A voltaic cell is constructed with an Ag/Ag⁺ half-cell and a Pb/Pb²⁺ half-cell. The silver electrode is positive.(a) Write balan
1 answer:
<h3>Redox Half reaction</h3>
Reduction
+ 1e- → Ag
Oxidation
Pb → + 2e-
+ Pb → Ag +
Cathodic protection is a method of controlling corrosion on a metal surface by converting it into the cathode of an electrochemical cell. A straightforward method of protection involves connecting protected metal to a more easily corroded "sacrificial anode" to serve as the anode. The sacrificial metal, rather than the protected metal, corrodes. Galvanized steel is a common application of cathodic protection, in which a sacrificial zinc coating on steel parts protects them from rust.
Oxidation is used in a wide range of industries, including the manufacture of cleaning products and the oxidation of ammonia to produce nitric acid.
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Answer:
35.41 L
Explanation:
Given, Volume of Copper = 4.84 cm³
Density = 8.95 g/cm³
Considering the expression for density as:
So,
So, Mass= Density Volume = 8.95 g/cm³ 4.84 cm³ = 43.318 g
Mass of copper = 43.318 g
Molar mass of copper = 63.546 g/mol
The formula for the calculation of moles is shown below:
Thus,
Moles of copper = 0.6817 moles
Given, Volume of nitric acid solution = 227 mL = 227 cm³
Density = 1.42 g/cm³
Considering the expression for density as:
So,
So, Mass= Density Volume = 1.42 g/cm³ 227 cm³ = 322.34 g
Also, Nitric acid is 68.0 % by mass. So,
Mass of nitric acid = = 219.1912 g
Molar mass of nitric acid = 63.01 g/mol
The formula for the calculation of moles is shown below:
Thus,
Moles of nitric acid = 3.4786 moles
According to the reaction,
1 mole of copper react with 4 moles of nitric acid
Thus,
0.6817 moles of copper react with 4*0.6817 moles of nitric acid
Moles of nitric acid required = 2.7268 moles
Available moles of nitric acid = 3.4786 moles
Limiting reagent is the one which is present in small amount. Thus, nitric acid is present in large amount, copper is the limiting reagent.
The formation of the product is governed by the limiting reagent. So,
1 mole of copper on reaction forms 2 moles of nitrogen dioxide
So,
0.6817 mole of copper on reaction forms 2*0.6817 moles of nitrogen dioxide
Moles of nitrogen dioxide = 1.3634 moles
Given:
Pressure = 724 torr
The conversion of P(torr) to P(atm) is shown below:
So,
Pressure = 724 / 760 atm = 0.9526 atm
Temperature = 28.2 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (28.2 + 273.15) K = 301.35 K
Using ideal gas equation as:
PV=nRT
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
0.9526 atm × V = 1.3634 mol × 0.0821 L.atm/K.mol × 301.35 K
⇒V = 35.41 L