A student combines 15.0 g FeS, with excess 02, which react according to the balanced equation shown below. From this information and using the molar masses of the reactants and products, what information can the student calculate about the reaction? 4FES,(s) + 150,(g)→ 2Fe,0, + 8SO,(g) The theoretical yield, actual yield, and percent yield of each product a O b The theoretical yield of each product The actual yield of each product The theoretical yield of Fe,03, but not SO3

A student combines 15.0 g FeS, with excess 02, which react according to the balanced equation shown below. From this information and using the molar masses of the reactants and products, what information can the student calculate about the reaction? 4FES,(s) + 150,(g)→ 2Fe,0, + 8SO,(g) The theoretical yield, actual yield, and percent yield of each product a O b The theoretical yield of each product The actual yield of each product The theoretical yield of Fe,03, but not SO3

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...

See similar textbooks

Similar questions

_ P4(s) + _ O2(g) –→_ P¾O10(s) o balance this reaction equation, first write correct formulas for the reactants and products, leaving the stoichiometric coefficients blank. Ve will balance P first. How many Pa molecules are needed to balance P for each P,010?
Determine the limiting reactant (LR) and the Theoretical Yield (in g) of nitrogen that can be formed from 58.0 g N2O4 and 40.0 g N2H4. Some possibly useful molar masses are as follows: N2O4= 92.02 g/mol, N2H4= 32.05g/mol. N2O4(l) + 2 N2H4 --------> (l) 3 N2(g) + 4 H2O(g)
DATA Record all masses to the maximum number of Run 1 Run 2 sig figs 200°C 400°C 1. Mass of beaker 81.061 27.986 2. Mass of beaker + NaHCO3 85.457 32.267 3. Initial mass of NaHCO3 4.476 4.292 Mass of beaker plus products after heating. 4. 84.3 80 30.742 5. Mass of product (actual yield) There are three theoretically possible chemical reactions that could occur during the thermal decomposition of baking soda. 1) sodium bicarbonate (s) → sodium hydroxide (s) + carbon dioxide (g) 2) sodium bicarbonate (s) → sodium oxide (s) + carbon dioxide (g) + water (g) 3) sodium bicarbonate (s)→ sodium carbonate (s) + carbon dioxide (g) + water (g)
Here is the organic chemical equation for the reaction of an inorganic compound B with a big organic molecule A that might be found in plant or animal fats or oils: A + NB X HO OH OH + 3 HO Complete this description of the reaction by answering the questions in the table below. What is the chemical formula of B? What is the stoichiometric coefficient N? Are there any special reaction conditions X needed? (You can assume the reaction mixture is gently heated, and X is not "A") If you said there were special reaction conditions needed, what is X? In the drawing area below, draw the chemical structure of A. Ú 0 0 yes no Click and drag to start drawing a structure. 00 X Ś X :0 Ś
For the following reaction, 0.343 moles of sulfuric acid are mixed with 0.223 moles of calcium hydroxide. sulfuric acid (aq) + calcium hydroxide(s) → calcium sulfate(s) + water(l) What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of calcium sulfate that can be produced? Amount = moles
Consider the reaction. 2 Pb(s) + O₂(g) - 2 PbO (s) An excess of oxygen reacts with 451.4 g of lead, forming 361.0 g of lead(II) oxide. Calculate the percent yield of the reaction. percent yield:
39.06 g C6H6) + (120.00 g O2) ------------> (132.03 g CO2) + (x g H2O) Assuming that both reactants are completely used up, calculate the numerical value of x. Place your answer in the box
Which formula can be used to calculate the percent yield? (Theoretical yield + actual yield) x 100 O (Actual yield + theoretical yield) x 100 (Amount of reactants + amount of products) x 100 O (Amount of products + amount of reactants) × 100
2 N₂O5(g) --> 4 NO₂(g) + O₂(g) True/False: The equation is already balanced as it is written.
Use the References to access important values if needed for this question. For the following reaction, 0.127 moles of barium hydroxide are mixed with 0.119 moles of sulfuric acid. barium hydroxide (aq) + sulfuric acid (aq) → barium sulfate(s) + water (l) What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of barium sulfate that can be produced? Amount = moles
For the following reaction: C3Hg(g) + O2(g) ————> CO2(g) + H2O(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams for each starting reactant c). calculate the theoretical yield of CO2(g) in grams d). calculate the percent yield if the actual yield was 10.7 grams
A reaction has a theoretical yield of 76.5 grams of a product, and a percent yield of 41.2 %. What is the actual yield (in g) of this product in this reaction?