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Both volume (V) and quantity (n) of the gas have to be known to calculate, not only the pressure by Gas Law:
p . V = n . T . (R)
in which (R) is the general 'gas constante': 8.3145 (J/mol.K)
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The pressure of a sample of gas at 10.0 C increases from 700 mm Hg to 900 mm Hg What is the new temperature?
39.0
What is the pressure in mm Hg of a gas at 2atm?
1 atm of pressure equals 760 mm Hg, so 2 atm = 1520 mm Hg.
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?
If the total (=atmospheric) gas pressure is 760 mm Hg, then the remaining partial pressure of 760 - (630 + 39) = 91 mm of Hg is for the 3rd gas in blood: Oxygen (O2)
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
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
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
The pressure of a sample of gas at 10.0 C increases from 700 mm Hg to 900 mm Hg What is the new temperature?
39.0
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
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?
190 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.
What is the pressure in mm Hg of a gas at 2atm?
1 atm of pressure equals 760 mm Hg, so 2 atm = 1520 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 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?
If the total (=atmospheric) gas pressure is 760 mm Hg, then the remaining partial pressure of 760 - (630 + 39) = 91 mm of Hg is for the 3rd gas in blood: Oxygen (O2)
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?
161 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
What would be the pressure in mm Hg if this gas was allowed to expand to 975 ml at a constant temperature?
This cannot be answered without an initial volume or pressure. But the final pressure of an expansion of a gas can be determined by the following formula. PV/T = P'V'/T' where P = pressure absolute V = volume T = temperature absolute ( ' ) indicates the new pressure, volume and temperature because the temperature is constant this can be reduced to PV = P'V' or P' = PV/V'
What pressure in kilopascals and in atmospheres does a gas exert at 385 mm Hg?
pressure in kilopascals = 3.38639 x (pressure in Hg/10) = 274.636229 kpa ~274.64 kpa
