How Many Kpa Is 1 Atm – Journal 1) Convert the following pressures to atmospheric pressure: A. 151.98 kPa B. 456 torr Conversions 1 atm=101.3 kPa= 760 mm Hg= 760.
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How Many Kpa Is 1 Atm
1 Journal 1) Convert the following pressures to pressures in standard atmospheres: A kPa B torr Conversions 1 atm=101.3 kPa= 760 mm Hg= 760 torr Standard temp. & pressure = 1 atm & 0°C (STP) 2) Draw a phase diagram kPa x 1 atm = 1.5 atm 101.3kPa 456 torr x 1 atm = 0.6 atm 760 torr
Examination Of The Kσ Overburden Correction Factor On Liquefaction Resistance
Gases are liquids – gases flow Gases have a low density 1/1000 the density of equivalent liquid or solid gases Gases are compressible.
1. regarding movement. 2. due to movement. 3. characterized by movement: Running and dancing are movement activities. Origin: 1850–55; < Gk kīnētikós moves, cf. to kīnē- (idiom s. of kīneîn to move) + -tikos Source: Websters Dictionary
Gas particles are always in motion. The number of individual gas particles is zero. The collision of gas particles with the walls of the container causes pressure exerted by the gas. The particles have no force on each other. Average kinetic energy is directly proportional to temperature (it moves faster when it’s hotter)
At the same temperature, all gases have the same average kinetic energy. At the same temperature, smaller molecules move faster than larger molecules m = mass v = velocity
How Many Atmospheric Pressures Is Equal To The Pressure Of 2 Kpa ?
Diffusion is the gradual mixing of molecules of different gases. (Smaller molecules mix faster, higher temperature speeds up the process) Effusion is the movement of molecules through a small hole into an empty container. (smaller molecules move faster)
Graham’s law calculates the efflux and diffusion rates of gas molecules. The speed of efflux is inversely proportional to its molecular weight – the lighter the faster it moves! Thomas Graham, Professor in Glasgow and London.
Example: A balloon filled with He or N2 will melt faster if P&T is constant? He molar mass = 4g N2 molar mass = 28g. It releases faster than N2 at the same T because it is lighter. she
11 Graham’s Law Compare the rate of outflow of helium (gas 1) and nitrogen (gas 2)… Velocity He = g N2 = g = 2.7 Velocity N g He g Helium gas escapes almost three times faster than nitrogen gas.
Pressure Units And Pressure Unit Conversion
Can the pressure increase Can the temperature increase? The volume may increase. Increase the pressure? It could decrease
15 Boyle’s Law Boyle’s Law states that the volume of a gas is inversely related to its pressure if the temperature remains constant. What does that mean? As the volume increases, the pressure decreases! (or vice versa!) P1V1 = P2V2
A sample of oxygen occupies a volume of 250.0mL at torr pressure. What volume will it occupy at torr pressure? Find what you know: V1=250.0 mL P1=740.0 torr P2= torr V2=? Solve for what you don’t know P1V1= V2 P2 (740 torr) (250 ml) = V2 (800.0 torr) V2 = 231 ml
Volume of gas changes directly according to Kelvin temperature (if the pressure is constant) V1 = V2 T1 T2 Temperature must be converted to Kelvin K= oC + 273
Solved: Convert Pressure Measurements From One Unit To Another. Given That: 1 Atm = 760 Mmhg = 14.7 Psi = 101.325 Kpa 320 Mmhg Into Atm 30.0 Atm Into Kpa
A sample of nitrogen occupies a volume of 250.0 ml at 25 oC. What volume will it occupy at 95 oC? 1) Find what you know: V1=250.0 mL T1= 25 oC (298 K) T2= 95 oC (368 K) V2=? 2) Convert Temp to Kelvin: K= 25oC + 273= 298 K & K= 95oC + 273= 368 K 3) Solve: V1 = V mL = V V2 =309 mL T1 T K K
19 Gay-Lussac’s Law Temperature and pressure are proportional if mass and volume remain constant. When one grows, the other grows and vice versa. Why? Think collisions – always remember the number. P1 = P2 T1 T2 Temperature must be in Kelvin. Example: Tires do not stretch with increased energy. Aerosols do not expand with increased energy.
Atmospheric pressure is 6.58 kPa at 540 K. What will the pressure be at 210 K if the volume remains constant? Identify what you know: P1 = 6.58 kPa; T1 = 540 K P2 = ? T2 = 210 K Solve for what you don’t know P1 = P kPa = P2 T1 T K K P2= (6.58 kPa) (210K) = KPa 540 K
21 The Combined Gas Law If you write Boyle’s, Charles’ and Gay-Lussac’s gas laws as a single formula, all three variables can change; only the mass remains constant. P1V1 = P2V2 T T2 Why are we interested? It allows us to predict what will happen to gas when conditions change.
