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If pressure is in mmHg and volume is in mL, the gas constant R will need to be adjusted to the appropriate units so that the equation PV = nRT balances out correctly. The value of R will remain the same (0.08206 L·atm/mol·K) but it will need to be used with the appropriate units for pressure and volume conversions.
What else can I help you with?
Is mm Hg and milileters a unit of air pressure?
Yes, mm Hg (millimeters of mercury) is a unit of air pressure commonly used in barometric pressure measurements. Milliliters (mL), on the other hand, is a unit of volume and is not used to measure air pressure.
What is vascular pressure that declines form 35 mm Hg to 18 mm Hg?
The change in vascular pressure is a decrease of 17 mm Hg (35 mm Hg - 18 mm 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 mm Hg?
The partial pressure of hydrogen gas can be calculated by subtracting the partial pressure of helium from the total pressure. Therefore, the partial pressure of hydrogen gas would be 161 mm Hg (600 mm Hg - 439 mm Hg = 161 mm Hg).
What would be the new pressure if a 400 mL gas sample at 380 mm Hg is expanded to 800 mL with no change of temperature?
According to Boyle's Law, if you double the volume of a gas at constant temperature, the pressure is halved. So, the pressure would decrease to 190 mm Hg when the gas sample is expanded to 800 mL.
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.
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 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?
Using the combined gas law (P1V1 = P2V2), we can solve for the new pressure: P2 = (P1*V1) / V2. Plugging in the values: P2 = (310 mm Hg * 185 ml) / 74.0 ml = 775 mm Hg. The required new pressure is 775 mm Hg.
What is the mean of 760mm of hg?
760 mm Hg is the standard barometric (atmospheric) pressure. It is the pressure giving a pillar of mercury (the elemental abbreviation of mercury is Hg) that is 760 millimeters (mm) high.
Is mm Hg and milileters a unit of air pressure?
Yes, mm Hg (millimeters of mercury) is a unit of air pressure commonly used in barometric pressure measurements. Milliliters (mL), on the other hand, is a unit of volume and is not used to measure air pressure.
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?
The partial pressure of oxygen in the mixture can be calculated using Dalton's Law of partial pressures. First, convert the percentages to decimal form (60% = 0.60, 40% = 0.40). Then, multiply the total pressure of 800.0 mm Hg by the volume percentage of oxygen (0.40) to find the partial pressure of oxygen in the mixture. This gives a partial pressure of oxygen of 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.
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?
The partial pressure of oxygen in air can be calculated as follows: 21% of 740 mm Hg = 0.21 * 740 mm Hg = 155.4 mm Hg. Therefore, the partial pressure of oxygen in this scenario would be close to 155.4 mm Hg.
What is vascular pressure that declines form 35 mm Hg to 18 mm Hg?
The change in vascular pressure is a decrease of 17 mm Hg (35 mm Hg - 18 mm Hg).
40 liters of gas were collected over water when the barometer read 622.0 mm Hg and temp was 20C what volume wuould dry gas occupy at standard conditions?
To find the volume of the dry gas at standard conditions (0°C and 1 atm), we need to correct for the water vapor using the vapor pressure of water at 20°C. The vapor pressure of water at 20°C is 17.5 mm Hg. Therefore, the pressure of the dry gas is 622.0 mm Hg (total pressure) - 17.5 mm Hg (water vapor pressure) = 604.5 mm Hg. Using the ideal gas law, we can calculate the volume of the dry gas at standard conditions.
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 mm Hg?
The partial pressure of hydrogen gas can be calculated by subtracting the partial pressure of helium from the total pressure. Therefore, the partial pressure of hydrogen gas would be 161 mm Hg (600 mm Hg - 439 mm Hg = 161 mm 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?
To find the volume at standard pressure, we can use the combined gas law equation, which states that (P1 x V1) / T1 = (P2 x V2) / T2. Assuming standard pressure is 760 mm Hg, we have: (745 mm Hg x 7.56 L) / T = (760 mm Hg x V2) / T. Solving for V2, we get V2 = (745 x 7.56 x T) / 760. Since the temperature is constant, the volume at standard pressure will be 745 x 7.56 = 5644.2 L.
