Organic Chemistry Chapter 4 Study Guide

Chapter 3

1. 1 atom of X = atomic mass (amu) 1 mole f X=atomic mass in grams 1 mole of something = 6.022 x 1023 units of that substance 1 mole of a compound =66.022 x 1023 atoms

6.022 x 1023 amu =1 g

2. What is the mass of 6 atoms of Fe?

Answer: 6 atoms of Fe x 55.85 amu÷atom of Fe x 1 g of Fe÷6.022 x 1023 amu =

3. How many atoms does it take to make 1 g of Gold (Au)?

Answer: 197.0 g Au =1 mole of Au

1 g of Au=? 1 mole of Au/197 g Au x 1 g of Au= 0.0051 or 5.10 x 10-3 moles of Au

1 mole of Au contains 6.022 x 1023 atoms of Au

5.10 x 10-3 moles of Au = 6.022 x 1023 atoms of Au/1
Consider the following reaction: [pic]

What mass of CCl4 will be formed if 1.20 moles of methane react with 1.28 moles of chlorine?

The percent yield is a ratio of the ____________ yield to the _____________ yield, multiplied by 100%.

20. 0.1156 g of a compound reacted with oxygen gives 0.1638 g CO2 and 0.1676 g of H2O, rest is nitrogen. What is the formula of the compound?

CO2 = 44.01 g/mole H2O=18.02 g/mole

Fraction of C in CO2: mass of C/total mass of CO2= 12.01g of C/44.01g of CO2

0.1638 g of CO2 x12.01g of C/44.01g of CO2 = 0.0447 g of C

0.0447g of C/0.1156 g compound x 100 = 38.67% C

Same way calculate % H = 16.22% H

= 45.11% N

Convert % to moles, find the ratio in whole number, empirical formula.

21. Balancing Equation:

Reactants = Products

CH4 (g) + 2O2(g) = CO2 (g)+ 2H2O(l)

1C, 4H + 4 O = 1C, 2O, 4H, 2O

1mole of CH4+ 2 moles of O2= 1 mole of CO2+ 2 moles of H2O

16 g of CH4+ 32 x 2 g of O2 = 44 g of CO2+ 36 g of H2O

80 g reactants=80g Products

6.022 x 1023 + 2 x 6.022 x 1023 =6.022 x 1023 +2 x 6.022 x 1023