However, my understanding is that the molar fraction is $\text{moles of Ar} / \text{total moles}$, so I need the number of moles for each substance in the mixture, not the pressures. Or perhaps the molar fraction can also be calculated by $\text{pressure of Ar} / \text{total pressure}$? $\endgroup$ - Voldemort Jul 15 '15 at 16:48
Jun 22, 2017 · What is the molar mass of a gas whose density is 0.761 g/L at STP? Step 1: List the known quantities and plan the problem. Known. density = 0.761 g/L; 1 mol = 22.4 L; Unknown. molar mass = ? g/mol; Molar mass is equal to density (in g/L) multiplied by molar volume. Step 2: Calculate. Step 3: Think about your result. Because the density of the gas is less than 1 g/L, the molar mass is less than 22.4 g/mol.
X is the component that is being identified for mole fraction. Example: Calculate the mole fraction of carbon tetrachloride (CCl 4) in solution if 2.5 moles of CCl 4 is dissolved in 8.0 moles of benzene (C 6 H 6).
density of dextrose, Oral glucose (15 to 20 grams) is the preferred treatment for the conscious patient, although any form of carbohydrate that contains glucose may be used. Glucose and dextrose administration pose no particular risks during breast-feeding.