A gas mixture consists of 320 mg (0.320 g) of methane (CH4), 175 mg of argon (Ar) and 225 mg of neon (Ne). The partial pressure of neon at 300 K is 66.5 Torr. Calculate (a) the volume of the mixture (b) the partial pressure of argon (c) the total pressure of the mixture.

in the following reaction, 27.1 mL of o2(g) is collected over water at 23*C and barometric pressure 751 mmHg. After the reaction, the buret could not be lowered far enough to make the water levels equal in both the burette and beaker. In fact, you measured the difference in water levels to be 34 mm, what must have been the mass of the Ag2O decomposed? (the vapor pressure of water at 23* C is 21.1 mmHg)

(a) (c) A column of water in a buret is 336 mm Hg high. How high would that column be if it were mercury instead of water? (d) In order for the pressures to be equal, density and height of a column are inversely proportional, therefore the following relationship applies: (denHg)(hHg) = (denH20)(hH20) Note: the density of mercury is 13.6 g/mL and the density of water is 1.00 g/mL. An electrolysis experiment was run for 15 minutes and 45 seconds at an average current of 189 milliamps (mA). The mass lost by the copper anode was 0.0589 grams. (b) Calculate the number of coulombs transferred. (Remember: coulomb = amps x sec) Show full calculation of the height in mercury (remember to use proper significant figures.) Calculate the moles of copper lost from the anode. Based on the moles of copper lost determined in 1c, calculate the moles of electrons transferred. Remember, the reaction at the copper anode is: Cu(s)---> Cu¹² (aq) + 2 e

Elemental analysis of an organic liquid with a fishy odour gives the following elemental mass percentages: H 14.94 % C 71.22% N 13.84 %. Vaporization of 270 mg of an impure sample in a 150-mL bulb at 150oC gives a pressure of 435 torr. What is the molecular formula of the compound, and the % purity of the sample?