Moles - University of Leicester
... 3) Find the relative atomic masses for the elements and enter them in the third column 4) Perform the calculation in the fourth column (i.e. divide the value in column 2 by that in column 1). 5) To determine the test ratio, take the smallest number in column 4 and divide each of the column 4 values ...
... 3) Find the relative atomic masses for the elements and enter them in the third column 4) Perform the calculation in the fourth column (i.e. divide the value in column 2 by that in column 1). 5) To determine the test ratio, take the smallest number in column 4 and divide each of the column 4 values ...
Test - Angelfire
... INSTRUCTIONS: You will be expected to communicate your knowledge and understanding of chemical principles in a clear and logical manner. Your steps and assumptions leading to a solution must be written in the spaces below the questions. Answers must include units where appropriate and be given to th ...
... INSTRUCTIONS: You will be expected to communicate your knowledge and understanding of chemical principles in a clear and logical manner. Your steps and assumptions leading to a solution must be written in the spaces below the questions. Answers must include units where appropriate and be given to th ...
II. Masses of Atoms
... • A MOLECULE OF CARBON MONOXIDE, CO, HAS ONE ATOM OF OXYGEN WHILE A MOLECULE OF CARBON DIOXIDE, CO2, HAS TWO. IN A SAMPLE OF CO CONTAINING 1 G OF CARBON, 1.33 G OF OXYGEN WILL COMBINE WITH THE CARBON TO FORM THE MOLECULE. WHAT IS THE MASS OF OXYGEN IN A SAMPLE OF CO2 CONTAINING 1 G OF CARBON? A.1.33 ...
... • A MOLECULE OF CARBON MONOXIDE, CO, HAS ONE ATOM OF OXYGEN WHILE A MOLECULE OF CARBON DIOXIDE, CO2, HAS TWO. IN A SAMPLE OF CO CONTAINING 1 G OF CARBON, 1.33 G OF OXYGEN WILL COMBINE WITH THE CARBON TO FORM THE MOLECULE. WHAT IS THE MASS OF OXYGEN IN A SAMPLE OF CO2 CONTAINING 1 G OF CARBON? A.1.33 ...
Unit 1 Student Booklet
... Chemists do not work with amounts of individual atoms or molecules. These particles are far too small to see or mass. Balances or scales do not measure mass in terms of atomic mass units. Chemists need a practical unit that relates mass, in grams, with the number of particles. We will use the word p ...
... Chemists do not work with amounts of individual atoms or molecules. These particles are far too small to see or mass. Balances or scales do not measure mass in terms of atomic mass units. Chemists need a practical unit that relates mass, in grams, with the number of particles. We will use the word p ...
Chemistry
... transitions will produce unique absorption spectra for each element. When the electron returns from an excited (high energy state) to a lower energy state, energy is emitted in only certain wavelengths of light, producing an emission spectra. C 4.8x Atomic Structure Electrons, protons, and neutrons ...
... transitions will produce unique absorption spectra for each element. When the electron returns from an excited (high energy state) to a lower energy state, energy is emitted in only certain wavelengths of light, producing an emission spectra. C 4.8x Atomic Structure Electrons, protons, and neutrons ...
Matter
... • 2 or more elements chemically combined in a definite ratio • Properties are different from those of elements formed from • Homogeneous • Broken into elements by chemical decomposition reaction • Formulas have 2 or more uppercase letters ...
... • 2 or more elements chemically combined in a definite ratio • Properties are different from those of elements formed from • Homogeneous • Broken into elements by chemical decomposition reaction • Formulas have 2 or more uppercase letters ...
The Mole - Piscataway High School
... composition? Percent composition – percent by mass of each element in the compound Percent by mass of an element in a compound is the number of grams of the element divided by the mass in grams of the compound multiplied by 100% Equation: Percent composition from Chemical formula ...
... composition? Percent composition – percent by mass of each element in the compound Percent by mass of an element in a compound is the number of grams of the element divided by the mass in grams of the compound multiplied by 100% Equation: Percent composition from Chemical formula ...
Chemistry Reference Table Review
... 82. The volume of a gas is 4.00 liters at 293 K and constant pressure. For the volume of the gas to become 3.00 liters, the Kelvin temperature must be equal to (1) 3.00 x 293 / 4.00 (2) 4.00 x 293 / 3.00 (3) 3.00 x 4.00 / 293 (4) 293 / 3.00 x 4.00 83. What are two properties of most nonmetals? (1) h ...
... 82. The volume of a gas is 4.00 liters at 293 K and constant pressure. For the volume of the gas to become 3.00 liters, the Kelvin temperature must be equal to (1) 3.00 x 293 / 4.00 (2) 4.00 x 293 / 3.00 (3) 3.00 x 4.00 / 293 (4) 293 / 3.00 x 4.00 83. What are two properties of most nonmetals? (1) h ...
