Homework Answers
Actual yield of Fe = 22.7 g
Use:
% yield = actual yield * 100 / theoretical yield
93.2 = 22.7 * 100 / theoretical yield
theoretical yield = 24.36 g
Molar mass of Fe = 55.85 g/mol
mass of Fe = 24.36 g
mol of Fe = (mass)/(molar mass)
= 24.36/55.85
= 0.4362 mol
According to balanced equation
mol of Al required = moles of Fe
= 0.4362 mol
Molar mass of Al = 26.98 g/mol
mass of Al = number of mol * molar mass
= 0.4362*26.98
= 11.8 g
Answer: C
Add Answer to:
2. Consider the balanced Thermite reaction below, which has a reaction yield of 93.2%. If you're...
In the thermite reaction, iron (III) oxide is reduced by aluminum to give molten iron, Fe2O3...
In the thermite reaction, iron (III) oxide is reduced by aluminum to give molten iron, Fe2O3 (s) + 2 Al (s) --> 2 Fe (l) + Al2O3 (s) If you begin with 10.0 g of Fe2O3 and 20.0 g Al, Which reactant is limiting? What mass of Fe can be produced? What mass of the excess reactant remains after the limiting reactant is consumed? Set up an amounts table for this problem.
2. Some underwater welding is done via the thermite reaction, in which rust (Fe2O3) reacts with...
2. Some underwater welding is done via the thermite reaction, in which rust (Fe2O3) reacts with aluminum to produce iron and aluminum oxide (Al2O3). In one such reaction, 258 g of aluminum and excess rust produced 464 g of iron. What was the percent yield of the reaction?
3. Iron can be produced by the thermite reaction according to the following equation: Fe2O3 (s)...
3. Iron can be produced by the thermite reaction according to the following equation: Fe2O3 (s) +2Al (s) produces 2 Fe (s) + Al2O3 (s) a) If 100.0 g of Fe2O3 reacts with 30.0 g of Al, which one will be used up first? b) How much iron (in g) could be produced? c) If the only result in 45.0 g what is the percent yield?
Question 21 5 pts Determine the percent yield of a reaction that produces 30.0 g of...
Question 21 5 pts Determine the percent yield of a reaction that produces 30.0 g of Fe in the laboratory when Fe2O3 react with 20.0 g excess Al according to the following reaction. The theoretical yield of the reaction is 45.0 g of Fe. Fe2O3(s) + 2 Al(s) A1203(s) + 2 Fe(s) 81.9390 66.79 57.30% 44,49 75.0
Given the equation, which may or may not be balanced: Fe2O3(s) + CO(g) → Fe(s) +...
Given the equation, which may or may not be balanced: Fe2O3(s) + CO(g) → Fe(s) + CO2(g) How many grams of Fe could be produced from the complete reaction of 3.196 grams of Fe2O3 with excess CO? grams Fe What is the percent yield of the reaction if only 1.571 grams of Fe are recovered after the reaction has completed? %
Determine the percent yield of a reaction that produces 28 65 g of Fe when 50.0...
Determine the
percent yield of a reaction that produces 28 65 g of Fe when 50.0
00 g of Fez0s react with excess Al according to the following
reaction Fe2O3(s)+2 Al(s) Al2O3(s)+2 Fe(s)
W-SUMMERZC xCourse Home urse html?courseld-14733194&OpenVellumHMAC 01b27od2b2d7819a51616320b79deb92 10001 CHIM 151 0W Summer 2018 SCC e Home xam 3 2 Hide em Constant Part A Determine the percent yield of a reaction that produces 28 65 g of Fe when 50 00 g of Fe0s react with excess Al...
Question 5 2 pts The thermite reaction, which Dr. Jew set off in class (!), is...
Question 5 2 pts The thermite reaction, which Dr. Jew set off in class (!), is the reaction of iron(III) oxide with aluminum according to the balanced reaction: Fe2O3(s) + 2 Al(s) --> Al2O3(s) + 2 Fe(l) dH = -849 kJ What would be the value of dH if... (a) ... the reaction is reversed? (b) ... the coefficients are all doubled? (c) ... the reaction is reversed and all coefficients are halved? value of dH if the reaction is...
How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below
How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s), ΔH°rxn = -852 kJ
For the reaction 2 Al + 3 H,SO -3H, + A1, (SO), how many grams of...