The Pressure Units In The Converter
P1V1 = P2V2 T1 T2 AKA: The Compound Gas Law allows you to predict what will happen to a gas if some conditions change!
23 Let’s practice! A gas with a volume of 4.0L at 90.0kPa expands until the pressure drops to 20.0kPa. What is the new volume if the temperature remains constant? Find What You Know V1=4.0L P1=90.0kPa P2=20.0kPa T1=T2 Solve What You Don’t Know V2 = P1V1 x T2 T P2 V2 = 18.0L
24 Now you try! A gas with a volume of 3.00x102mL at 150.0˚C is heated until its volume is 6.00x102mL. What is the new temperature of the gas if the pressure remains constant at 1.0 atm during heating. T2= 300.0˚C
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Solved] Convert 618 Mm Hg To Kpa. (1 Atm = 760 Mm Hg = 101.3 Kpa). Show All…
1. Millimeter of mercury (mmHg): 1 mmHg is also called torr 2. atmosphere (atms): 1 atm = 760 mmHg 3. kilopascal (kPa): 1 atm = kPa
F. Conversion exercises: convert 4.60 atm to kPa convert kPa to atm convert 580 mmHg to atm mmHg to kPa
F. Conversion exercises: convert 4.60 atm to kPa 4.60 atm 1 × kPa 1 atm =466 kPa convert kPa to atm 793.8 kPa 1 × 1 atm kPa =7.834 atm.
Converting Between Units Of Pressure And
F. Conversion exercises: convert 580 mmHg to atm 580 mmHg 1 × 1 atm 760 mmHg =0.76 atm convert mmHg to kPa mmHg 1 × kPa 760 mmHg = kPa
G. Absolute zero: – °C or 0 K K = ˚C ˚C = K – H. Conversion exercise 1. convert 24.8 ˚C to K 2. convert 376 K to ˚C
G. Absolute zero: – °C or 0 K K = ˚C ˚C = K – H. Conversion exercise 1. convert 24.8 ˚C to K K = = K 2. convert 376 K to ˚C ˚C = 376 – = 103 ˚C
10 𝐓𝐡𝐚 𝐆𝐰𝐬𝐋𝐬𝐋𝐬𝐬 A. Dalton’s law of partial pressure: states that the total pressure of a gas mixture is the sum of the partial pressures of the gases
Chapter 6 Gases 6.2 Gas Pressure.
11 𝐓𝐡𝐞 𝐆𝐰𝐬𝐬 𝐋𝐬𝐬 1. Partial pressure: the pressure of each type of gas in a mixture 2. PT = P1 + P2 + P3
The total pressure of a gas mixture of nitrogen, oxygen and argon is mmHg. If the pressure of nitrogen is mmHg and the pressure of oxygen is 312.8, what is the pressure of argon gas?
The total pressure of a gas mixture of nitrogen, oxygen and argon is mmHg. If the pressure of nitrogen is mmHg and the pressure of oxygen is 312.8, what is the pressure of argon gas? 𝐏 ██𝐭𝐦 = 𝐏 𝐍 𝟐 + 𝐏 𝐎 𝟐 + 𝐏 𝐀𝐫 762.4 = PAr 𝐏 𝐀𝐫 = mmHg
𝐏 ██𝐭𝐦 = 𝐏 𝐠𝐬𝐬 + 𝐏 𝐇 𝟐 𝐎 B. Partial pressure exercise Gas is collected above water with a sound meter. A barometer indicates air pressure in mmHg. If the gas pressure at the sound meter is mmHg, what is the water vapor pressure?
What Is A Kilopascal (kpa)?
16 𝐏 ⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀
𝐏 ██𝐭𝐦 = 𝐏 𝐠𝐬𝐬 + 𝐏 𝐇 𝟐 𝐎 B. Partial pressure exercise Gas is collected above water with a sound meter. A barometer indicates air pressure in mmHg. If the gas pressure at the sound meter is mmHg, what is the water vapor pressure? 𝐏 ██𝐭𝐦 = 𝐏 𝐠𝐬 + 𝐏 𝐇 𝟐 𝐎 748.2 = P H 2 O 𝐏 𝐇 𝟐 𝐎 = 26.5 mmHg
17 𝐓𝐡KEY🐰 𝐆𝐰𝐬𝐋𝐬 C. Boyle’s law: states that the volume of a fixed mass of gas is inversely proportional to the pressure at constant temperature P1V1 = P2V2
Charles’ law: states that the volume of a solid mass of gas at constant pressure changes directly with the Kelvin temperature V 1 T 1 = V 2 T 2
Unit 12: Gas Laws Section 1: Gas Pressure.
19 𝐓𝐡𝐞 𝐆𝐰𝐬𝐬 𝐋𝐬𝐬 Law of E. Gay-Lussac: pressure from
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