Last Name Professor BEAMER First Name
... The “aq” in the reactants tells you that water is present. Therefore, you must determine the solubility of iron(III) chloride. ...
... The “aq” in the reactants tells you that water is present. Therefore, you must determine the solubility of iron(III) chloride. ...
Ch 2 Atoms, Molecules, and Ions
... - A molecule is a finite arrangement of atoms chemically bonded together. The molecule has particular chemical bonds, as well a 3D structure. Generally, all of the atoms in a molecule are nonmetals. - The molecular formula shows the proportions of each atom. The structural formula shows how atoms ar ...
... - A molecule is a finite arrangement of atoms chemically bonded together. The molecule has particular chemical bonds, as well a 3D structure. Generally, all of the atoms in a molecule are nonmetals. - The molecular formula shows the proportions of each atom. The structural formula shows how atoms ar ...
Chapter 2_Application Problems
... have one oxygen atom and two hydrogen atoms – correct; according to Dalton, atoms combine together in compounds in small whole-number ratios, so that you could describe a compound by describing the number of atoms of each element in a molecule. He used this idea to explain why compounds obey the Law ...
... have one oxygen atom and two hydrogen atoms – correct; according to Dalton, atoms combine together in compounds in small whole-number ratios, so that you could describe a compound by describing the number of atoms of each element in a molecule. He used this idea to explain why compounds obey the Law ...
CHEM 1411 EXAM I (Chapters 1, 2, 3): 25
... Stoichiometrey. Method One (ratio approach): From the equation, the involving species, 2 Al(OH)3 and 6 H2O with coefficients 2 and 6 respectively, tell us that for 2 moles of Al(OH)3 it produces 6 moles of H2O. According to this proportion or ratio, 5.500 m ...
... Stoichiometrey. Method One (ratio approach): From the equation, the involving species, 2 Al(OH)3 and 6 H2O with coefficients 2 and 6 respectively, tell us that for 2 moles of Al(OH)3 it produces 6 moles of H2O. According to this proportion or ratio, 5.500 m ...
Congratulations! You have signed up for AP Chemistry for this year
... AP stands for “Advanced Placement” and AP Chemistry is the equivalent of a college chemistry class. There are some chemistry principles that are important that you remember from Pre-AP Chemistry, so I have compiled some practice notes and assignments that will equip you for the beginning of the year ...
... AP stands for “Advanced Placement” and AP Chemistry is the equivalent of a college chemistry class. There are some chemistry principles that are important that you remember from Pre-AP Chemistry, so I have compiled some practice notes and assignments that will equip you for the beginning of the year ...
Halogens - Cronodon
... In elemental form, the halogens exist as simple molecular compounds, containing diatomic molecules (i.e. molecules of two atoms): F2, Cl2, Br2, I2. Fluorine is a paleyellow gas of F2 molecules, chlorine is a greenish-yellow gas of Cl2 molecules. Bromine is a reddish-orange liquid of Br2 molecules wi ...
... In elemental form, the halogens exist as simple molecular compounds, containing diatomic molecules (i.e. molecules of two atoms): F2, Cl2, Br2, I2. Fluorine is a paleyellow gas of F2 molecules, chlorine is a greenish-yellow gas of Cl2 molecules. Bromine is a reddish-orange liquid of Br2 molecules wi ...
Chapter 8 Quantities in Chemical Reactions
... 1. LO: Recognize the numerical relationship between chemical quantities in a balanced chemical equation. 2. LO: Carry out mole-to-mole conversions between reactants and products based on the numerical relationship between chemical quantities in a balanced chemical equation. 3. LO: Carry out mass-to- ...
... 1. LO: Recognize the numerical relationship between chemical quantities in a balanced chemical equation. 2. LO: Carry out mole-to-mole conversions between reactants and products based on the numerical relationship between chemical quantities in a balanced chemical equation. 3. LO: Carry out mass-to- ...
