Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Gravimetric Analysis of AgNO3 A student attempts to determine the correct equation to describe the thermal decomposition reaction of AgNO3. Heating 4.7885 g of AgNO3 (i.e. about 5 g) gave 3.0406 g of residue. The following three equations have been determined as the most likely possibilities: 1. 2 AgNO3(s) → 2 AgNO2(s) + O2(g) 2. 2 AgNO3(s) → 2 Ag(s) + 2 NO2(g) + O2(g) -> 3. 4 AgNO3(s) → 2 Ag2O(s) + 4 NO2(g) + O2(g) -> sito ince fill out fornill, bubora bilo to Using the data provided and the stoichiometry of the above equations, determine which of the equations correctly describes the thermal decomposition of AgNO3. If Initial mass of AgNO3 = 4.7885 g Initial number of moles of AgNO3 = .02819mol - Table 1. Calculation of % Discrepancy Possible Percent Expected #moles Expected mass (g) residueat pitone (theoretical) open cidi (theoretical) osals Discrepancy bus codesup olve or benisido If AgNO₂ Giste abiz all to If Ag 2

Gravimetric Analysis of AgNO3 A student attempts to determine the correct equation to describe the thermal decomposition reaction of AgNO3. Heating 4.7885 g of AgNO3 (i.e. about 5 g) gave 3.0406 g of residue. The following three equations have been determined as the most likely possibilities: 1. 2 AgNO3(s) → 2 AgNO2(s) + O2(g) 2. 2 AgNO3(s) → 2 Ag(s) + 2 NO2(g) + O2(g) -> 3. 4 AgNO3(s) → 2 Ag2O(s) + 4 NO2(g) + O2(g) -> sito ince fill out fornill, bubora bilo to Using the data provided and the stoichiometry of the above equations, determine which of the equations correctly describes the thermal decomposition of AgNO3. If Initial mass of AgNO3 = 4.7885 g Initial number of moles of AgNO3 = .02819mol - Table 1. Calculation of % Discrepancy Possible Percent Expected #moles Expected mass (g) residueat pitone (theoretical) open cidi (theoretical) osals Discrepancy bus codesup olve or benisido If AgNO₂ Giste abiz all to If Ag 2

Chemistry
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
icon
Related questions
Question
How to calculate expected moles and expected mass? Information provided in the picture.
Gravimetric Analysis of AgNO3 A student attempts to determine the correct equation to describe the thermal decomposition reaction of AgNO3. Heating 4.7885 g of AgNO3 (i.e. about 5 g) gave 3.0406 g of residue. The following three equations have been determined as the most likely possibilities: dista ifree eli suhoa bil.. Using the data provided and the stoichiometry of the above equations, determine which of the equations correctly describes the thermal decomposition of AgNO3. 1. 2 AgNO3(s) → 2 AgNO2(s) + O2(g) 2. 2 AgNO3(s) → 2 Ag(s) + 2 NO2(g) + O2(g) 3. 4 AgNO3(s) → 2 Ag2O(s) + 4 NO2(g) + O2(g) If AgNO₂ If Ag If Ag₂0 Table 1. Calculation of % Discrepancy Possible Expected #moles Expected mass (g) Percent residuettone (theoretical) nonoscidi (theoretical) osoals Discrepancy uste oblast on to aaam istnomsqs stil bes nouzsup erolvórg sal or bepistdo 1. Initial mass of AgNO3 4.7885 g Initial number of moles of AgNO3 = .02819mol 2. your979216 IositoreenT Calculations. Show all calculations, formulae and units below; give your final answers to the appropriate number of significant figures and place in chart above. = Molar mass of AgNO3. M= (1x 107.87) + (1x 14.01) + (3x 16.00) = 169.88g/mol Moles of AgNO3. n = m M qka fe ad as solit tegut al anc n = 4.7885g 169.88 g/mol = 0.02819 mol noitzu
Transcribed Image Text:Gravimetric Analysis of AgNO3 A student attempts to determine the correct equation to describe the thermal decomposition reaction of AgNO3. Heating 4.7885 g of AgNO3 (i.e. about 5 g) gave 3.0406 g of residue. The following three equations have been determined as the most likely possibilities: dista ifree eli suhoa bil.. Using the data provided and the stoichiometry of the above equations, determine which of the equations correctly describes the thermal decomposition of AgNO3. 1. 2 AgNO3(s) → 2 AgNO2(s) + O2(g) 2. 2 AgNO3(s) → 2 Ag(s) + 2 NO2(g) + O2(g) 3. 4 AgNO3(s) → 2 Ag2O(s) + 4 NO2(g) + O2(g) If AgNO₂ If Ag If Ag₂0 Table 1. Calculation of % Discrepancy Possible Expected #moles Expected mass (g) Percent residuettone (theoretical) nonoscidi (theoretical) osoals Discrepancy uste oblast on to aaam istnomsqs stil bes nouzsup erolvórg sal or bepistdo 1. Initial mass of AgNO3 4.7885 g Initial number of moles of AgNO3 = .02819mol 2. your979216 IositoreenT Calculations. Show all calculations, formulae and units below; give your final answers to the appropriate number of significant figures and place in chart above. = Molar mass of AgNO3. M= (1x 107.87) + (1x 14.01) + (3x 16.00) = 169.88g/mol Moles of AgNO3. n = m M qka fe ad as solit tegut al anc n = 4.7885g 169.88 g/mol = 0.02819 mol noitzu
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Green Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS