ebapps/portal/execute/tabs/tabAction?tab tab group id- 11 Chem. 1411 Study Guide

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ebapps/portal/execute/tabs/tabAction?tab tab group id- 11 Chem. 1411 Study Guide Exam 2.2018 Spring - Compatibility Mode - Saved to this PC gn Layout References Mailings Review View Help Tell me what you want to do Heading 2 Styles ?.H.I| 1Normal Heading 1 Title :E. 1No Spac- Fort Paragraph 14. Definition of Electron Affinity 15. Definition of Octet rule. 16. Lattice energy: based on Coulomb's Law II. Sample questions 1. How many moles of NO2 are needed to form 5.24 moles of NO if there is plenty of water present? 3 NO2(8)+H20(0) 2 HNO30)+NOG) A) 15.72 moles NO: B) 25.3 moles NO D) 5.63 moles NO2E) 1.83 moles NO c) 8.44 moles NO 2. How many grams of NO are formed when 6.21 moles of NO2 are reacted? 3 NO2(g)+ H20() 2 HNO3(ag)+ NO(E) A) 19.9 g NO B) 27.9 g NO C)62.1 g NO D)3.59 gNO E) 11.7 g NO 3. If 14.01 g sample of N2 reacts with 4.02 g of H2 to form ammonia (NH3), what is the mass of ammonia formed? A) 34.02 g B) 11.10 g C)17.01 g D) 30.02g E) 23.07 g 4. The chemical equation shows that carbonic acid is decomposed to form water and carbon dioxide by heating. What is the mass of carbon dioxide formed from 12.40 g of carbonic acid? H2CO3-H20 + CO2 A)7.58 g B)8.80 g 5. How many milliliters of a 0.294 M Lioil solution contain 0.223 moles of LiOH? C) 2.20 g D) 6.20 g ts Get Microsoft C

Explanation / Answer

Ans 2

Moles of NO2 = 6.21 mol

From the stoichiometry of the reaction

3 mol NO2 produces = 1 mol NO

6.21 mol NO2 produces = 6.21/3 = 2.07 mol NO

Mass of NO formed = Moles x molecular weight

= 2.07 mol x 30 g/mol

= 62.1 g

Option C is the correct answer

Ans 3

Mass of N2 = 14.01 g

Moles of N2 = mass/molecular weight

= 14.01g / 28g/mol

= 0.500357 mol

Mass of H2 = 4.02 g

Moles of H2 = mass/molecular weight

= 4.02g / 2g/mol

= 2.01 mol

Balanced chemical equation

N2 + 3H2 = 2NH3

1 mol N2 reacts with = 3 mol H2

0.500357 mol N2 reacts with = 3*0.500357

= 0.1667 mol H2

We have 2.01 mol H2 which is greater than 0.1667 mol H2

H2 is excess reactant

N2 is limiting reactant

Moles of NH3 formed

= 2 mol NH3 x 0.500357 mol N2 / 1 mol N2

= 1.000714 mol

Mass of NH3 formed = Moles x molecular weight

= 1.000714 mol x 17 g/mol

= 17.01 g

Option C is the correct answer

Ans 4

From the stoichiometry of the reaction

62 g H2CO3 produces = 44 g CO2

12.40 g H2CO3 produces = 44*12.40/62

= 8.8 g CO2

Option B is the correct answer

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