NH3 and 50.0 g
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b. Oxygen is left over and 0.1375 g of oxygen is left over.

c. The theoretical yield of NO is 35.29 g.

d. The theoretical yield of H_2O is 31.74 g.

Explanation:

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}  

For NH_3

Given mass of ammonia = 20.0 g

Molar mass of ammonia = 17.031 g/mol

Putting values in equation 1, we get:

\text{Moles of ammonia}=\frac{20.0g}{17.031g/mol}=1.17mol

For O_2

Given mass of oxygen gas = 50.0 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

\text{Moles of oxygen gas}=\frac{50.0g}{32g/mol}=1.6mol

The chemical equation for the reaction is

4NH_3+5O_2\rightarrow 4NO+6H_2O

By Stoichiometry of the reaction:

4 moles of ammonia reacts with = 5 moles of oxygen

So 1.17 moles of ammonia will react with = \frac{5}{4}\times 1.17=1.4625mol of oxygen

As, given amount of oxygen is more than the required amount. So, it is considered as an excess reagent and (1.6-1.4625)= 0.1375 g of oxygen is left unreacted.

Thus ammonia is considered as a limiting reagent because it limits the formation of product.

1. By Stoichiometry of the reaction:

4 moles of ammonia produces = 4 moles of NO

1.17 moles of ammonia will produce = \frac{4}{4}\times 1.17=1.17moles of NO

Mass of NO=moles\times {\text{Molar Mass}}=1.17\times 30=35.29g

Thus Theoretical yield of NO is 35.29 grams.

2. By Stoichiometry of the reaction:

4 moles of ammonia produces = 6 moles of H_2O

1.2 moles of ammonia will produce = \frac{6}{4}\times 1.2=1.8moles of H_2O

Mass of H_2O=moles\times {\text{Molar Mass}}=1.8\times 18.015=31.74g  H_2O

Thus Theoretical yield of H_2O is 31.74 grams.

8 0
3 years ago
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