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What happens to the value R if your pressure is in mm- Hg and your volume in mL?
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A 30 L sample of gas exerts 200 mm Hg pressure at 10 Celsius What volume does the gas have at 300 mm Hg and 25 Celsius?
17 l
A sample of helium has a volume of 325mL and a pressure of 655mm Hg what will be the pressure if the helium you compressed to 125mL?
P1V1=P2V2 VI=325ml P1=655mm Hg V2=125ml P2=? =655 x 325= P2 x 125 =(655 x 325)/ 125 =212875/125 =1703mm Hg. :)
What is the partial pressure of hydrogen gas in a mixture of hydrogen and helium if the total pressure is 600 mm Hg and the partial pressure of helium is 439 Torr?
To convert Torr to mm Hg, divide by 1.33. So, the partial pressure of helium in mm Hg is 439 Torr / 1.33 = 330 mm Hg. To find the partial pressure of hydrogen, subtract the partial pressure of helium from the total pressure: 600 mm Hg - 330 mm Hg = 270 mm Hg. Hence, the partial pressure of hydrogen gas is 270 mm Hg.
When a gas occupies a volume of 0.2 L at 176 mm Hg. What volume will the gas occupy at 760 mm Hg?
The volume is 0,046 L.
What is vascular pressure that declines form 35 mm Hg to 18 mm Hg?
Peripheral pressure.
A container filled with gas has a volume of 185 ml and a pressure of 310 mm Hg The desired new volume is 74.0 ml What is the required new pressure?
the answer is 72.1 Hg
Normal blood pressure value is 140 90mm Hg true or false?
False, normal blood pressure is a value of 120/80 mm Hg or lower.
A gas occupies 30 L at 760 mm Hg what is its volume at 350 mm Hg?
The phrase "760 mm Hg" is physicists' shorthand for "an atmospheric pressure equal to that needed to support a column of mercury [chemical symbol Hg] of length 760 mm". This is approximately average atmospheric pressure at sea level. As the pressure decreases from "760 mm Hg" to "350 mm Hg", the volume of the gas will increase (assuming a constant temperature). The new volume can be determined using Boyle's Law: New Volume = 30 x 760 / 350 = 65.143 Litres
A mixture of gases with a pressure of 800.0 mm Hg contains 60 percent nitrogen and 40 percent oxygen by volume What is the partial pressure of oxygen in this mixture?
320.0 mm Hg
The volume of a gas collected when the temperature is 11.0 C and the pressure is 710 millimeter Hg measures 14.8 mL What is the calculated volume of the gas at 20.0 C and 740 millimeter Hg?
13.7, using P1V1T2=P2V2T1.
A 30 L sample of gas exerts 200 mm Hg pressure at 10 Celsius What volume does the gas have at 300 mm Hg and 25 Celsius?
17 l
If 18.0 g O2 has a temperature of 350 K and a pressure of 550 mm Hg what is its volume?
22.3 L
What is the volume of 0.700 mol of neon gas at a pressure of 609.5 mm Hg and 117C?
First two conversions: 609.5mm Hg = 0.8atm, and 117 deg. Celsius = 390 kelvins. Now, use the ideal gas law equation, PV=nRT with 0.082 as your value for R, the ideal gas constant: 0.8V=(0.7)(0.082)(390) and you get about 28L for the volume.
When a sample of nitrogen has a volume of 3.97 L at 1479 mm Hg and - 42 C what volume will it occupy at standard temperature and pressure?
I'm not going to do all your work. The formula is Pressure1 X Volume 1 X Temperaure 1(in Kelvins)= Pressure 2 X Volume 2 X temperaure 2 So 3.97L X 1479mm Hg X 231.15K = y volume X 760mm Hg (1 atmosphere) X 293.15 (20 degrees C) I'll let you figure out the maths.
Air contains 21 percent oxygen by volume and the rest nitrogen If the barometer pressure is 740 mm of Hg the partial pressure of oxygen is close to?
If we consider oxygen content in atmosphere to be roughly around 21% and the rest nitrogen then answer to the above question will be: 155.4 mm of Hg
A sample of helium has a volume of 325mL and a pressure of 655mm Hg what will be the pressure if the helium you compressed to 125mL?
P1V1=P2V2 VI=325ml P1=655mm Hg V2=125ml P2=? =655 x 325= P2 x 125 =(655 x 325)/ 125 =212875/125 =1703mm Hg. :)
If 7.56 L of a gas are collected at a pressure of 745 mm Hg then what volume will this gas occupy at standard atmospheric pressure if the temperature remains the same?
7.41 L
