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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.
Sixty Liters of gas were collected over water when the barometer read 670 60 L of a gas collected over water when the barometer read 670 mm Hg and the temperature was 20 C What volume would the dr?
since we know that the total pressure is 670 mmhg and the pressure of water at 20 c is 17.5 mmhg, we use dalton's law. 670=17.5+ gas pressure 652.5=gas pressure by definition then we use the law P1V1T2=P2V2T1 tp find V2=47.9969 L
What is the partial pressure of oxygen in blood gas a mixture of N2 O2 and CO2 if the partial pr. of Nitrogen 630 mm of Hg and partial pressure of CO2 is 39 mm of Hg?
To find the partial pressure of oxygen, we need to subtract the partial pressures of nitrogen and CO2 from the total pressure of the mixture, which is typically around 760 mmHg at sea level. Therefore, the partial pressure of oxygen would be 760 - 630 - 39 = 91 mmHg.
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 answer Convert the pressure 0.840 ATM to mm Hg?
1atm is equal to 760mmHg. Therefore, .520atm * 760mmHg/1atm = 395.2mmHg
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 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.
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).
A balloon contains a gas with a pressure of 580 mm Hg and a temperature of 227 degrees C What is the new pressure mm Hg of the gas when the temperature drops to 27 degrees C?
375mmhg
What If the manometer reading is 305 mm and the atmospheric pressure is 1.03 ATM what is the pressure of the gas in the flask?
478 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.
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.
If an anesthetic mixture used by a dentist has a total pressure of 740 torr and the partial pressure of the oxygen is 370 mm Hg what is the pressure in mm Hg of the nitrogen oxide the only remaining g?
Converting 740 torr to mm Hg: 1 torr = 1 mm Hg so 740 torr = 740 mm HgTotal pressure = partial pressure O2 + partial pressure N2O (nitrous oxide, not nitrogen oxide)Pressure of N2O = 740 mm Hg - 370 mm Hg = 370 mm Hg
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
If the atmospheric pressure is 24.9 inches what is the pressure in mm Hg?
To convert inches of mercury (in Hg) to millimeters of mercury (mm Hg), you multiply by 25.4. So, 24.9 in Hg * 25.4 mm/in = 632.46 mm Hg.
Sixty Liters of gas were collected over water when the barometer read 670 60 L of a gas collected over water when the barometer read 670 mm Hg and the temperature was 20 C What volume would the dr?
since we know that the total pressure is 670 mmhg and the pressure of water at 20 c is 17.5 mmhg, we use dalton's law. 670=17.5+ gas pressure 652.5=gas pressure by definition then we use the law P1V1T2=P2V2T1 tp find V2=47.9969 L
What is the partial pressure of oxygen in blood gas a mixture of N2 O2 and CO2 if the partial pr. of Nitrogen 630 mm of Hg and partial pressure of CO2 is 39 mm of Hg?
To find the partial pressure of oxygen, we need to subtract the partial pressures of nitrogen and CO2 from the total pressure of the mixture, which is typically around 760 mmHg at sea level. Therefore, the partial pressure of oxygen would be 760 - 630 - 39 = 91 mmHg.