CHEM 102 FINAL EXAM WINTER 07-08
... 7. Polyamides can be produced from a. two monomers, one containing two amino groups, the other containing two carboxylic acid groups. b. one monomer, containing one amino and one carboxylic acid group. c. one monomer, containing two amide groups. d. either a or b above. ANSWER: d 8. Which statement ...
... 7. Polyamides can be produced from a. two monomers, one containing two amino groups, the other containing two carboxylic acid groups. b. one monomer, containing one amino and one carboxylic acid group. c. one monomer, containing two amide groups. d. either a or b above. ANSWER: d 8. Which statement ...
Writing and Balancing Chemical Equations
... One methane molecule and two oxygen molecules react to yield one carbon dioxide molecule and two water molecules. One dozen methane molecules and two dozen oxygen molecules react to yield one dozen carbon dioxide molecules and two dozen water molecules. One mole of methane molecules and 2 mole ...
... One methane molecule and two oxygen molecules react to yield one carbon dioxide molecule and two water molecules. One dozen methane molecules and two dozen oxygen molecules react to yield one dozen carbon dioxide molecules and two dozen water molecules. One mole of methane molecules and 2 mole ...
Chemistry-5th-Edition-Brady-Solution-Manual
... Since we know that the formula is CH4, we know that one fourth of the total mass due to the hydrogen atom constitutes the mass that may be compared to the carbon. Hence we have 0.33597 g H 4 = 0.083993 g H and 1.00 g assigned to the amount of C-12 in the compound. Then it is necessary to realize t ...
... Since we know that the formula is CH4, we know that one fourth of the total mass due to the hydrogen atom constitutes the mass that may be compared to the carbon. Hence we have 0.33597 g H 4 = 0.083993 g H and 1.00 g assigned to the amount of C-12 in the compound. Then it is necessary to realize t ...
Chapter 8
... calculated from atomic masses water = H2O = 2(1.008 amu) + 16.00 amu = 18.02 amu • 1 mole of H2O will weigh 18.02 g, therefore the molar mass of H2O is 18.02 g • 1 mole of H2O will contain 16.00 g of oxygen and 2.02 g of hydrogen ...
... calculated from atomic masses water = H2O = 2(1.008 amu) + 16.00 amu = 18.02 amu • 1 mole of H2O will weigh 18.02 g, therefore the molar mass of H2O is 18.02 g • 1 mole of H2O will contain 16.00 g of oxygen and 2.02 g of hydrogen ...
Final Review
... c. Definite volume; shape of container; no intermolecular attractions d. Volume and shape of container; no intermolecular attractions e. Volume and shape of container; strong intermolecular attractions 102. Which transformation is evaporation? a. liquid ---> solid d. solid ---> gas b. liquid ---> ga ...
... c. Definite volume; shape of container; no intermolecular attractions d. Volume and shape of container; no intermolecular attractions e. Volume and shape of container; strong intermolecular attractions 102. Which transformation is evaporation? a. liquid ---> solid d. solid ---> gas b. liquid ---> ga ...
Thermodynamics
... In a perfect crystal (diamond), the entropy at 0K is 0 J/K. Can use third law to develop standard molar entropy values ...
... In a perfect crystal (diamond), the entropy at 0K is 0 J/K. Can use third law to develop standard molar entropy values ...
2009 Chemistry Midterm Review Packet
... c) 0.50 mol H3PO4 (41 g); 1.5 mol HCl (55 g) d) o.50 mol NaHCO3 (42 g) 11. molar mass 15. a) 1.03 molCuCl2 b) 0.0735 mol NiCl2 c) 0.240 mol NaOH d) 0.250 mol HCl 17. 500. g H20 19. 18.3 g CO2; 11.7 g CO 21. 4.704 g O2 23. 0.437 g N2; 0.250 g O2; 0.562 g H2O 26. 3.26 x 10-3 g Cl2 31. use masses given ...
