Heat capacity - Department of Chemistry and Physics
... Heat of vaporization: heat needed to convert a substance from a liquid to a gas (at its boiling/condensation point) 2256 J/g for water ...
... Heat of vaporization: heat needed to convert a substance from a liquid to a gas (at its boiling/condensation point) 2256 J/g for water ...
AP `99 Multiple Choice
... (NH4)2SO4(s) (E) Sr(NO3)2(s) 66. When solid ammonium chloride, NH4Cl(s), is added to water at 25_C it dissolves and the temperature of the solution decreases. Which of the following is true for the values of _H and _S for the dissolving process? (A) Positive ...
... (NH4)2SO4(s) (E) Sr(NO3)2(s) 66. When solid ammonium chloride, NH4Cl(s), is added to water at 25_C it dissolves and the temperature of the solution decreases. Which of the following is true for the values of _H and _S for the dissolving process? (A) Positive ...
1999 Advanced Placement Chemistry Exam
... (NH4)2SO4(s) (E) Sr(NO3)2(s) 66. When solid ammonium chloride, NH4Cl(s), is added to water at 25_C it dissolves and the temperature of the solution decreases. Which of the following is true for the values of _H and _S for the dissolving process? (A) Positive ...
... (NH4)2SO4(s) (E) Sr(NO3)2(s) 66. When solid ammonium chloride, NH4Cl(s), is added to water at 25_C it dissolves and the temperature of the solution decreases. Which of the following is true for the values of _H and _S for the dissolving process? (A) Positive ...
AP Ch 5 Gases . ppt
... Kinetic Molecular Theory of Gases 1. A gas is composed of molecules that are separated from each other by distances far greater than their own dimensions. The molecules can be considered to be points; that is, they possess mass but have negligible volume. 2. Gas molecules are in constant motion in ...
... Kinetic Molecular Theory of Gases 1. A gas is composed of molecules that are separated from each other by distances far greater than their own dimensions. The molecules can be considered to be points; that is, they possess mass but have negligible volume. 2. Gas molecules are in constant motion in ...
GENERAL CHEMISTRY REVIEW
... Binary Ionic Compounds, where the metal ion has only one oxidation state (Group 1A, alkali metals and group 2A, alkali earth metals) 1. the cation (positive ion) named first using the element name 2. monatomic cations take name from the corresponding element (i.e., cesium) 3. monatomic anions (negit ...
... Binary Ionic Compounds, where the metal ion has only one oxidation state (Group 1A, alkali metals and group 2A, alkali earth metals) 1. the cation (positive ion) named first using the element name 2. monatomic cations take name from the corresponding element (i.e., cesium) 3. monatomic anions (negit ...
Unit 10
... surface of calcium. This insoluble layer prevents the further attack of the acid. All metal sulphates are soluble in water, except calcium sulphate, barium sulphate and lead(II) sulphate. ...
... surface of calcium. This insoluble layer prevents the further attack of the acid. All metal sulphates are soluble in water, except calcium sulphate, barium sulphate and lead(II) sulphate. ...
Chemistry I - Net Start Class
... A mixture of baking soda and vinegar give off a gas. Heated moth balls turn into a liquid. A powder mixed with water makes lemonade. 3. A solid, silver-colored metallic element is combined with a light green, gaseous element, producing a powdery white solid product. What type of substance was the re ...
... A mixture of baking soda and vinegar give off a gas. Heated moth balls turn into a liquid. A powder mixed with water makes lemonade. 3. A solid, silver-colored metallic element is combined with a light green, gaseous element, producing a powdery white solid product. What type of substance was the re ...
MIDDLE COLLEGE HIGH SCHOOL
... 8. Given the potential energy diagram for a (3) more surface area chemical reaction: (4) more zinc atoms 3. In most aqueous reactions as temperature increases, the effectiveness of collisions between reacting particles (1) decreases (3) remains the same (2) increases 4. Based on the nature of the re ...
... 8. Given the potential energy diagram for a (3) more surface area chemical reaction: (4) more zinc atoms 3. In most aqueous reactions as temperature increases, the effectiveness of collisions between reacting particles (1) decreases (3) remains the same (2) increases 4. Based on the nature of the re ...
Chapter 4,5,6
... solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. 4. A sodium hydroxide solution of unknown concentration is used to titrate a solution containing 865 mg of KHP (KHC8H4O4 , molar mass = 204.22 g/mol ). Unfortunately ...
... solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. 4. A sodium hydroxide solution of unknown concentration is used to titrate a solution containing 865 mg of KHP (KHC8H4O4 , molar mass = 204.22 g/mol ). Unfortunately ...
File
... of the equation to equal to the number of H+(aq) ions added. Step 8: Combine the H+(aq) and OH-(aq) ions on the same side of the equation to create H2O(l) and cancel any excess H2O(l) on either side of the equation. Homework: Pg. 668 #1, 2, 3, 4 and Pg. 673 #6, 7, 8 ...
