2-7 Gas Laws
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The document discusses the gas laws and how temperature, pressure, and volume of a gas are related. It defines key terms like pressure, temperature, and volume. It explains Boyle's law, Charles' law, and the combined gas law. Boyle's law states that if temperature and amount of gas are kept constant, pressure and volume are inversely related. Charles' law states that if pressure and amount of gas are kept constant, volume and temperature are directly related. The combined gas law incorporates all factors - if temperature increases while amount and volume remain constant, pressure will also increase.
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4. Practice problems provide additional examples for readers to work through the calculations.
23 gases
- Gases have negligible volume and molecules are far apart with mostly empty space between them. Gas molecules move randomly in straight lines and collide elastically.
- The kinetic molecular theory describes gas properties including high translational energy of gas molecules that move randomly in all directions.
- Pressure, volume, temperature of gases are directly or inversely related as described by Boyle's, Charles', and Gay-Lussac's laws and the combined gas law.
Kinetic molecular theory
The document summarizes the kinetic molecular theory and gas laws. It explains that kinetic molecular theory models gases as particles in constant, random motion that exert pressure during collisions. It describes the gas laws of Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's hypothesis, and Dalton's law of partial pressures which relate the variables of pressure, volume, temperature, and moles of gas. Examples are provided to illustrate applications of the gas laws.
Intro to Gases and Gas Laws.ppt
The document discusses the kinetic molecular theory of gases and the gas laws. It explains that according to the kinetic molecular theory, gas particles are in constant, random, straight-line motion and have no intermolecular forces. The gas laws - Boyle's law, Charles' law, and Gay-Lussac's law - describe the relationships between pressure, volume, temperature for an ideal gas. Boyle's law states that pressure and volume are inversely proportional at constant temperature. Charles' law states that volume and temperature are directly proportional at constant pressure. Gay-Lussac's law states that pressure and temperature are directly proportional at constant volume. Examples are given to demonstrate calculating unknown values using the gas laws and combined gas law.
Intro to Gases and Gas Laws.ppt
The document discusses the kinetic molecular theory of gases and the gas laws. It explains that according to the kinetic molecular theory, gas particles are in constant, random, straight-line motion and have no intermolecular forces. The gas laws - Boyle's law, Charles' law, and Gay-Lussac's law - describe the relationships between pressure, volume, temperature for an ideal gas. Boyle's law states that pressure and volume are inversely proportional at constant temperature. Charles' law states that volume and temperature are directly proportional at constant pressure. Gay-Lussac's law states that pressure and temperature are directly proportional at constant volume. Examples are given to demonstrate using the gas laws to calculate unknown properties.
9_Gas_Laws.pdf
The document discusses the four main gas laws:
1) Boyle's law states that at a constant temperature, the pressure and volume of a gas are inversely proportional.
2) Charles' law explains that at constant pressure, the volume of a gas is directly proportional to its temperature.
3) Avogadro's law says that equal volumes of gases under the same conditions contain equal numbers of molecules.
4) The ideal gas law combines these to give the equation of state that relates pressure, volume, temperature and moles of gas.
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2-2 Chemical & Physical Changes
This document discusses clues that indicate a chemical change has occurred, including a change in color, production of a gas, formation of a solid precipitate, and release of energy in the form of heat or light. It also mentions applying the kinetic theory of matter and recognizing that multiple physical changes may occur.
2-1 Chemical & Physical Properties
The document discusses the properties and states of matter. It defines matter as anything that has mass and takes up space. It distinguishes between physical properties, which can be observed without chemical change, and chemical properties, which involve chemical reactions. Matter can exist in three main states - solid, liquid, and gas - which differ in how tightly or loosely the particles are packed and how they move. Phase changes between these states involve adding or removing energy without changing temperature.
2-3 Classifying Matter
This document discusses classifying different types of matter. It defines matter as anything that has mass and takes up space. Pure substances are made of only one type of matter and have consistent properties, while mixtures contain two or more substances mixed together. Pure substances are classified as either elements, which contain only one type of atom, or compounds, which are made of two or more simpler substances combined chemically. Mixtures can be either heterogeneous, with distinct parts visible throughout, or homogeneous, appearing uniform throughout.
1-2 Introduction to Chemistry
This document provides an introduction to chemistry concepts and the scientific method. It defines chemistry as the study of matter, and matter as anything that takes up space and has mass. It distinguishes between mass, which is a measurement of how much matter is present, and weight, which is a measurement of the gravitational force acting on mass. The five steps of the scientific method are outlined as observation, hypothesis, experiment, data analysis, and conclusion.
8-1 Electric Charge
Kinetic energy is the energy of moving objects. When a ball is thrown up, gravity converts the kinetic energy into potential energy. Gravity is directed downward with an acceleration of 9.8 m/s2. The two types of electric charge are positive and negative. Charged objects become charged through friction, conduction, or induction which leads to electric forces and fields between them.
