Chemistry exam review
... 2.1.5 Explain the relationships among pressure, temperature, volume, and quantity of gas, both quantitative and qualitative. 1. What happens to the pressure of a constant mass of gas at constant temperature when the volume is doubled? a. The pressure is doubled. b. The pressure remains the same. c. ...
... 2.1.5 Explain the relationships among pressure, temperature, volume, and quantity of gas, both quantitative and qualitative. 1. What happens to the pressure of a constant mass of gas at constant temperature when the volume is doubled? a. The pressure is doubled. b. The pressure remains the same. c. ...
An Introduction to Matter
... – A physical change is a change that does not alter the identity of the matter. – A chemical change is a change that does alter the identity of the matter. – A compound is a pure substance that can be decomposed by a chemical change into simpler substances – An element is a pure substance which can ...
... – A physical change is a change that does not alter the identity of the matter. – A chemical change is a change that does alter the identity of the matter. – A compound is a pure substance that can be decomposed by a chemical change into simpler substances – An element is a pure substance which can ...
Chemistry exam review
... 2. The gases helium, neon, and argon are in separate containers at 55°C. Which is true about the kinetic energy of the gases? a. Helium has the lowest mass and therefore the greatest kinetic energy. b. They each have a different kinetic energy. c. Argon has greatest mass and therefore the greatest ...
... 2. The gases helium, neon, and argon are in separate containers at 55°C. Which is true about the kinetic energy of the gases? a. Helium has the lowest mass and therefore the greatest kinetic energy. b. They each have a different kinetic energy. c. Argon has greatest mass and therefore the greatest ...
The collision theory of reactions
... At X (this is a very unstable arrangement and only lasts for a very short time). The enthalpy profile is shown as a single curve (this is only true for single-step reactions). Other reactions have several steps, so the enthalpy profile would show several steps, too. do problems for 10.1 ‘Rates of ...
... At X (this is a very unstable arrangement and only lasts for a very short time). The enthalpy profile is shown as a single curve (this is only true for single-step reactions). Other reactions have several steps, so the enthalpy profile would show several steps, too. do problems for 10.1 ‘Rates of ...
Equilibrium Constant - Faculty Server Contact
... dilution is used as the standard state; -- the activity of H2O = 1 at infinite dilution. The activity of water is related to the mole fraction of pure water, XH2O as follows: mH2O = moH2O + RTlnXH2O In most cases, we are dealing with dilute solutions and we can set the activity of H2O = 1. In more c ...
... dilution is used as the standard state; -- the activity of H2O = 1 at infinite dilution. The activity of water is related to the mole fraction of pure water, XH2O as follows: mH2O = moH2O + RTlnXH2O In most cases, we are dealing with dilute solutions and we can set the activity of H2O = 1. In more c ...
Figure 1.01a: (a.)The surface of a single grain of table salt.
... Using the mass percentage and molar mass to determine the mass of each element per mole of compound. Determine the # of moles of each element /mol compound. The integers of # of moles of each element are the subscript in the molecular formula. ...
... Using the mass percentage and molar mass to determine the mass of each element per mole of compound. Determine the # of moles of each element /mol compound. The integers of # of moles of each element are the subscript in the molecular formula. ...
Measuring Energy Changes In A Chemical Reaction Sept. 2016
... EVERY chemical reaction either releases energy to the surroundings (exothermic reactions) OR absorbs energy from the surrounding (endothermic reactions) We cannot measure the energy changes in the chemical reaction (the system) BUT we can easily measure the energy changes in the surroundings If we a ...
... EVERY chemical reaction either releases energy to the surroundings (exothermic reactions) OR absorbs energy from the surrounding (endothermic reactions) We cannot measure the energy changes in the chemical reaction (the system) BUT we can easily measure the energy changes in the surroundings If we a ...
Reading-Chem v Phys
... signify a physical change. Table salt (sodium chloride) is a white solid at room temperature. It can also exist in each of the three physical states. However, the temperatures at which the changes of state occur in sodium chloride are much higher than for the corresponding changes in water. Sodium c ...
... signify a physical change. Table salt (sodium chloride) is a white solid at room temperature. It can also exist in each of the three physical states. However, the temperatures at which the changes of state occur in sodium chloride are much higher than for the corresponding changes in water. Sodium c ...
writing and balancing equations
... • Hydrogen gas combined with Oxygen gas will produce Dihydrogen Monoxide liquid H 2 + O 2 H 2O • Should be: • H2(g) + O2(g) H2O(l) ...
... • Hydrogen gas combined with Oxygen gas will produce Dihydrogen Monoxide liquid H 2 + O 2 H 2O • Should be: • H2(g) + O2(g) H2O(l) ...
Chem 30A Fa_06 FE Review
... (a) SO3 : ___________________________________ (b) FeSO4: __________________________________ (c) HC2H3O2: _________________________________ (d) Ca3(PO4)2: __________________________________ (e) Hg2Cl2: ____________________________________ ...
... (a) SO3 : ___________________________________ (b) FeSO4: __________________________________ (c) HC2H3O2: _________________________________ (d) Ca3(PO4)2: __________________________________ (e) Hg2Cl2: ____________________________________ ...
know thy reference tables!
... (1) chemical formulas and mass numbers (2) chemical formulas and coefficients (3) first ionization energies and mass numbers (4) first ionization energies and coefficients The percent composition by mass of nitrogen in NH4OH (gramformula mass 35 grams/mole) is equal to ...
... (1) chemical formulas and mass numbers (2) chemical formulas and coefficients (3) first ionization energies and mass numbers (4) first ionization energies and coefficients The percent composition by mass of nitrogen in NH4OH (gramformula mass 35 grams/mole) is equal to ...
