logging in or signing up Empirical & Molecular Formula Calculations mreisley Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: Embed: Flash iPad Dynamic Copy Does not support media & animations Automatically changes to Flash or non-Flash embed WordPress Embed Customize Embed URL: Copy Thumbnail: Copy The presentation is successfully added In Your Favorites. Views: 408 Category: Education License: All Rights Reserved Like it (0) Dislike it (0) Added: January 08, 2012 This Presentation is Public Favorites: 0 Presentation Description A brief comparison of empirical and molecular formula definitions is presented, followed by several worked out examples of how to determine empirical and molecular formulas. Comments Posting comment... Premium member Presentation Transcript Determining Empirical Formulas (from masses): Determining Empirical Formulas ( from masses ) Convert each mass to moles. Divide all answers by the smallest mole number. Use the quotients as subscripts in the empirical formulaWhat is the empirical formula for a compound if a 2.50 g sample contains 0.900 g of calcium and 1.60 g of chlorine? : What is the empirical formula for a compound if a 2.50 g sample contains 0.900 g of calcium and 1.60 g of chlorine? CaCl 2PowerPoint Presentation: Tip: If your division of mole numbers gives you a .5 or .25 or .33…, multiply all your mole numbers by a common factor, so that you have whole numbers for your subscripts.PowerPoint Presentation: What is the empirical formula of a compound that has 7.22g Ni, 2.53g P, and 5.25g O? Ni 3 P 2 O 8Determining Empirical Formulas (from percentages): Determining Empirical Formulas ( from percentages ) Assume total mass is 100.g => Change “%” to grams Convert each mass to moles. Divide all answers by the smallest mole number. Use the quotients as subscripts in the empirical formulaA compound has a percentage composition of 40.0% C, 6.71% H, and 53.3% O. What is the empirical formula?: A compound has a percentage composition of 40.0% C, 6.71% H, and 53.3% O. What is the empirical formula? CH 2 O Assume total mass is 100. gDetermining Molecular Formulas: Determining Molecular Formulas Calculate the Empirical Formula (if necessary) Calculate the formula mass of the empirical formula Divide the Molecular Mass by the Empirical Mass => Quotient is the multiplier for the subscripts in the Empirical FormulaAscorbic acid (vitamin C) has a percentage composition of 40.9% carbon, 4.58% hydrogen, and 54.5% oxygen. Its molecular mass is 176.1 u. What is its molecular formula? : Ascorbic acid (vitamin C) has a percentage composition of 40.9% carbon, 4.58% hydrogen, and 54.5% oxygen. Its molecular mass is 176.1 u. What is its molecular formula? C 3 H 4 O 3 Assume total mass is 100. g Empirical Formula One More Step…Finding the Molecular Mass…: Finding the Molecular Mass… Empirical Formula = C 3 H 4 O 3 Empirical Mass = 88.0 u Multiply by the subscripts Molecular Formula = C 6 H 8 O 6 You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.
Empirical & Molecular Formula Calculations mreisley Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: Embed: Flash iPad Dynamic Copy Does not support media & animations Automatically changes to Flash or non-Flash embed WordPress Embed Customize Embed URL: Copy Thumbnail: Copy The presentation is successfully added In Your Favorites. Views: 408 Category: Education License: All Rights Reserved Like it (0) Dislike it (0) Added: January 08, 2012 This Presentation is Public Favorites: 0 Presentation Description A brief comparison of empirical and molecular formula definitions is presented, followed by several worked out examples of how to determine empirical and molecular formulas. Comments Posting comment... Premium member Presentation Transcript Determining Empirical Formulas (from masses): Determining Empirical Formulas ( from masses ) Convert each mass to moles. Divide all answers by the smallest mole number. Use the quotients as subscripts in the empirical formulaWhat is the empirical formula for a compound if a 2.50 g sample contains 0.900 g of calcium and 1.60 g of chlorine? : What is the empirical formula for a compound if a 2.50 g sample contains 0.900 g of calcium and 1.60 g of chlorine? CaCl 2PowerPoint Presentation: Tip: If your division of mole numbers gives you a .5 or .25 or .33…, multiply all your mole numbers by a common factor, so that you have whole numbers for your subscripts.PowerPoint Presentation: What is the empirical formula of a compound that has 7.22g Ni, 2.53g P, and 5.25g O? Ni 3 P 2 O 8Determining Empirical Formulas (from percentages): Determining Empirical Formulas ( from percentages ) Assume total mass is 100.g => Change “%” to grams Convert each mass to moles. Divide all answers by the smallest mole number. Use the quotients as subscripts in the empirical formulaA compound has a percentage composition of 40.0% C, 6.71% H, and 53.3% O. What is the empirical formula?: A compound has a percentage composition of 40.0% C, 6.71% H, and 53.3% O. What is the empirical formula? CH 2 O Assume total mass is 100. gDetermining Molecular Formulas: Determining Molecular Formulas Calculate the Empirical Formula (if necessary) Calculate the formula mass of the empirical formula Divide the Molecular Mass by the Empirical Mass => Quotient is the multiplier for the subscripts in the Empirical FormulaAscorbic acid (vitamin C) has a percentage composition of 40.9% carbon, 4.58% hydrogen, and 54.5% oxygen. Its molecular mass is 176.1 u. What is its molecular formula? : Ascorbic acid (vitamin C) has a percentage composition of 40.9% carbon, 4.58% hydrogen, and 54.5% oxygen. Its molecular mass is 176.1 u. What is its molecular formula? C 3 H 4 O 3 Assume total mass is 100. g Empirical Formula One More Step…Finding the Molecular Mass…: Finding the Molecular Mass… Empirical Formula = C 3 H 4 O 3 Empirical Mass = 88.0 u Multiply by the subscripts Molecular Formula = C 6 H 8 O 6