Question

Antimony (Sb, 121.8 g/mol) is a metal that is used in applications such as fire retardant...

Antimony (Sb, 121.8 g/mol) is a metal that is used in applications such as fire retardant
materials, electronics, bullets, lead shot, and in lead-free solders. The primary source of
antimony in nature is its sulfide, stibinite (Sb2S3, 339.7 g/mol). Pure antimony is obtained by
heating pulverized stibnite with scrap iron (Fe, 55.85 g/mol), and drawing off the molten
antimony from the bottom of the reaction vessel.
Sb2S3 + 3 Fe ------> 2Sb + 3FeS
(FeS = 87.91 g/mol). Suppose that 6.0 kg of stibinite and 2.5 kg of iron are heated together
to give 2.0 kg of Sb metal.
(a) What is the limiting reactant?
(b) Calculate the % excess of the excess reactant?
(c) Calculate the fractional conversion based on Sb2S3?
(d) Calculate the yield as kg Sb produced/kg Sb2S3 fed to the reactor?
(e) Calculate the degree of completion of the reaction (i.e., how close to complete reaction).

Engineering   Chemical-Engineering   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g) A reaction mixture initially contains...
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g) A reaction mixture initially contains 0.208 mol FeS and 0.678 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?
In the production of iron metal, a mixture of 228g P4 (MW=154 g/mol) and 205g Cl2...
In the production of iron metal, a mixture of 228g P4 (MW=154 g/mol) and 205g Cl2 (MW=71 g/mol) are heated together the following reaction takes place to form PCl5 (MW=208 g/mol): P4(g)+10 Cl2(g)---> 4PCl5(g). a) what is the limiting reactant? b) How many grams of PCl5 can be produced? c) If 157 g of Pcl5 is actually obtained what is the percent yield of the reaction?
1. In the following reaction, 451.4 g of lead reacts with excess oxygen forming 365.8 g...
1. In the following reaction, 451.4 g of lead reacts with excess oxygen forming 365.8 g of lead(II) oxide. Calculate the percent yield of the reaction. 2Pb(s)+O2(g) = 2PbO(s) 2. Assuming an efficiency of 32.60%, calculate the actual yield of magnesium nitrate formed from 119.8 g of magnesium and excess copper(II) nitrate. Mg + Cu(NO3)2 = Mg(NO3)2 + Cu 3. Combining 0.282 mol of Fe2O3 with excess carbon produced 18.8 g of Fe. Fe2O3 + 3C = 2Fe + 3CO...
1. The specific heat of iron metal is 0.450 J/g⋅K. How many J of heat are...
1. The specific heat of iron metal is 0.450 J/g⋅K. How many J of heat are necessary to raise the temperature of a 1.05 −kg block of iron from 28.0 ∘Cto 85.0 ∘C? 2. A 1.80-g sample of phenol (C6H5OH) was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/∘C. The temperature of the calorimeter plus contents increased from 21.36∘Cto 26.37∘C. A. Write a balanced chemical equation for the bomb calorimeter reaction. B. What is the heat...
Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen in the following equation. N2H4(g)...
Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen in the following equation. N2H4(g) +O 2(g) →N2(g) + 2 H2O(g) The reaction, at 50% yield, produces 4.0 moles of N2. What was the mass of hydrazine used? Assume that O2 is in excess. A) 64 g B) 0.063 g C) 260 g D) 32.0 g 42) 43) Which of the following is the lowest temperature? A) 313 K B) 37°C C) 54°F D) All of these temperatures are...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT