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What is the density in g L of carbon dioxide gas at 7.40 102 torr and 37.0ºC Molar mass of carbon dioxide equals 44.0 g mol?
To calculate the density of carbon dioxide gas, first convert the pressure to atm (1 atm = 760 torr). Next, use the ideal gas law: PV = nRT to find the number of moles of CO2. Then, divide the mass of CO2 (44 g/mol) by this number of moles to find the density in g/L.
What is the partial pressure of N2 and O2 having a total pressure of 1075 torr if the partial pressure of 02 is 720 torr?
1075 torr - 720 torr = 355 torr
Uranium hexafluoride is a solid at room temperature but it boils at 56C Determine the density of uranium hexafluoride at 68C at 743 Torr?
To determine the density of uranium hexafluoride at 68°C and 743 Torr, you need to use the ideal gas law equation in combination with the density formula. First, calculate the pressure at 68°C using the ideal gas law. Then, use the density formula (density = (mass * molar mass) / volume) to find the density of uranium hexafluoride at the given conditions.
How many kPa are equal to 1250 torr?
1 torr is equal to 1.33322 kPa. Therefore, 1250 torr is equal to 1666.53 kPa.
What is 456 Torr into standard atmospheres?
456 Torr is equivalent to 0.601 standard atmospheres. This conversion is done by dividing the pressure in Torr by 760 (the number of Torr in 1 standard atmosphere).
What is the density in g L of carbon dioxide gas at 7.40 102 torr and 37.0ºC Molar mass of carbon dioxide equals 44.0 g mol?
To calculate the density of carbon dioxide gas, first convert the pressure to atm (1 atm = 760 torr). Next, use the ideal gas law: PV = nRT to find the number of moles of CO2. Then, divide the mass of CO2 (44 g/mol) by this number of moles to find the density in g/L.
What is the density of oxygen gas at 77 degrees C and 700 Torr?
The density of oxygen gas at 77°C and 700 Torr pressure is approximately 1.429 g/L.
The gases in a mixture have the following partial pressures at the same volume and temperature 1013000 Pa nitrogen 700 mm argon 1.20 ATM of helium 790 torr oxygen and 0.50 ATM of carbon dioxide?
Carbon dioxide Argon Oxygen Helium Nitrogen
What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2 degrees C when it occupies a volume of 5.00 L?
The pressure exerted by the carbon dioxide gas is 22.8 torr. This can be calculated using the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Given the mass of the gas, the number of moles can be calculated and used to determine the pressure.
What is the density in g/L of fluorine gas at 7.00 × 102 torr and 27.0ºC?
1.42
What is the density in gL of chlorine gas at 7.50 102 torr and 25.0ºC?
The density of chlorine gas at 7.50 × 10^2 torr and 25.0ºC can be calculated using the ideal gas law. First, convert the pressure to atm (7.50 × 10^2 torr = 0.988 atm). Then, use the ideal gas law equation: PV = nRT and rearrange it to solve for density (density = PM/RT where M is the molar mass of chlorine gas). Substituting the values and calculating will give the density in g/L.
What is the vapor pressure of C2H5OH in torr?
The vapor pressure of carbon tetrachloride is 11.94 Pa at 20°C This is 0.0896 torr or 89.6 mTorr
What is the pressure in Torr at 4345 meters?
The pressure at 4345 meters is approximately 529 Torr. This can be calculated using the barometric formula, which takes into account the decrease in pressure with increasing altitude. At higher altitudes, the atmospheric pressure decreases due to the lower density of air molecules.
One torr is equal to?
1 Torr = 0.00133322 bar 1 Torr = 133.322 Pa 1 Torr = 0.00131578584 ATM 1 Torr = 1 mmHg
What is the partial pressure of N2 and O2 having a total pressure of 1075 torr if the partial pressure of 02 is 720 torr?
1075 torr - 720 torr = 355 torr
What is the correct perssure in ATM pressure if the air is 742 torr?
1 torr is 0.00131578947 atm. Therefore, 742 torr is 0.976315789 atm.
A closed end manometer has a U tube with a sample of hydrogen gas in the bulb The difference in the height of the columns of mercury is 18.0 cm What is the pressure of the hydrogen gas in torr?
To find the pressure of the hydrogen gas in torr, you can use the difference in height of the mercury columns and the density of mercury. First, calculate the pressure difference due to the 18.0 cm height difference in the mercury columns. Then, convert this pressure into torr using the conversion factor 1 atm = 760 torr.