... c) 0.50 mol H3PO4 (41 g); 1.5 mol HCl (55 g) d) o.50 mol NaHCO3 (42 g) 11. molar mass 15. a) 1.03 molCuCl2 b) 0.0735 mol NiCl2 c) 0.240 mol NaOH d) 0.250 mol HCl 17. 500. g H20 19. 18.3 g CO2; 11.7 g CO 21. 4.704 g O2 23. 0.437 g N2; 0.250 g O2; 0.562 g H2O 26. 3.26 x 10-3 g Cl2 31. use masses given ...
Equilibrium
... contains more reactant than product. In principle, almost all reactions are reversible to some extent under the right conditions. In practice, one set of components is often so favored that the other set cannot be detected. If one set of components (reactants) is completely converted to new substanc ...
... contains more reactant than product. In principle, almost all reactions are reversible to some extent under the right conditions. In practice, one set of components is often so favored that the other set cannot be detected. If one set of components (reactants) is completely converted to new substanc ...
Unit 2 matter - Kowenscience.com
... • ex. Water molecules are composed of hydrogen and oxygen atoms Pure compounds are made up of only one type of molecule! ...
... • ex. Water molecules are composed of hydrogen and oxygen atoms Pure compounds are made up of only one type of molecule! ...
MASS RELATIONS and STOICHIOMETRY
... Before you balance chemical equations, you have to understand how these equations are written. Writing chemical equations: 1. Write the formulas of reactants on the left side and products on the right side of the equation. 2. Use an arrow to separate reactants from products (The arrow means “to prod ...
... Before you balance chemical equations, you have to understand how these equations are written. Writing chemical equations: 1. Write the formulas of reactants on the left side and products on the right side of the equation. 2. Use an arrow to separate reactants from products (The arrow means “to prod ...
(3.3 × 10!4) + (2.52 × 10!2) = (3.3 × 10!4) × (2.52 × 10!2)
... A pure substance has well defined physical and chemical properties. Pure substances can be classified as elements or compounds. Compounds can be further reduced into two or more elements. Elements consist of only one type of atom. They cannot be decomposed or further simplified by ordinary means. ...
... A pure substance has well defined physical and chemical properties. Pure substances can be classified as elements or compounds. Compounds can be further reduced into two or more elements. Elements consist of only one type of atom. They cannot be decomposed or further simplified by ordinary means. ...
Semester I CP Chemistry Review
... 42. How many moles are in the following: b. 22 grams of N2O 22g N2O 1 mole N2O = 0.5 mole 44g N2O b. 342 grams of Al2(SO4)3 342 g Al2(SO4)3 1 mole Al2(SO4)3 = 1 mole 342 g Al2(SO4)3 c. 10 grams of Fe2O3 10g Fe2O3 1 mole Fe2O3 = 0.06 mole 160 g Fe2O3 ...
... 42. How many moles are in the following: b. 22 grams of N2O 22g N2O 1 mole N2O = 0.5 mole 44g N2O b. 342 grams of Al2(SO4)3 342 g Al2(SO4)3 1 mole Al2(SO4)3 = 1 mole 342 g Al2(SO4)3 c. 10 grams of Fe2O3 10g Fe2O3 1 mole Fe2O3 = 0.06 mole 160 g Fe2O3 ...
FINAL REVIEW Vella Name_______________ Period___
... 4. a. What volume in milliliters of .25 M sodium chromate will react with 75.0 mL of .100 M copper (II) chloride to form copper(II) chromate and sodium chloride ? ...
... 4. a. What volume in milliliters of .25 M sodium chromate will react with 75.0 mL of .100 M copper (II) chloride to form copper(II) chromate and sodium chloride ? ...
THERMOCHEMISTRY or Thermodynamics
... Heating/Cooling Curve for Water Note that T is constant as ice melts or water boils ...
... Heating/Cooling Curve for Water Note that T is constant as ice melts or water boils ...
Stoichiometry
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.