pi = nRT
You know pi, R, and T (By the way, the new rules state that the degree sign is NOT used with Kelvin; i.e., you would write 300 Kelvin although 300o C is correct). Solve for n, then n = grams/molar mass to calculate molar mass.
Calculate the vapor pressure of water over each of the following ethylene glycol C2H6O2 solutions at 80 degree C (vp=pure water=657.6 mm Hg). Ethylene glycol can be assumed to be nonvolatile. (a) X (ethylene glycol)= 0.288 (b) %
A chemist has two ethylene glycol and water solutions: one that contains 11.98% ethylene glycol and another with 7.30% ethylene glycol. How many litres of each must be mixed to make 7.50 x 102 L containing 10.50% ethylene glycol?
A 13.03 g sample contains only ethylene glycol (C2H6O2) and propylene glycol (C3H8O2). When the sample is added to 100.0g of pure water, the resulting solution has a freezing point of -3.5C. What is the percent composition of
Hi Just want to know if water from a 20mm Polyethylene pipe under pressure of 3 bars passes to a 25mm polyethylene will cause a slight increase in volume output with a little drop in pressure? If yes then to obtain this benefit ,
1)If 746.4 g of a substance is dissolved in 1723 g of benzene solvent, the freezing point of the solution is -9.19 oC. Calculate the apparent molar mass (g/mol) of substance. 2) What mass ( g ) of the solvent water should be mixed
Okay so I know how I would normally determine molar mass of a compound *get out periodic table, sum up elements present, eg. H20 = [2(1.008)+16.00]g/mol* But this is for a lab class and they want us to derive it. Info found:
What is a minimum volume (in gallons) of ethylene glycol (CH2OHCH2OH, an antifreeze) that has to be added to 3.00 gal of water if you desire this engine cooling solution (for a auto radiator) NOT to be frozen below - 34.1 oC - a