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Ethanol (C2H5OH) is synthesized for industrial use by the following reaction, carried out at very high pressure. C2H4(g) + H2O(g) right-arrow C2H5OH(l) What is the maximum amount, in kg, of ethanol that can be produced when 1.41 kg of ethylene (C2H4) and 0.0320 kg of steam are placed into the reaction vessel? 

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Related questions

9.Nickel, a common metal used in a variety of alloys, is purified via the Mond process to a very high (> 99.99%) purity. One of the steps in the Mond process involves the reaction of solid nickel with carbon monoxide to produce Ni(CO)4, as shown in the unbalanced equation below.

Ni(s) + CO(g) → Ni(CO)4(g)

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10.Thermite is a metal powder mixture used frequently in pyrotechnics and metal construction work. It is composed of highly powderized aluminum and iron(III) oxide and when ignited by a high temperature source (such as burning magnesium ribbon), it reacts according to the following equation.

Fe2O3(s) + 2 Al(s) → 2 Fe(l) + Al2O3(s)

What mass of powderized Al is required to completely react with 34.8 g Fe2O3?

11.In a reaction vessel, 18.0 g of solid chromium(III) oxide, Cr2O3, was allowed to react with excess carbon tetrachloride in the following reaction.

Cr2O3(s) + 3 CCl4(l) → 2 CrCl3(s) + 3 COCl2(aq)

Determine the percent yield of the reaction, given that the actual yield of chromium chloride, CrCl3, was 29.5 g. (The molar mass of Cr2O3 is 152.00 g/mol and the molar mass of CrCl3 is 158.35 g/mol.)

12. Ammonia (NH3) can be synthesized from nitrogen gas (N2) and hydrogen gas (H2) by the following reaction.

N2(g) + 3 H2(g) → 2 NH3(g)

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13.In making wine, glucose (C6H12O6) is fermented to produce ethanol (C2H5OH) and carbon dioxide (CO2), according to the following reaction.

C6H12O6 → 2 C2H5OH + 2 CO2

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The reaction 1⁄2O2(g) + H2(g) → H2O(l) is used in fuel cells to produce an electrical current. The reaction can also be carried out by direct combustion.

Thermodynamic data: standard molar entropies in J mol–1 K–1:

O2(g) 205.0

H2(g)130.6

H2O(l) 70.0; and H2O(l) ΔH°f = –285.9 kJ mol–1.

Use this information to find:

a) The amount of heat released when the reaction takes place by direct combustion

b) The amount of electrical work the same reaction can perform when carried out in a fuel cell at 298K under reversible conditions

c) The amount of heat released under the same conditions.

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