... of the equation to equal to the number of H+(aq) ions added. Step 8: Combine the H+(aq) and OH-(aq) ions on the same side of the equation to create H2O(l) and cancel any excess H2O(l) on either side of the equation. Homework: Pg. 668 #1, 2, 3, 4 and Pg. 673 #6, 7, 8 ...
How to balance chemical equations.
... •When pieces of matter come together or break apart, it is called a reaction. •The law of conservation of matter states that matter can not be created or destroyed. •In any reaction, you must have the same amount of each part before and after the reaction happens. •We show how reactions become balan ...
... •When pieces of matter come together or break apart, it is called a reaction. •The law of conservation of matter states that matter can not be created or destroyed. •In any reaction, you must have the same amount of each part before and after the reaction happens. •We show how reactions become balan ...
Chemistry II Exams and Keys 2014 Season
... 1. What mass of propane, C3H8, would need to be combusted in order to convert 2.00 kg of water that is initially at 20.0°C to steam at 100.0°C? Assume that all of the heat generated goes directly into heating the water. Enthalpy of combustion of gaseous propane is -2202 kJ/mol. Heat of vaporization ...
... 1. What mass of propane, C3H8, would need to be combusted in order to convert 2.00 kg of water that is initially at 20.0°C to steam at 100.0°C? Assume that all of the heat generated goes directly into heating the water. Enthalpy of combustion of gaseous propane is -2202 kJ/mol. Heat of vaporization ...
Year 9 Chemical Sciences Program Term 3 Course 2 2017
... investigating reactions of acids with metals, bases, and carbonates investigating a range of different reactions to classify them as exothermic or endothermic recognising the role of oxygen in combustion reactions and comparing combustion with other oxidation reactions comparing respiration ...
... investigating reactions of acids with metals, bases, and carbonates investigating a range of different reactions to classify them as exothermic or endothermic recognising the role of oxygen in combustion reactions and comparing combustion with other oxidation reactions comparing respiration ...
Study Guide
... 6. An iodine sample contains 2.91 × 1022 atoms of iodine. What is its mass in grams? [Use atomic weight: I, 126.9] 7. When a solid compound is described as a “hydrate”, what does this mean? 8. What is the difference in meaning between “2O” and “O2” when they occur in chemical equations? 9. 6.022 ×10 ...
... 6. An iodine sample contains 2.91 × 1022 atoms of iodine. What is its mass in grams? [Use atomic weight: I, 126.9] 7. When a solid compound is described as a “hydrate”, what does this mean? 8. What is the difference in meaning between “2O” and “O2” when they occur in chemical equations? 9. 6.022 ×10 ...
09/11/03 lecture
... Going from amu to grams... • Atomic mass units are still really small…how do we relate amu to something we can measure easily in the lab (like grams)? • Introduce a new unit: the mole • A mole is equal to the number of carbon atoms in exactly 12 grams of carbon. This number is called Avogadro’s numb ...
... Going from amu to grams... • Atomic mass units are still really small…how do we relate amu to something we can measure easily in the lab (like grams)? • Introduce a new unit: the mole • A mole is equal to the number of carbon atoms in exactly 12 grams of carbon. This number is called Avogadro’s numb ...
chapter 1 - College Test bank - get test bank and solution manual
... liquid gasoline is converted to heat and gases. Another constructive example is the burning of coal to heat water into steam, which is then used to turn a turbine and produce electricity. The combustion of coal results in a flame plus other gases. The above two examples are examples of chemical chan ...
... liquid gasoline is converted to heat and gases. Another constructive example is the burning of coal to heat water into steam, which is then used to turn a turbine and produce electricity. The combustion of coal results in a flame plus other gases. The above two examples are examples of chemical chan ...
Kinetics - Chemistry Geek
... The experimental rate law for the reaction between NO2 and CO to produce NO and CO2 is rate = k[NO2]2. The reaction is believed to occur via two steps: ...
... The experimental rate law for the reaction between NO2 and CO to produce NO and CO2 is rate = k[NO2]2. The reaction is believed to occur via two steps: ...
3.Masses of individual atoms
... The Carbon-12 Scale • Relative masses of atoms of different elements are express in terms of their atomic masses . • The atomic mass of an element indicates how heavy, on average, an atom of an element is when compared to an atom of another element • Unit is the amu (atomic mass unit) • Mass of one ...
... The Carbon-12 Scale • Relative masses of atoms of different elements are express in terms of their atomic masses . • The atomic mass of an element indicates how heavy, on average, an atom of an element is when compared to an atom of another element • Unit is the amu (atomic mass unit) • Mass of one ...
Topic 3
... (6.022 x 1023 FU or molecules) of a substance. This is the term we will use the most in the course and is done the same way as formula wt. except using gram instead of amu. – For all substances, molar mass, in grams per mole, is numerically equal to the formula weight in atomic mass units. – That is ...
... (6.022 x 1023 FU or molecules) of a substance. This is the term we will use the most in the course and is done the same way as formula wt. except using gram instead of amu. – For all substances, molar mass, in grams per mole, is numerically equal to the formula weight in atomic mass units. – That is ...
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.