For the reaction 2 Al + 3 H,SO -3H, + A1, (SO), how many grams of sulfuric acid, H2SO4, are needed to react completely with 51.9 g of aluminum, Al? 100 mass: 1/100 0/100 Consider the reaction. heat 2 Al(s) + Fe,0,(3) ***, ALO3(s) + 2 Fe(1) If 17.7 kg Al reacts with an excess of Fe,Og, how many kilograms of A1, O, will be produced? mass of A1,03 produced:
Consider the balanced chemical reaction that phosphorus and iodine react to produce phosphorus triodide: 2 P(s)...
Consider the balanced chemical reaction that phosphorus and iodine react to produce phosphorus triodide: 2 P(s) + 3 I2(g) → 2 PI3(g) If 131 g of I2(s) area reacted with excess P(s) to produce 0.306 mol of PI3(g), what is the percent yield of PI3(g)?
Question 21 5 pts Determine the percent yield of a reaction that produces 30.0 g of Fe in the laboratory when Fe2O3 react with 20.0 g excess Al according to the following reaction. The theoretical yield of the reaction is 45.0 g of Fe. Fe2O3(s) + 2 Al(s) A1203(s) + 2 Fe(s) 81.9390 66.79 57.30% 44,49 75.0
Determine the
percent yield of a reaction that produces 28 65 g of Fe when 50.0
00 g of Fez0s react with excess Al according to the following
reaction Fe2O3(s)+2 Al(s) Al2O3(s)+2 Fe(s)
W-SUMMERZC xCourse Home urse html?courseld-14733194&OpenVellumHMAC 01b27od2b2d7819a51616320b79deb92 10001 CHIM 151 0W Summer 2018 SCC e Home xam 3 2 Hide em Constant Part A Determine the percent yield of a reaction that produces 28 65 g of Fe when 50 00 g of Fe0s react with excess Al...
Question 5 2 pts The thermite reaction, which Dr. Jew set off in class (!), is the reaction of iron(III) oxide with aluminum according to the balanced reaction: Fe2O3(s) + 2 Al(s) --> Al2O3(s) + 2 Fe(l) dH = -849 kJ What would be the value of dH if... (a) ... the reaction is reversed? (b) ... the coefficients are all doubled? (c) ... the reaction is reversed and all coefficients are halved? value of dH if the reaction is...
For the reaction 2 Al + 3 H,SO -3H, + A1, (SO), how many grams of sulfuric acid, H2SO4, are needed to react completely with 51.9 g of aluminum, Al? 100 mass: 1/100 0/100 Consider the reaction. heat 2 Al(s) + Fe,0,(3) ***, ALO3(s) + 2 Fe(1) If 17.7 kg Al reacts with an excess of Fe,Og, how many kilograms of A1, O, will be produced? mass of A1,03 produced:
Most questions answered within 3 hours.
-
Where is the error in this code sequence?
String s1 = "Hello";
String s2 = "ello";...
asked 10 months ago -
Financial data for Joel de Paris, Inc., for last year
follow:
Joel de Paris, Inc.
Balance...
asked 10 months ago -
Consider this reaction:
Al2(SO4)3 (aq)+ BaCl3
(aq) Al2Cl6 (aq)- +
3BaSO4(s) . What is the...
asked 10 months ago -
Suppose that Savneet is considering increasing her
recent random sample from 20 car rentals to 40...
asked 10 months ago -
Trucks arrive at an unloading terminal at an average rate of 120
per hour.
Trucks arrive...
asked 10 months ago -
Why are methanol and ethanol completely soluble in water while
octanol is not very little soluble....
asked 10 months ago -
A facilities manager at a university reads in a research report
that the mean amount of...
asked 10 months ago -
When the CuSO4 is rehydrated by adding water to the anhydrous
compound, is this an endothermic...
asked 10 months ago -
A ray of sunlight is passing from diamond into crown glass; the
angle of incidence is...
asked 10 months ago -
A block of mass 0.249 kg is placed on top of a light, vertical
spring of...
asked 10 months ago -
how do the kidneys compensate in the presences of acidosis
a) trigger hyperventilate
b) reserve acid...
asked 10 months ago -
Question 501 pts
The rental rate of capital to the firm increases. Which of the
following...
asked 10 months ago