Synthesis Reaction
... I can write chemical reactions by interpreting word equations I can classify reaction types (synthesis, decomposition, single replacement, double replacement, combustion) I can predict the products of chemical reactions in writing complete chemical equations (synthesis, decomposition, single replace ...
... I can write chemical reactions by interpreting word equations I can classify reaction types (synthesis, decomposition, single replacement, double replacement, combustion) I can predict the products of chemical reactions in writing complete chemical equations (synthesis, decomposition, single replace ...
Document
... I can write chemical reactions by interpreting word equations I can classify reaction types (synthesis, decomposition, single replacement, double replacement, combustion) I can predict the products of chemical reactions in writing complete chemical equations (synthesis, decomposition, single replace ...
... I can write chemical reactions by interpreting word equations I can classify reaction types (synthesis, decomposition, single replacement, double replacement, combustion) I can predict the products of chemical reactions in writing complete chemical equations (synthesis, decomposition, single replace ...
AL COS #
... The molar mass of CO2 is 44 g/mol. How many moles are present in 2.5 mol 110 g? The molar mass of H2O is 18.015 g/mol. How many moles of water 0.20 mol are present in 3.6 g? The molar mass of NH3 is 17.0 g/mol. How many grams of NH3 are 59.5 g present in 3.50 moles? What volume of oxygen is needed t ...
... The molar mass of CO2 is 44 g/mol. How many moles are present in 2.5 mol 110 g? The molar mass of H2O is 18.015 g/mol. How many moles of water 0.20 mol are present in 3.6 g? The molar mass of NH3 is 17.0 g/mol. How many grams of NH3 are 59.5 g present in 3.50 moles? What volume of oxygen is needed t ...
M.Sc. 2015
... (i) When nicotine is treated with methyl iodide , it gives dimethiodide. This shows that the two nitrogen atoms in nicotine are tertiary. (ii) When nicotine is oxidized with nitric acid, it gives nicotinic acid, this shows that nicotine contains a ...
... (i) When nicotine is treated with methyl iodide , it gives dimethiodide. This shows that the two nitrogen atoms in nicotine are tertiary. (ii) When nicotine is oxidized with nitric acid, it gives nicotinic acid, this shows that nicotine contains a ...
Chem 430 - Fall 1994
... Chem 430 - Fall 2001 - Test 1 - Page 5 ( 2) 10. What is the SSYS for one cycle of a Carnot Engine? ...
... Chem 430 - Fall 2001 - Test 1 - Page 5 ( 2) 10. What is the SSYS for one cycle of a Carnot Engine? ...
AP Chemistry Review Assignment Brown and LeMay: Chemistry the
... The last part of this section, including how to determine the formula of a hydrate, and how to use combustion analyses to determine empirical formulas will be addressed early in the semester, probably Thurs., Aug. 20. 43. Give the empirical formula of each of the following compounds if a sample cont ...
... The last part of this section, including how to determine the formula of a hydrate, and how to use combustion analyses to determine empirical formulas will be addressed early in the semester, probably Thurs., Aug. 20. 43. Give the empirical formula of each of the following compounds if a sample cont ...
Final Exam Review
... Which statement best describes the effect of the temperature changes on the kinetic energy of the particles? a. Kinetic energy of metal atoms decreases in the flame. b. Kinetic energy of water molecules increases when the heated metal is immersed. c. Kinetic energy of water molecules decreases when ...
... Which statement best describes the effect of the temperature changes on the kinetic energy of the particles? a. Kinetic energy of metal atoms decreases in the flame. b. Kinetic energy of water molecules increases when the heated metal is immersed. c. Kinetic energy of water molecules decreases when ...
Unit 3: Bonding and Nomenclature Content Outline: Calculating
... A. This refers to the sum of the average atomic masses for all the atoms present within a chemical formula for any given ionic compounds formula ( formula unit), or ion. B. Step 1: Use the Periodic Table and the chemical formula to find the average atomic masses for each element present. Step 2: Cal ...
... A. This refers to the sum of the average atomic masses for all the atoms present within a chemical formula for any given ionic compounds formula ( formula unit), or ion. B. Step 1: Use the Periodic Table and the chemical formula to find the average atomic masses for each element present. Step 2: Cal ...
unit 6 - writing and balancing chemical equations
... on heating lost mass and returned to pure metals. Many imaginative explanations of these mass changes were proposed. Antoine Lavoisier (1743-1794), a French nobleman later guillotined in the revolution, was an amateur chemist with a remarkably analytical mind. He considered the properties of metals ...
... on heating lost mass and returned to pure metals. Many imaginative explanations of these mass changes were proposed. Antoine Lavoisier (1743-1794), a French nobleman later guillotined in the revolution, was an amateur chemist with a remarkably analytical mind. He considered the properties of metals ...
Lecture 3
... (2) Molecular formulas from Avogadro’s hypothesis (3) Compute % elements in compounds (1-8) (4) Distinguish between empirical and molecular formulae (1-8) (5) Compute empirical formulas (1-8) Chapter 2 (substances in action: chemical reaction) (6) Balance chemical equations (2-1) (7) Mass (mole) rel ...
... (2) Molecular formulas from Avogadro’s hypothesis (3) Compute % elements in compounds (1-8) (4) Distinguish between empirical and molecular formulae (1-8) (5) Compute empirical formulas (1-8) Chapter 2 (substances in action: chemical reaction) (6) Balance chemical equations (2-1) (7) Mass (mole) rel ...
Chemical Reactions
... the reactants to the left of the arrow separated by plus signs. Write the names of the products to the right of the arrow, also separated by plus ...
... the reactants to the left of the arrow separated by plus signs. Write the names of the products to the right of the arrow, also separated by plus ...
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.