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1 Torr = 0.00133322 bar
1 Torr = 133.322 Pa
1 Torr = 0.00131578584 ATM
1 Torr = 1 mmHg
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1075 torr - 720 torr = 355 torr
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To convert from torr to atm, you divide the torr value by 760. So, 742 torr is equal to 0.976 atm.
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To convert psi to Torr, you can use the conversion factor: 1 psi is approximately equal to 51.715 Torr. Therefore, to convert 102.872 psi to Torr, you would multiply by this conversion factor to get approximately 5332.73 Torr.
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1 torr = 0.13 kilopascals. So, multiply torr by 0.13 to get kilopascals.
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The pressure of 600 torr is equivalent to 0.789 atmospheres.
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456 Torr is equivalent to 0.601 standard atmospheres. This conversion is done by dividing the pressure in Torr by 760 (the number of Torr in 1 standard atmosphere).
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There are 760 torr in 1 inch of mercury. Therefore, 28.5 inches of mercury is equal to 28.5 x 760 = 21660 torr.
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1 torr is equal to 1.33322 kPa. Therefore, 1250 torr is equal to 1666.53 kPa.
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24.34 inches of Mercury is equivalent to 823.86 torr.
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To convert from torr to psi, divide by 51.715. Therefore, 752 torr is approximately 14.55 psi when rounded to two decimal places.
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The unit torr is a measure of pressure, not of atoms. So, there are no atoms in 774 torr.
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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.
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8.95*100 torr, if you must have it in scientific notation.
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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
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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.
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Gragson says 3900 torr.
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742 torr is 0.97632atm. This is gotten by multiplying by 0.00131578947, what one torr is in ATM. i.e 742 x 0.00131578947.
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At 10,000 feet above sea level, the atmospheric pressure is approximately 528 torr. This is lower than the standard atmospheric pressure at sea level, which is 760 torr.
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Using Boyle's law (P1V1 = P2V2), the initial pressure is 820 torr, the initial volume is 110.0 mL, and the final volume is 83.0 mL. Solving for P2, we get P2 = (P1V1) / V2 = (820 torr * 110.0 mL) / 83.0 mL = 1088.55 torr. Therefore, the pressure of the trapped nitrogen in the syringe is 1088.55 torr.
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A torr is a unit of pressure; a micron is a unit of length. You can't convert that.
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Equals 101,325 pascals, 101.325 kpascals, 760 mm of Mercury, and/or 1 atmosphere
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Using Boyle's Law (P1V1 = P2V2), we can find the final pressure with the initial pressure (P1 = 790 torr), initial volume (V1 = 125.0 mL), and final volume (V2 = 75.0 mL). Plugging in the values: (790 torr)(125.0 mL) = P2(75.0 mL). Solving for P2 gives a pressure of 1327 torr for the trapped nitrogen.
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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!
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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.
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The vapor pressure of ethanol (C2H5OH) at 20°C is approximately 43.9 torr.
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No, Torr is a unit of pressure, not energy. It is used to measure gas pressure in many industries, such as chemistry and physics.
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The mole fraction of F2 can be calculated using the equation: Mole fraction of F2 = Partial pressure of F2 / Total pressure of the mixture Mole fraction of F2 = 300 torr / 760 torr = 0.3947
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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.
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To find the volume of dry hydrogen at STP, we need to correct for the presence of water vapor. First, calculate the pressure of dry hydrogen by subtracting the vapor pressure of water from the total pressure: 745.5 torr - 14.5 torr = 731 torr. Then, apply the ideal gas law to solve for the volume of dry hydrogen at STP: V = (200 ml * 731 torr * 273 K) / (290 K * 760 torr) ≈ 181 ml.
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