0
1 atmosphere pressure = 760 torr
655 torr / ( 760 torr / ATM) = 0.86184 ATM
If you're not sure whether to multiply or divide when doing conversions, do this:
655 torr . 1 ATM
------------ * ---------
1. . 760 torr
The formatting did not display exactly as I wanted it to appear
This is read like a fraction. Since 1 ATM = 760 torr, the numerator and denominator are equal, so it's like just multiplying by 1 and won't change the value.
The torr units in numerator/denominator cancel out, and the only unit remaining is atmospheres.
What else can I help you with?
How do you convert kelvin to torr?
What a stupid question. You can't convert things that are units of completely different categories! Kelvin measures temperature while torr measures pressure. They are not related in any way that you can convert them!
What volume is occupied by 1.00 kg of helium at 5.00 degrees celsius at a pressure of 735 torr?
Well, we might as well convert all of this mess. ( we could work in Torr, but why when we are mass converting )1.00 kg He (1000 grams/1 kg) = 1000 grams He (1 mole He/4.003 grams) = 250 moles He5.00o Celsius = 278.15 Kelvin735 Torr = (1 atm/760 Torr = 0.967 atmospheres=========================================Now,PV = nRT(0.967 atm)(Volume) = (250 moles He)(0.08206 L*atm/mol*K)(278.15 K)0.967V = 5706.247Volume = 5.90 X 103 Liters-----------------------------------
Pressure units ATA full form?
A unit of absolute pressure in the metric.ATA(s): Abbreviation for "Atmospheres Absolute", defines as the total pressure exerted on an object, by a gas or mixture of gases, at a specific depth or elevation, including normal atmospheric pressure.
If the height of the mercury column in the leveling bulb is 30 mm greater than that in the gas buret and atmospheric pressure is 670 mm what is the pressure on the gas trapped in the buret?
If the height of the mercury column in the leveling bulb is 30mm greater than that in the gas buret and atmospheric pressure is 670mm, what is the pressure on the gas trapped in the buret?
A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37 degrees Celsius How many moles of nitrogen are in the container?
To calculate the number of moles of nitrogen gas in the container, you can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. Convert the pressure to atm, the volume to L, and the temperature to Kelvin. Then plug in the values and solve for n.
What is the pressure in atmosphere of gas that has a pressureof 600 torr?
600 Torr (1 atm/760 Torr) = 0.789 atmospheres ================
The ideal gas law measures pressure in?
The ideal gas law measures pressure in pascals (Pa) or atmospheres (atm).
Is Torr a common unit of energy?
No, Torr is a unit of pressure, not energy. It is used to measure gas pressure in many industries, such as chemistry and physics.
A closed end manometer has a U tube with a sample of hydrogen gas in the bulb The difference in the height of the columns of mercury is 18.0 cm What is the pressure of the hydrogen gas in torr?
To find the pressure of the hydrogen gas in torr, you can use the difference in height of the mercury columns and the density of mercury. First, calculate the pressure difference due to the 18.0 cm height difference in the mercury columns. Then, convert this pressure into torr using the conversion factor 1 atm = 760 torr.
What are the most common units of pressure volume and temperature?
pressure -- Torr which is equivalent to mmHg, Pascals or kPa, atmospheres, psi, inches Hg Volume -- usually liters Temperature -- Kelvin or Celsius which must be converted to Kelvin to be used in any gas law equations
What law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of its individual gases?
The pressure of each gas in a mixture is called the partial pressure of that gas.
What is the density of oxygen gas at 77 degrees C and 700 Torr?
The density of oxygen gas at 77°C and 700 Torr pressure is approximately 1.429 g/L.
What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2 degrees C when it occupies a volume of 5.00 L?
The pressure exerted by the carbon dioxide gas is 22.8 torr. This can be calculated using the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Given the mass of the gas, the number of moles can be calculated and used to determine the pressure.
A 100 ml sample of nitrogen at 810 torr was compressed to a volume of 72 mL in a syringe What was the pressure of trapped nitrogen in torr?
To find the final pressure of the nitrogen, we can use Boyle's Law which states that the pressure and volume of a gas are inversely proportional when temperature is constant. Therefore, 100 mL * 810 torr = 72 mL * final pressure. Solving for final pressure, we get: final pressure = (100 mL * 810 torr) / 72 mL = 1125 torr. So, the pressure of the trapped nitrogen in the syringe is 1125 torr.
What will be the final volume of a 500 ml sample of helium if its pressure is changed from 740 Torr to 780 Torr and its temperature is kept constant?
According to Boyle's Law, the volume of a gas is inversely proportional to its pressure when temperature is constant. So, if the pressure increases from 740 Torr to 780 Torr, the volume will decrease accordingly. Using the formula P1V1 = P2V2, where P1 = 740 Torr, V1 = 500 ml, and P2 = 780 Torr, you can solve for V2 to find the final volume.
How do you convert kelvin to torr?
What a stupid question. You can't convert things that are units of completely different categories! Kelvin measures temperature while torr measures pressure. They are not related in any way that you can convert them!
What does 500 mm Hg equals?
500 mmHg or 500 torr is a gas pressure approximately 66% of the standard sea level air pressure of 760 torr ... it is the air pressure one would find at an altitude of approximately 3km or 10000 feet ... at sea level, 500 torr would be considered a partial vacuum of 0.66 atm.
