volume of the football starts to decrease. Boyle’s Law describes how the pressure of the gas tends to decrease as the volume of a gas increases. As the pressure decreases‚ the volume of the gas increases. The bubbles exhaled by the fish grow as it approaches the surface of the ocean. When the fish is exhaling out the air‚ the bubbles tend to become bigger and bigger. As the bubbles start to approach the sea surface‚ less pressure will be put on the bubbles‚ so the volume of the bubbles start to increase
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financial pressures‚ vices‚ or because of work-related pressures. As well‚ perpetrators of fraud can be motivated by a perceived opportunity to commit fraud and the ability to rationalize that what they are doing is not wrong. Their motivations are usually combined into the fraud triangle of perceived pressure‚ perceived opportunity‚ and rationalization. 3. The fraud triangle includes three elements that almost always must be present in order for someone to commit fraud: a perceived pressure‚ a perceived
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intentional at the top becaue again the premiss that palnned change should flow from the top. 2. Rationale for choosing model. A review of internal and external pressures. Before I discuss the rationale rational behind choosing the Burke-Litwin Model‚ I would like to review the internal and external pressures that have affected these companies. As we know when a inside the company and outside the company for change. This situation was no different. One thing that I would like
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measure the pressure inside the container. Procedure: 1. Move the lid of the container up or down. Record the resulting volume and pressure inside the container. 2. Continue this process until data is obtained for at least six different volume and pressure combinations. Be sure to use a range of volume measurements to help you better compare the relationship of volume and pressure. Please record the data below in the data chart. Data and Observations: Part 1: Boyle’s Law Lab Pressure in (Kpa)
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Variable- Independent- Amount of Catalase (Filter Paper) Dependent- Amount of Oxygen (kPa) Constant- Temperature in Fahrenheit‚ 2 Pipette of Hydrogen Peroxide‚ 0.8 Cm Filter Paper Punches Materials: * 6 Test Tubes * Vernier Gas Pressure * Sensor * Catalase * Filter Paper Punches * Beaker * Control Group * Test Subject * Safety Goggles * Dropper Pipette * Go Link Procedure- 1. Gather Your Materials Figure 2 2. Put on your
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change in temperature and pressure of ethanol using a Vernier temperature probe. By using the ideal gas equation‚ and plugging the slope value from the graph into the Clausius-Claypernon equation‚ enthalpy of vaporization was determined to be 10kJ/mol. The percent error was determined to be 76.0%. Introduction: The purpose of this lab is to investigate vapor pressures and the partial pressure of gas produced from liquids at different temperatures. These pressures vary at different temperatures
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ways to find the molar mass of a substance. One way‚ if the substance is a gas‚ is to use the Ideal Gas Equation to find molar mass. The standard equation reads PV=nRT where “n” is the number of moles present‚ “P” is the pressure (which is obtained by reading the barometric pressure of the room with the class barometer)‚ “V” is the volume of the gas‚ “R” is the universal constant‚ and “T” is the temperature of the gas. The experiment’s objective is to calculate the experimental value of molar mass
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collecting lab data‚ determine the hydrogen gas’s molar volume at STP through calculation. Materials: -LabQuest data collector - 3.0 M of HCl solution - Ribbon of Mg metal - Gas pressure sensor - Temperature probe - 600 mL beaker - 125 mL Erlenmeyer flask - 20 mL gas syringe - Rubber stopper with two-way valve
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spherical and elastic particles. Although an ideal gas is a theoretical model and so cannot exist in practice‚ most gases behave fairly similarly to an ideal gas. Gases behave more like an ideal gas when they are at a higher temperature and lower pressure‚ as the potential energy of the intermolecular forces becomes negligible compared to the kinetic energy of the gas. Butane gas does follow the ideal gas law fairly well‚ as it is non-polar and hence has
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R = 1. What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 20.(C? 2. Oxygen gas is collected at a pressure of 123 kPa in a container which has a volume of 10.0 L. What temperature must be maintained on 0.500 moles of this gas in order to maintain this pressure? Express the temperature in degrees Celsius. 3. How many moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and
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