6. (6.0 pts) If 15.00 g of FeBr3 is combined with 8.50 g of H2SO4, how many grams of Fe2(SO4)3 will be produced?
7. (2.0 pts) If only 6.25 g of Fe2(SO4)3 is actually produced, what is the percent yield?
6.
7. Now, actual yield in grams (given) = 6.25 g.
As we know, percentage yield
6. (6.0 pts) If 15.00 g of FeBr3 is combined with 8.50 g of H2SO4, how...
If 15.00 g of FeBr3 is combined with 8.50 g of H2SO4, how many grams of Fe2(SO4)3 will be produced?
Phosphoric acid can be prepared from calcium phosphate according to the following reaction: Ca3(PO4)2 (s) + 3 H2SO4 (l) → 3 CaSO4 (s) + 2 H3PO4 (l) 310. g/mol 98.0 g/mol 136 g/mol 98.0 g/mol [a] If 0.664 mole of Ca3(PO4)2 are combined with 1.53 mole of H2SO4, how many grams of H3PO4 can be produced? [4 pts] [b] If 62.6 g of H3PO4 is actually produced in the above reaction, what is the percent yield for the reaction? [2...
I need help Consider the following equations: H2(g) + O2(g) → 2H2O(g) 1. How many grams of water will be produced if there 5.0 gram of oxygen? 2. How many moles of water will be produced if there are 2.0 moles of hydrogen? 3. You conducted the above experiment in the lab and found that the 100 moles of water are produced, how many grams you actually produced of water? 4. If you correctly done number 3, then it is...
I need help Consider the following equations: H2(g) + O2(g) → 2H2O(g) 1. How many grams of water will be produced if there 5.0 gram of oxygen? 2. How many moles of water will be produced if there are 2.0 moles of hydrogen? 3. You conducted the above experiment in the lab and found that the 100 moles of water are produced, how many grams you actually produced of water? 4. If you correctly done number 3, then it is...
Question 7 How many grams of KAl(SO4)2 • 12 H2O (474.39 g/mol) can be produced from 1.83 g of aluminum (27 g/mol)? (report 2 digits after the decimal point) __________ g KAl(SO4)2 • 12 H2O (s) Question 8: If you recover 27.7 g of alum from question 7, what is the percent yield of this process?Question 8 (report as a %, not in decimal form; 2 digits before the decimal point) __________ % yield
pts) Consider the following balanced equation: Na2SO4 (aq) + 2AgNO3 (aq) → Ag2SO4 (9) + 2NaNO3(aq) a. How many grams of Ag2SO4 result from the reaction of 6.764 g of Na SO, with 15.00 g of AgNO3? b. If the reaction has a 57.3% percent yield, how much Ag2SO4 was actually made? pts) How many grams of O, reacted if 306 kcal are released in the following reaction? CH(g) + 2O2(g) - CO2(g) + 2H2O(l) + 213 kcal
A 75.0 mL solution of 0.240 M Na3PO4 is combined with excess CaCl2. How many grams of calcium phosphate will form as a precipitate if all of the Na3PO4 is consumed in the reaction? What is the percent yield for the reaction if 2.13 g of calcium phosphate is produced?
How many grams of carbon tetrachloride, CCL4, can be prepared from 100.0 g of CS2, and 100.0 grams of Cl2? what is the percent yield of the reaction if 65.0 g of CCL4 was actually produced?
questions 35,36,37,38, and 39 all refer to the problem below In the reaction of iron (III) sulfate and barium hydroxide, Fe2(SO4)3 + 3Ba(OH)2 -> 3BaSO4 + 2Fe(OH)3. If 20.0 g of Fe2(SO4)3 is mixed with 20.0 g of Ba(OH)2. Molar masses Fe2(SO4)3 = 399.91 Ba(OH)2 = 171.35 Fe(OH)3 = 106.88 39. If one of the chem 10 students ran the reaction as stated in problem 35 and got 7.052 g of Ba(OH)2, what is the percentage yield for the reaction...
Question 6 1 pts Suppose you are measuring the mass of a solid sample on a balance using a weigh boat. You record the data in a table. Mass of weigh boat 3.117 g Mass of weigh boat and sample 9.405 g What is the mass, in grams, of the solid sample? Question 7 2 pts Sulfuric acid, H2SO4, is an important industrial chemical (typically used for fertilizers and making of many other chemicals), typically synthesized in a multi-step process....