(Cl) in magnesium chloride (Mg1Cl2). Chapter 3 Set #1. Practice Problem #6. Determine the percent by mass of Carbon (C) , Hydrogen (H) and. Oxygen (O)...
Chapter 3 Set #1 Practice Problem #1: A 56.00 gram sample of Nitrogen gas combines completely with 12.00 grams of Hydrogen gas to form Ammonia gas. 1N2
+
3H2
--->
2N1H3
______ ______ _______ What is the mass of Ammonia formed?
Practice Problem #2: In a reaction, 60.00 grams of Sodium combines with an excess of Chlorine gas to form 250.00 grams of Sodium Chloride. 2Na + ______
1Cl2 ______
--->
2Na1Cl1 _______
What mass of Chlorine gas is used in the reaction?
Chapter 3 Set #1 Practice Problem #3: Magnesium Metal reacts with Chlorine gas to form Magnesium Chloride. 1Mg(s) + 1Cl2(g) ---> 1Mg1Cl2(s) 1000 atoms of Magnesium is Reacted with 2000 molecules of Chlorine a. How many total atoms are involved in the reaction? b. How many molecules of Magnesium Chloride are formed?
Chapter 3 Set #1 Practice Problem #4 Determine the percent by mass of aluminum (Al) and fluorine (F) in aluminum fluoride (Al1F3)
Chapter 3 Set #1
Chapter 3 Set #1
Practice Problem #5 Determine the percent by mass of magnesium (Mg) and chlorine (Cl) in magnesium chloride (Mg1Cl2)
Practice Problem #6 Determine the percent by mass of Carbon (C) , Hydrogen (H) and Oxygen (O) in a molecule of Sucrose (C12H24O11)
Chapter 3 Set #1 Practice Problem #7 Calculate the percent by mass of Hydrogen (H) and Oxygen (O) in: a. Water (H2O) b. Hydrogen Peroxide (H2O2)
Chapter 3 Set #1 Practice Problem #8 Calculate the percent by mass of Copper (Cu) in the following copper chloride compounds: a. Copper (I) Chloride (CuCl) b. Copper (II) Chloride (CuCl2)
Chapter 3 Set #1 Practice Problem #9 Calculate the percent by mass of Carbon (C) and Oxygen (O) in: a. Carbon Monoxide (CO) b. Carbon Dioxide (CO2)
Chapter 3 Set #2 Practice Problem #1: (Use Table 2 on page 80) Calculate the Following: Electrons a. The symbol for 8 electrons b. The mass of 8 electrons in kg
c. The charge of 8 electrons in Coulombs
d. The charge of 8 electrons in common charge
Chapter 3 Set #2
Chapter 3 Set #2 Practice Problem #2: (Use Table 2 on page 80) Calculate the Following: Protons a. The symbol for 8 protons
Practice Problem #3: (Use Table 2 on page 80) Calculate the Following: Neutrons a. The symbol for 8 neutrons
b. The mass of 8 protons
b. The mass of 8 neutrons
c. The charge of 8 protons in Coulombs
c. The charge of 8 neutrons in Coulombs
d. The charge of 8 protons in common charge
d. The charge of 8 neutrons in common charge
Chapter 3 Practice Set #2
Chapter 3 Set #2 Practice Problem #4
Practice Problem #4: (Use Table 2 on page 80)
Oxygen is element number eight (8) Oxygen has 8 protons (p+), 8 electrons (e-), and 8 neutrons (no) a. Using your data from questions 1-3, calculate the mass in kilograms of one oxygen atom b. Using your data from questions 1-3, calculate the total charge in Coulombs (C) for one oxygen atom c. Using your data from questions 1-3, calculate the total common charge for one oxygen atom
Element name! Isotope name ! Protons! Electrons! Neutrons!
= = = = =
Practice Problem #6
Practice Problem #5
Iron-56 Protons! Electrons! Neutrons! = = = = =
= = = = =
Chapter 3 Practice Set #2
Chapter 3 Practice Set #2
Element name! Isotope name ! Protons (p+)! Electrons (e-)! Neutrons (n0)!
Element name! Isotope name ! Protons! Electrons! Neutrons!
Element name! Isotope name ! Protons! Electrons! Neutrons!
= = = = =
Iron-52 = = =
Protons! Electrons! Neutrons!
= = =
Chapter 3 Practice Set #2
Chapter 3 Practice Set #2 Practice Problem #7
Practice Problem #8
Uranium-234
Uranium-238
Protons! Electrons! Neutrons!
Protons! Electrons! Neutrons!
= = =
= = =
Carbon-12
12 6
C
Number of Neutrons in both Carbon isotopes = _____, ______
Chapter 3 Practice Set #2 Practice Problem #9
Chapter 3 Practice Set #2 Practice Problem #10
Potassium-39
Uranium-238 Number of Neutrons in both Potassium isotopes = ______, _____
Number of Neutrons in both Uranium isotopes = _____, ______
