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3.17 What is the mass in grams of a single atom of each of the following elements? (a) Hg, (b) Ne.

This study guide covers calculating atomic and molecular masses, empirical formulas, and balancing chemical equations in Chemistry. Learn to solve stoichiometry problems and determine limiting reagents. Practice with examples involving various elements and compounds. Enhance your understanding of chemistry concepts and problem-solving skills with this comprehensive resource.

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3.17 What is the mass in grams of a single atom of each of the following elements? (a) Hg, (b) Ne.

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  1. Chapter3 3.17 What is the mass in grams of a single atom of each of the following elements? (a) Hg, (b) Ne. 3.20 How many atoms are present in 3.14 g of copper (Cu)? 3.23 Calculate the molecular mass or formula mass (in amu) of each of the following substances: (a) CH4 , (b) NO2 , (c) SO3 , (d) C6H6 , (e) NaI, (f) K2SO4 , (g) Ca3(PO4 )2 . 3.50 What are the empirical formulas of the compounds with the following compositions? (a) 40.1 percent C, 6.6 percent H, 53.3 percent O, (b) 18.4 percent C, 21.5 percent N, 60.1 percent K. 3.60 Balance the following equations using the method outlined in Section 3.7: (a) N2O5N2O4 + O2 (b) KNO3KNO2 + O2 (c) NH4NO3N2O + H2O (d) NH4NO2N2 + H2O (e) NaHCO3Na2CO3 + H2O +CO2

  2. 3.83 Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2 ), a dark-brown gas: 2NO(g) + O2 2NO2 (g) In one experiment 0.886 mole of NO is mixed with 0.503 mole of O2 . Calculate which of the two reactants is the limiting reagent. Calculate also the number of moles of NO2 produced. 3.92 Ethylene (C 2H4), an important industrial organic chemical, can be prepared by heating hexane (C6H14) at 800 C: C6H14 C2H4 + other products If the yield of ethylene production is 42.5 percent, what mass of hexane must be reacted to produce 481g of ethylene?

  3. Chapter 4 4.21

  4. 4.54

  5. Chapter 5

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