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1. Calculate the molar mass of each of the following: a. (NH4)3PO4 b. BaF2 c. CH₂Cl₂ d. Ca(C₂H3O2)2

1. Calculate the molar mass of each of the following: a. (NH4)3PO4 b. BaF2 c. CH₂Cl₂ d. Ca(C₂H3O2)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...
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Name Period Unit 4 Review Worksheet #1 Molar Mass and Percent Composition Date Directions: Complete on a separate piece of paper. 1. Calculate the molar mass of each of the following: a. (NH4)3PO4 b. BaF2 c. CH₂Cl₂ d. Ca(C₂H3O2)2 2. Calculate each of the following quantities: a. Mass in grams of 0.68 mol KMnO4 b. Mass in kilograms of 4.6 x 1021 molecules of NO₂ c. Moles of Fe(CIO4)3 in a 15.8 kg sample 3. Calculate the number of moles and formula units in 78.9 g of sodium perchlorate. 4. What is the percent composition of each in element in NH4HCO3? 5. What is the percent composition of Mn in KMnO4? 6. Ammonium nitrate is a common fertilizer. Agronomist base the effectiveness of fertilizers on their nitrogen content. Calculate the mass percent of N in ammonium nitrate. 7. How many moles are in 15 g of lithium? 8. How many grams are in 88.1 moles of magnesium? 9. How many atoms are in 98.3 grams of aluminum hydroxide? 10. How many carbon dioxide molecules are there in 3.25 moles of carbon dioxide? 11. What is the mass of 3.40 moles of Cu(NO3)2? 12. A chemist determines that 1.26 g of iron reacts with 0.54 g of oxygen to form rust [iron (III) oxide]. What is the percent composition of each element in the new compound? 13. In an experiment, a student took a 12.2 g sample of table salt and chemically separated the chlorine from the sodium. He determined that there were 5.2 g of chlorine in the sample. What is the percent composition of each element in the table salt sample?
Transcribed Image Text:Name Period Unit 4 Review Worksheet #1 Molar Mass and Percent Composition Date Directions: Complete on a separate piece of paper. 1. Calculate the molar mass of each of the following: a. (NH4)3PO4 b. BaF2 c. CH₂Cl₂ d. Ca(C₂H3O2)2 2. Calculate each of the following quantities: a. Mass in grams of 0.68 mol KMnO4 b. Mass in kilograms of 4.6 x 1021 molecules of NO₂ c. Moles of Fe(CIO4)3 in a 15.8 kg sample 3. Calculate the number of moles and formula units in 78.9 g of sodium perchlorate. 4. What is the percent composition of each in element in NH4HCO3? 5. What is the percent composition of Mn in KMnO4? 6. Ammonium nitrate is a common fertilizer. Agronomist base the effectiveness of fertilizers on their nitrogen content. Calculate the mass percent of N in ammonium nitrate. 7. How many moles are in 15 g of lithium? 8. How many grams are in 88.1 moles of magnesium? 9. How many atoms are in 98.3 grams of aluminum hydroxide? 10. How many carbon dioxide molecules are there in 3.25 moles of carbon dioxide? 11. What is the mass of 3.40 moles of Cu(NO3)2? 12. A chemist determines that 1.26 g of iron reacts with 0.54 g of oxygen to form rust [iron (III) oxide]. What is the percent composition of each element in the new compound? 13. In an experiment, a student took a 12.2 g sample of table salt and chemically separated the chlorine from the sodium. He determined that there were 5.2 g of chlorine in the sample. What is the percent composition of each element in the table salt sample?
111 and Name Period Date 1/2001-1s (0)-001 + (a) 05 +00 si Thermochemical Equations Worksheet 1. How much heat is released when 6.44 g of sulfur reacts with excess oxygen according to the following equation? 2S (s) + 302 (g) → 2SO3 (g) AH--791.4 kJ (3) M 2. What is the heat change when 4.72 g of carbon reacts with excess oxygen according to the following equation? C(s) + O2(g) → CO₂ (g) AH = -393.5 kJ angenbyd as ditiw saimoidlog 28€ 10897 01 butoon ai sod doum woll 8 Snoitsups gniwollot di of LI 08.ST-HA (2) 78H (3) 78+ (g) H 3. What is the heat change when 1.48 g of chlorine reacts with excess phosphorus according to the following equation? 2P (s) + 5Cl2 (g) → 2 PCls (g) AH = -886 kJ 1961 nagorbyd to go.81 nodw leol ai jead doum wol e Shoitaupe galwollot or HA (DOHS (g) 0+ (g) (HS 4. How much heat is gained when 5.81 g of carbon reacts with excess hydrogen gas according to the following equation? 6C (s, graphite) + 3 H2 (g) → C6H6 (g) AH = 49.03 kJ oxo diw arouon ainomms to g 0.4I now sgasilo teori odatdW 01 noitenps gorwellol sh WOH-=HA () Oct à (2) 0/ 5. What is the heat change when 4.77 g of ethanol reacts with excess oxygen according to the following equation? C₂H5OH (g) + 302 (g) → 2CO2 (g) + 3H₂O (g) AH = -1366.7 kJ
Transcribed Image Text:111 and Name Period Date 1/2001-1s (0)-001 + (a) 05 +00 si Thermochemical Equations Worksheet 1. How much heat is released when 6.44 g of sulfur reacts with excess oxygen according to the following equation? 2S (s) + 302 (g) → 2SO3 (g) AH--791.4 kJ (3) M 2. What is the heat change when 4.72 g of carbon reacts with excess oxygen according to the following equation? C(s) + O2(g) → CO₂ (g) AH = -393.5 kJ angenbyd as ditiw saimoidlog 28€ 10897 01 butoon ai sod doum woll 8 Snoitsups gniwollot di of LI 08.ST-HA (2) 78H (3) 78+ (g) H 3. What is the heat change when 1.48 g of chlorine reacts with excess phosphorus according to the following equation? 2P (s) + 5Cl2 (g) → 2 PCls (g) AH = -886 kJ 1961 nagorbyd to go.81 nodw leol ai jead doum wol e Shoitaupe galwollot or HA (DOHS (g) 0+ (g) (HS 4. How much heat is gained when 5.81 g of carbon reacts with excess hydrogen gas according to the following equation? 6C (s, graphite) + 3 H2 (g) → C6H6 (g) AH = 49.03 kJ oxo diw arouon ainomms to g 0.4I now sgasilo teori odatdW 01 noitenps gorwellol sh WOH-=HA () Oct à (2) 0/ 5. What is the heat change when 4.77 g of ethanol reacts with excess oxygen according to the following equation? C₂H5OH (g) + 302 (g) → 2CO2 (g) + 3H₂O (g) AH = -1366.7 kJ
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