8-2 Electric Current
Electric current is the steady flow of electrons through a conductor. It is measured in amps. Direct current flows in one direction, while alternating current regularly reverses direction. Voltage is the "push" that causes electrons to flow and is measured in volts. Resistance slows the flow of electrons and is measured in ohms. Ohm's Law mathematically shows the relationship between current (I), voltage (V), and resistance (R) as V=IR. Sample problems demonstrate calculating voltage, current, and resistance using Ohm's Law.
7-5 Newtons Third Law
1) A skydiver feels weightless while falling and accelerating due to gravity, heavier when the parachute deploys due to increased air resistance, and a normal weight at terminal velocity when acceleration equals zero.
2) Newton's Third Law states that for every action force there is an equal and opposite reaction force. Examples include a hand pushing a wall, which results in the wall pushing back on the hand, or a foot kicking a ball which causes the ball to push back on the foot.
3) Action and reaction forces do not cancel each other out, but rather act on different objects. They can cause motion, such as a swimmer pushing back on water which pushes the swimmer forward, but
7-3 Newtons 2nd Law
Newton's second law relates force, mass, and acceleration. It states that the acceleration of an object is directly proportional to the net force acting on it, and inversely proportional to its mass. Greater force or lower mass results in greater acceleration. The law can be used to calculate acceleration, force, or mass when two of the three values are known. Mass resists changes in motion, so objects with greater mass experience less acceleration from the same force.
Unit 6 Practice Test
The document contains practice problems for creating distance vs. time and velocity vs. time graphs. For d vs. t graphs, there are 7 scenarios to graph such as a car accelerating from rest and a skier decelerating to a stop. For v vs. t graphs, there are also 7 scenarios like a runner falling during a run and a space shuttle taking off. Answers with the corresponding graph for each scenario are provided.
7-2 Newtons 1st Law
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3) Tosh is correct - inertia depends on an object's mass, not its speed. The greater the mass, the greater the inertia.
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Forces are pushes or pulls that cause changes in motion or acceleration. There are four main types of friction: static, sliding, rolling, and fluid friction. Gravity acts everywhere, pulling objects toward the center of masses like the Earth. Gravity affects falling objects, along with air resistance from the atmosphere. Balanced forces cause no changes in motion, while unbalanced forces result in movement.
6-4 Speed & Velocity
Sam walked 10 meters down a hall, then turned right and walked 25 meters to the cafeteria. His total distance traveled was 35 meters but his displacement was only 25 meters since he returned to his starting point. An airplane will have a greater velocity flying in the same direction as the wind, since velocities add when traveling in the same direction but subtract when traveling in opposite directions. Distance-time graphs can be used to determine if an object is moving at a constant or changing speed based on whether the graph is a straight line or curved line.
5-4 Classifying Reactions
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1) Synthesis reactions combine two reactants to form one product.
2) Decomposition reactions involve a compound breaking down into simpler substances.
3) Single replacement reactions occur when one element replaces another in a compound.
4) Double replacement reactions involve two compounds exchanging ions to form two new compounds.
5) Combustion reactions involve rapid reaction with oxygen, often producing heat and light.
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5-3 Balancing Moles
This document defines the mole as the standard unit used by chemists to count particles and explains how moles are used to balance chemical equations. It states that one mole is equal to 6.022 x 1023 particles of a substance and that different substances have different molar masses based on their atomic or molecular masses. It also describes how moles allow chemists to show the conservation of mass in chemical reactions by converting between mass and moles using molar mass.
5-1 Describing Reactions
The document discusses chemical reactions and balancing chemical equations. It explains that chemical reactions involve reactants combining to form products, with compounds changing forms. Mass is conserved in chemical reactions, with the total mass of reactants equaling the total mass of products. It also provides examples of how to count atoms in chemical formulas using subscripts and coefficients.
5-2 Balancing Reactions
This document discusses balancing chemical equations by manipulating coefficients to ensure conservation of mass. It provides examples of balancing a variety of chemical equations including reactions involving polyatomic ions, metals, nonmetals, hydrogen, and oxygen. The key steps are to count the number of atoms on each side of the equation and adjust coefficients until balanced.
4-4 Ionic & Covalent Bonding
Ionic bonds form when electrons are transferred between metals and nonmetals, resulting in oppositely charged ions. Covalent bonds form when nonmetals share electrons in order to achieve a stable electron configuration. Ionic compounds have high melting points and conduct electricity well when melted but not solid, while covalent compounds have low melting points and generally do not conduct electricity or dissolve in water well.
4-1: Ions & Ionic Bonding
1) Atoms form ions when they lose or gain electrons to achieve a stable electron configuration like the noble gases.
2) Metals form positive ions (cations) by losing electrons, while nonmetals form negative ions (anions) by gaining electrons.
3) Ionic bonds form when oppositely charged ions are attracted to each other, such as sodium (Na+) and chlorine (Cl-), resulting in an ionic compound.
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2-7 Gas Laws
- 6. Boyle’s Law Keep amount and Temperature of gas constant: pressure increases, volume decreases pressure decreases, volume increases
- 7. Charles’s Law Keep pressure and amount of gas constant: temperature increases, volume increases. Temperature decreases, volume decreases.
- 8. Combined Gas Law If the amount and volume of a gas remains constant and the temperature increases, the pressure will increase. If T increases then P increases.