តើកាបូនមានវ៉ាឡង់ប៉ុន្មាន

An iron storage tank is placed in the ocean with no cathodic protection. a. What is the electrolyte in this reaction? b. As the

MariettaO [177]

Answer:

Iron is being oxidized at the anode and water is acting as the electrolyte.

Explanation:

When iron is exposed to oxygen and water , the rusting of iron takes place.

The reaction taking place at anode : Oxidation of iron.

${anode:}\;\text{Fe}(s)\;{\longrightarrow}\;\text{Fe}^{2+}(aq)\;+\;2\text{e}^{-}$

The reaction taking place at cathode : Reduction of oxygen in the air.

${cathode:}\;\text{O}_2(g)\;+\;4\text{H}^{+}(aq)\;+\;4\text{e}^{-}\;{\longrightarrow}\;2\text{H}_2\text{O}(l)$

The overall reaction:

${overall:}\;2\text{Fe}(s)\;+\;\text{O}_2(g)\;+\;4\text{H}^{+}(aq)\;{\longrightarrow}\;2\text{Fe}^{2+}(aq)\;+\;2\text{H}_2\text{O}(l)$

The rust that is hydrated iron(III) oxide can form iron(II) ions which can react further with oxygen.

$4\text{Fe}^{2+}(aq)\;+\;\text{O}_2(g)\;+\;(4\;+\;2x)\;\text{H}_2\text{O}(l)\;{\longrightarrow}\;2\text{Fe}_2\text{O}_3{\cdot}x\text{H}_2\text{O}(s)\;+\;8\text{H}^{+}(aq)$

Thus, from the above reactions ,

Iron is being oxidized at the anode and water is acting as the electrolyte.

3 0

4 years ago

Use bond energies from Table 10.3 in the textbook to estimate the enthalpy change (ΔH) for the following reaction. C2H2(g)+H2(g)

Digiron [165]

Answer: $=176.6kJmol^{-1}$

Explanation:Bond energy of H-H is 436.4 kJ/mole

Bond energy of C-H is 414 kJ/mol

Bond energy of C=C is 620 kJ/mol

Bond energy of C≡C is 835 kJ/mol

$\Delta H= {\text {sum of bond energies of reactants}}- {\text {sum of bond energies of products}}$

$\Delta H$ = {1B.E(C≡C)+2B.E(C-H) +1B.E(H-H)} - {1B.E(C=C)+4B.E(C-H)}

$\Delta H= {1B.E(835kJmole^{-1})+2B.E(414kJmole^{-1}) +1B.E(436.4kJmole^{-1})} - {1B.E(620kJmole^{-1})+4B.E(414kjmole^{-1})}$

$=176.6kJmol^{-1}$

7 0

4 years ago

A reaction is designated as exergonic rather than endergonic when _____.

dem82 [27]

Answer:

Reaction is called exergonic when ΔG is negative i.e. ΔG < 0

Explanation:

The Gibbs free energy represents the spontaneity or feasibility of a given chemical reaction at constant pressure and temperature and is given by the equation:

ΔG = ΔH - TΔS

Here, ΔG - change in the Gibbs free energy

ΔS - change in the entropy

ΔH - change in the enthalpy

T - temperature

If the value of ΔG for a chemical reaction is positive i.e. ΔG > 0, then the given chemical reaction is said to be nonspontaneous. Such a reaction is called endergonic.

Whereas, if the ΔG value for a chemical reaction is negative i.e. ΔG < 0, then the given chemical reaction is said to be spontaneous. Such a reaction is called exergonic.

7 0

4 years ago

Assume you have a sealed jug that only contains air. If you heat the air in the jug it will have a higher temperature. What are

shutvik [7]

Answer: pressure

Explanation: expands

4 0

3 years ago

A 1.25 g sample of aluminum is reacted with 3.28 g of copper (II) sulfate. What is the limiting reactant? 2Al(s) + 3CuSO4(aq) →

vova2212 [387]

Answer:

Copper (II) sulfate

Explanation:

Given reaction is

2Al(s) + 3CuSO4(aq) → Al2(SO4)3(aq) + 3Cu(s)

Amount of aluminum = 1·25 g

Amount of copper (II) sulfate = 3·28 g

Atomic weight of Al = 26 g

Molecular weight of CuSO4 ≈ 159·5

Number of moles of Al = 1·25 ÷ 26 = 0·048

Number of moles of CuSO4 = 3·28 ÷ 159·5 = 0·021

From the above balanced chemical equation for every 2 moles of aluminum, 3 moles of copper (ll) sulfate will be required

So for 1 mole of Al, 1·5 moles of copper (ll) sulfate will be required

For 0·048 moles of Al, 1.5 × 0·048 moles of copper (ll) sulfate will be required

∴ Number of moles of copper (ll) sulfate required = 0·072

But we have only 0·021 moles of copper (ll) sulfate

As copper (ll) sulfate is not there in required amount, the limiting reactant will be copper (ll) sulfate

∴ The limiting reactant is copper (ll) sulfate

7 0

3 years ago