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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 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).
How many cm in 630 mm?
630 mm = 630/10 = 63 cm
What does 1444 Torr equal in mm Hg?
1444 Torr is equal to 1925.06 mm Hg.
Psi equlas how many mm Hg?
1 psi is equal to approximately 51.715 mm Hg.
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 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 500 ml sample of gas at 760 mm Hg is compressed to 100 ml what is the new pressure?
To find the new pressure after the compression, you can use Boyle's Law, which states that pressure and volume are inversely related at constant temperature. Using the formula P1V1 = P2V2, where P1 = 760 mm Hg, V1 = 500 ml, V2 = 100 ml, you can calculate the new pressure (P2) by rearranging the formula as follows: P2 = P1V1 / V2 = (760 mm Hg * 500 ml) / 100 ml. Substituting these values gives you the new pressure after compression.
If 545 mL of oxygen gas is collected at 21ºC and 754 mm Hg what is its volume at STP?
502 mL
If 244 mL of oxygen gas is collected at 30ºC and 514 mm Hg what is its volume at STP?
149 mL
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.
If 665 mL of oxygen gas is collected at 20ºC and 784 mm Hg what is its volume at STP?
639-640 mL
If 565 mL of oxygen gas is collected at 25ºC and 744 mm Hg what is its volume at STP?
506 - 507 mL
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).
How many cm in 630 mm?
630 mm = 630/10 = 63 cm
Does a pressure of 350 mm Hg equals 350 pascal?
No. 1 mm Hg = 133.3224 pascal 350 mm Hg = 46662.84 pascal 1 pascal = 0.0075006 mm Hg 350 pascal = 2.62522 mm Hg
How to convert mm H2O IN mm hg in?
To convert millimeters of water (mm H2O) to millimeters of mercury (mm Hg), you can use the conversion factor of 1 mm H2O = 0.73556 mm Hg. Simply multiply the value in mm H2O by 0.73556 to obtain the equivalent value in mm Hg.
