Question 22 of 29> < 0/100 Combining 0.371 mol Fe, O, with excess carbon produced 16.6 g Fe. Fe2O3+3C 2 Fe 3 CO 0/100 What is the actual yield of iron in moles? 100/100 Correct actual yield: mol 100/100 What is the theoretical yield of iron in moles? Correct 0/100 theoretical yield: mol What is the percent yield? 73/100 In Progress 0/100 percent yield: 0% help privacy policy terms of use contact us about us careers

Question 22 of 29> < 0/100 Combining 0.371 mol Fe, O, with excess carbon produced 16.6 g Fe. Fe2O3+3C 2 Fe 3 CO 0/100 What is the actual yield of iron in moles? 100/100 Correct actual yield: mol 100/100 What is the theoretical yield of iron in moles? Correct 0/100 theoretical yield: mol What is the percent yield? 73/100 In Progress 0/100 percent yield: 0% help privacy policy terms of use contact us about us careers

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A chemist setup a synthesis of phosphorus trichloride by mixing 12.0gP with 35.0gCl _(2) and obtained 42.4gPCl _(3). Calculate the percentage yield of this compound. P(s)+Cl_(2)(g)->PCl _(3)(l) Please type answer note write by hend
Give the theoretical yield, in moles, of CO2 from the reaction of 0.60 moles of C8H18 with 40.00 moles of O2. 2C8H18+25O2 ---> 16CO2 + 18H2O
Calculate the theoretical yield of (in grams) of Ca3(PO3)2 when 7.15 g of calcium hydroxide reacts with excess phosphours acid. Be sure to balance the chemical reaction before beginning. ____Ca(OH)2 + ____H3PO3 ---> ____ H2O + ____Ca3(PO3)2
For the following reaction: C3H8(g) + O2(g) ------> CO2(g) + H2O(g) Q: Calculate the theoretical yield of CO2(g) in gram
A sample of an industrial waste water is analyzed and found to contain 16.5ppb Fe2+. How many grams of iron could be recovered from 1.81×103 kg of this waste water? Answer:_______ grams Fe
A chemist carries out the reaction below and obtains 3.45g of iron Fe (Fe, MW=55.845g/mol). Fill in the blanks below to determine the percent yield of the reaction when 8.30g of Fe2O3 (MW= 159.69g/mol) and 3.50g of CO (MW=28.01G/mol)were used in the reaction. Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g) Note that for two of the blanks, will be the same answer. 1. What would be the mass in grams of Fe produced based on the mass of Fe2O3 used? answer: (blank) 2. What would be the mass in grams of Fe produced based on the mass of CO used? answer: (blank) 3. What is the theoretical yield of Fe in grams? answer: (blank) 4. What is the limiting reagent? Enter the formula of compound. answer: (blank) 5. What is the percent yield of this reaction? answer: (blank)
When the equation? PbS+? O2 →? PbO+? SO2is balanced, the coefficients are
Quesiton 19 Calcium carbonate reacts with acetic acid following the UNBALANCED chemical reaction: CaCO3+ CH3COOH→Ca(CH3COO)2+ CO2+ H2O How many moles of CO2are produced by the decomposition of 240 g CH3COOH? You must balancethe equation before completing the problem. A. 1.0 moles CO2 B. 2.0 moles CO2 C. 3.0 moles CO2 D. 4.0 moles CO2 E. 5.0 moles CO2
Please give both answer... 19) (a) Isolating iron metal in a metallurgical process has the chemical equation shown below: 3 CO (g) + Fe2O3 (s) -----> 2 Fe (s) + 3 CO2 (g) If 134 mg of carbon monoxide are reacted with 32.70 cg of iron(III) oxide solid, how many grams of Iron metal can be created? State which reactant is limiting and which is in excess (b) In a metallurgical practice run from part (a), 0.1257 g of Fe are collected. What is the % Yield?
Mass of Na2CO3.H2O (g) = 2.12g (g) Mass of the CaCl2.2H2O (g) = 1.98g Mass of the top funnel + filter paper (g) = 15.85g Mass of top funnel + filter paper + CaCO3 collected (g) = 17.81g CaCl2 + Na2CO3 ==== CaCo3 + 2NaCl Theoretical yield in moles and grams? Moles of reagent in excess left unreacted? Mass of precipitate? Experimental yield? Percent yield?
South Africa is one of the world's largest ion ore producers. From the reaction below, answer the following questions on the iron ore extraction Fe2O3(s) + c(s) - Fe(l) + CO2(g) a. Give the correct chemistry name for Fe2O3 and CO2. B. If 9888.8 g of Fe2O3 and 1258.2g of C react, determine which reagents is the limiting reactant/reagents of the reaction. C. Calculate the theoretical yield of the reaction. D. If the foreman on side obtained 6.12g of Fe, for the reaction described in b above, what is the %yield of the reaction. E. The product Fe is in liquid format. Do you think this is correct or not and justify why you think so?
Chemistry PLEASE HELP! THANK YOU 1. Define hydrate. 2. Name each of the following hydrates. A. CuCl2·3H2O ____________________________________ C. BeSO4·4H2O ____________________________________ 3. Complete the following equation and balance. B. LiClO4·3H2O → 4. A hydrate of Na2B4O7 · x H2O was heated to obtain the following data. Empty crucible 14.550 g Crucible + hydrate 19.552 g Crucible + contents after first heating 17.199 g after second heating 17.188 g A. Calculate the mass of the anhydrous Na2B4O7 obtained after heating . B. Convert this mass of Na2B4O7 to moles of Na2B4O7. C. Calculate the mass of water driven off by the heating. D. Convert this to moles of water. C. Find the mole ratio of H2O to Na2B4O7. D. What is the formula of this hydrate? Na2B4O7 ·? H2O ___________