Unit B: Matter and Chemical Change
... Adapted from Figure 2.18 Page 112 Science Focus 9 Laws: Describe and summarize what happens in a natural system. Theories: Imaginative ways to explain why something happens in a natural system. Models: Help picture structures or processes that cannot be directly seen. Observations: Thousands of obse ...
... Adapted from Figure 2.18 Page 112 Science Focus 9 Laws: Describe and summarize what happens in a natural system. Theories: Imaginative ways to explain why something happens in a natural system. Models: Help picture structures or processes that cannot be directly seen. Observations: Thousands of obse ...
Key Concept 1: An atom is the smallest unit of an element that
... Key Concept 10: The reactivity of an atom is how easily and readily its valence electrons interact with the valence electrons of other atoms. Atoms of metals have a tendency to transfer electrons to nonmetals when they react. Atoms of nonmetals have a tendency to gain or share electrons when they re ...
... Key Concept 10: The reactivity of an atom is how easily and readily its valence electrons interact with the valence electrons of other atoms. Atoms of metals have a tendency to transfer electrons to nonmetals when they react. Atoms of nonmetals have a tendency to gain or share electrons when they re ...
key concepts of matter
... Key Concept 1: During a chemical reaction, the atoms of substances rearrange themselves into a new configuration forming new substances. The reactants (or the energy and atoms or molecules of the original substance) combine to produce products (or the energy, atoms, and molecules of the new substanc ...
... Key Concept 1: During a chemical reaction, the atoms of substances rearrange themselves into a new configuration forming new substances. The reactants (or the energy and atoms or molecules of the original substance) combine to produce products (or the energy, atoms, and molecules of the new substanc ...
Exam #2
... 65. The solubility of CuI is 2 x 10¯6 molar. What is the solubility product constant, Ksp, for CuI? (A) 1.4 x 10¯3 (B) 2 x 10¯6 (C) 4 x 10¯12 (D) 2 x 10¯12 (E) 8 x 10¯18 66. MnS(s) + 2 H+ <===> Mn2+ + H2S(g) At 25 °C the solubility product constant, Ksp, for MnS in 5 x 10¯15 and the acid dissociatio ...
... 65. The solubility of CuI is 2 x 10¯6 molar. What is the solubility product constant, Ksp, for CuI? (A) 1.4 x 10¯3 (B) 2 x 10¯6 (C) 4 x 10¯12 (D) 2 x 10¯12 (E) 8 x 10¯18 66. MnS(s) + 2 H+ <===> Mn2+ + H2S(g) At 25 °C the solubility product constant, Ksp, for MnS in 5 x 10¯15 and the acid dissociatio ...
3 CHEMICAL THERMODYNAMICS
... becomes more dilute, γi approaches 1. The activity generally is assumed to be 1 for the dilute solutions of concern here. 3. For pure solids or liquids in equilibrium with a solution, (i) = 1. 4. For gases in equilibrium with a solution, (i) = γi Piwhere Pi = is the partial pressure of the gas in at ...
... becomes more dilute, γi approaches 1. The activity generally is assumed to be 1 for the dilute solutions of concern here. 3. For pure solids or liquids in equilibrium with a solution, (i) = 1. 4. For gases in equilibrium with a solution, (i) = γi Piwhere Pi = is the partial pressure of the gas in at ...
4. chemical kinetics
... If concentration is higher, the number of molecules per unit volume is, more and the number of active collisions increases. According to collision theory, rate of reaction increases with increase in the number of ...
... If concentration is higher, the number of molecules per unit volume is, more and the number of active collisions increases. According to collision theory, rate of reaction increases with increase in the number of ...
Unit B Chemistry Unit study guide
... halogens, noble gases as well as metals vs nonmetals Why are lanthanides and actinides on bottom? What are the only two liquids? Where are the gasses? Which element is in a group of its own? Which element is needed for substances to burn? Mendeleev did such a great job creating his periodic table be ...
... halogens, noble gases as well as metals vs nonmetals Why are lanthanides and actinides on bottom? What are the only two liquids? Where are the gasses? Which element is in a group of its own? Which element is needed for substances to burn? Mendeleev did such a great job creating his periodic table be ...
Key - GCC
... attractive forces between water molecules.) Boiling water is endothermic because heat must be absorbed (go into) the system in order to break the intermolecular forces that hold molecules together. ...
... attractive forces between water molecules.) Boiling water is endothermic because heat must be absorbed (go into) the system in order to break the intermolecular forces that hold molecules together. ...
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.