A 0.046 mol sample of water (molar mass: 18.01 g/mol) is reacted with excess of Mg3N2 in the following reaction: Mg3N2 + 3 H20 → 2 NH3 + 3 MgO In this experiment, 1.60 g of MgO (molar mass: 40.3 g/mol) was obtained. What is the percent yield of the reaction? 71.5 % O A. 77.5 % В. 86.3 % C. 88.1 % D. 64.7 % E.

A 0.046 mol sample of water (molar mass: 18.01 g/mol) is reacted with excess of Mg3N2 in the following reaction: Mg3N2 + 3 H20 → 2 NH3 + 3 MgO In this experiment, 1.60 g of MgO (molar mass: 40.3 g/mol) was obtained. What is the percent yield of the reaction? 71.5 % O A. 77.5 % В. 86.3 % C. 88.1 % D. 64.7 % E.

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

Hydrazine (N₂H4), a component of some rocket fuels, is industrially produced using the following reaction. 2 NH3 + H₂O2 → N₂H4 + 2 H₂O Molar masses (in g mol-¹) NH3 17.03 Number % H₂O₂ 34.02 N₂H4 32.05 A: What is the percent atom economy for the synthesis of hydrazine? Enter a percentage accurate to 3 significant figures. Do not enter the "%" symbol. The E-factor is greater than 1. The E-factor is less than 1. H₂O 18.02 B: What is the E-factor when a reaction between 170.3 g of NH3 and 170.1 g of H₂O₂ produces 160.3 g of N₂H4 and 90.1 g of water? The E-factor is 0.
Menthol is composed of C,H, and O. A 0.1005g sample of menthol is combusted, producing 0.2829g of CO2 and 0.1159g of H20. What is the empirical formula for menthol? If menthol has a molar mass of 156g/mol, what is its molecular formula?
A chemist carries out this reaction, starting with 30.5 g of C6H6 and an excess Br2: C6H6(l) + Br2 (l) --> C6H5Br (g) + HBr (g) What is the theoretical yield of C6H5Br for this reaction?
Consider the reaction between HCl and O2: 4HCl(aq) + O2(g) -> 2H2O(l)+2Cl2(g) When 15.4 g of HCl reacts with 18.2 g of O2, 14.3 g og Cl2 are collected a) Determine the limiting reactant b) Deteremine the theoretical yield of Cl2 c) Determine the % yield of Cl2
||| O CHEMICAL REACTIONS Theoretical yield of chemical reactions Th... S CD33 Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H₂O). What is the theoretical yield of water formed from the reaction of 33.2 g of hydrobromic acid and 31.0 g of sodium hydroxide? Be sure your answer has the correct number of significant digits in it. 0-
8. Consider the following reaction: 5A + 3B --> 2C + 2D 10.0 moles of A and 6.00 moles of B reacted and produced 3.00 moles of D. What is the percent yield of product D in this reaction?
0 A reaction of 36.9 g of Na and 46.9 g of Br₂ yields 51.9 g of NaBr. What is the percent yield? 2 Na(s) + Br₂(g) - ->> 2 NaBr(s) percent yield:
C3H8(g) + O2(g) ------> CO2(g) + H2O(g) a. Balance the reaction: b. Determine the limiting reactant from 20.0 grams of 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:
25. Consider the balanced equation: 2N₂H4(g) + N₂04(8) 3N₂(g) + 4H₂O(g) Complete the table with the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product formed. If the num- ber of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made. mol N₂H4 || 3 mol N₂O4 2 5.5 mol N₂ 12.4 mol H₂O 8
Each step in the following process has a yield of 60.0%. CH4 + 4Cl₂ CCl₂ + 4HCI CCl₂ + 2 HF CC1₂F₂ + 2HCl The CCI, formed in the first step is used as a reactant in the second step. If 5.00 mol CH4 reacts, what is the total amount of HCI produced? Assume that Cl₂ and HF are present in excess. moles HCl: mol
What is the theoretical yield of HCI if 30.0 g of BCI3 and excess H20 are reacted according to the following balanced reaction? BC13(g) +3 H20(1) + H3BO3(s) + 3HCI(g) The following molar masses are: HCI = 36.46 g/mol BCI3 = 117.17 g/mol H2O = 18.02 g/mol
Synthesis of disulfur diclhoride S8 + 4Cl2 —> 4 S2 Cl2 0.7797 mol S8 and 1.410 mol Cl2 are combined to make S2Cl2 1.What is the limiting reactant? 2.How much excess reactant will be left 3. How many moles of product can be made