Question 3 of 8SubmitAccording to the balanced reaction below, calculate the moles of NH: gas that formwhen 4.2mol of N2H4 liquid completely reacts:3N2H4(1) →4NH:(g) + N:(g)STARTING AMOUNTADD FACTORANSWERRESET*( )33.216.022 x 102317.0428.02432.064.25.616.8g N2H.mol NH3mol N2H4g N2mol N2g NH,

Answered: Image /qna-images/answer/9904dcd6-51ef-492b-989c-73872e55ef68.jpg

Answered: Question 3 of 8 According to the…

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

Ca(OH)2 (s) + H₂S(g) →→→ CaS (s) + 2H₂O(l) In the reaction above, calcium hydroxide and hydrogen sulfide react to form calcium sulfide and water. If you combine 11 g of hydrogen sulfide with 15 g of calcium hydroxide: 1) Which reactant is limiting? [Select] 2) Calculate the number of moles of calcium sulfide produced if the percent yield is 100%. [Select] ✓ mol Cas
Calculate the theoretical yield in grams All3 from the complete reaction of 18.3 grams Al according to the following balanced chemical equation: 2 Al(s) + 3 12(s) → 2 All;(s) -> STARTING AMOUNT ANSWER RESET ADD FACTOR * ( ) 18.3 407.7 3 1.47 277 26.98 0.678 1 138 mol All3 g All3 g/mol All; g/mol Al g Al mol Al WIDA A AR 2.
Question 86 of 97 According to the balanced reaction below, calculate the moles of NH; gas that form when 4.2 mol of N2H. liquid completely reacts: 3 N2H.(0)→ 4 NH3(g) + N2(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 4.2 28.02 5.6 17.04 16.8 3.2 32.06 6.022 x 10 mol NH3 mol N2H4 g N2 g NH3 g N2H4 mol N2 MacBook Air
How many moles of H2SO4 are required to completely react with 7.20 mol of Al according to the balanced chemical reaction: 2 Al(s) + 3 H:SO-(aq) → Al:(SO-):(aq) + 3 H2(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 21.6 26.98 6.022 x 1023 2 7.20 2.40 3.60 1 98.08 342.14 3 2.02 10.8 g Al mol Al:(SO.)s g Al:(SO4)s mol Hz mol Al g H2SO. mol H2SO4 g H2 I
If baking soda (sodium hydrogen carbonate) is heated strongly, the following reaction occurs: 2NaHCO3(s) - Na₂CO3 (s) + H₂O(g) + CO₂ (g) Calculate the mass in grams of sodium carbonate (Na2CO3) that will remain if a 1.52-g sample of sodium hydrogen carbonate (NaHCO3) is heated. This equation is balanced. Edit View Insert Format Tools Table 12pt Paragraph IM BI SI T² ✓ TE
How many grams of N2 are needed to completely (stoichiometrically) react with 222 g of Br2 ? N2 + 3 Br2 2 NB13 + 44.0 kJ The molar mass of Br2 is g and the molar mass of N2 is mol Br2 (2.22 x 102 g Br2)(- mol Br2 g Br2 mol N2 mol Br2 (-- -) = mol N2 mol Br2 g N2 mol N2 (-- -) = |v g N2 mol N2 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.38 х 100 h. 3.26 x 103 i. 44.0 j. 1.33 x 102 k. 9.77 x 103 I. 4.44 x 102 m. 6.66 x 10² n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved Cc. absorbed dd. exothermic ee. endothermic
Consider the gaseous reaction at 347 C N2 + 3H2 ---> 2NH3 if 2.00 mole of N2 and 3.00 mole of H2 react, a) which of the two reactants is the limiting reagent b) if the reaction goes completely, how many grams of NH3 should be produced c) calculate the percent yield of 2.50 g of NH3 are actually obtained
In the following reaction, oxygen is the excess reactant.SiCl4 + O2 → SiO2 + Cl2The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2 1 150 g 200 g 49.2 g 2 75 g 50 g 25.2 g Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work. Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction. Source StylesNormal
Question 3 of 15 Submit How many moles of H2SO. are required to completely react with 7.20 mol of Al according to the balanced chemical reaction: Al(s) + 3 H:SO(aq) → Al:(SO.):(aq) + 3 H2(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 6.022 x 1023 7.20 3.60 342.14 2.02 21.6 98.08 2.40 26.98 2 10.8 1 g H2SO, g Al:(SO.)s mol Al:(SO.)s g H2 mol H2SO4 mol Al mol H2 g Al
In the following reaction, oxygen is the excess reactant.SiCl4 + O2 → SiO2 + Cl2The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2 1 120 g 240 g 38.2 g 2 75 g 50 g 25.2 g Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work. Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction.

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS