Suppose you start with a liquid mixture of 60% nitrogen and 40% oxygen. Describe what happens as the temperature of this mixture increases. Be sure to give the temperatures and compositions at which boiling begins and ends.

A solution of methylene chloride (CH2Cl2) and ethanol (CH3CH2OH) that is 10.% methylene chloride by mass is boiling at 75°C. The vapor is collected and cooled until it condenses to form a new solution. Calculate the percent by mass of methylene chloride in the new solution. Here's some data you may need:   normal boiling point density vapor pressure at  75°C methylene chloride 40.°C 1.3g/mL 2263.torr ethanol 78.°C 0.79g/mL 669.torr Be sure your answer has 2 significant digits.   Note for advanced students: you may assume the solution and vapor above it are ideal.

You synthesized a sample of tetramethylammonium triiodide and managed to measure the melting point. However, the melting point deviates from the ideal melting point for tetramethyl-ammonium tri-iodide, which is 117 degrees C. This suggests that your sample may be impure. Unfortunately, you ran out of time and were unable to carry out the gravimetry. Your demonstrators agreed to help you out, but instead of using gravimetry, they carried out the elemental analysis of your product. The sample contains C - 9.27 %, H -2.33 %, and N - 2.70 %. How many iodine atoms does your sample have according to this analysis?

Given the following information, determine the percentage by mass of cyclohexane in the mixture. volume of the solution in mL 3.15 Vapor temperature when distillation of cyclohexane started (°C) 80.95 Vapor temperature when distillation of cyclohexane finished (°C) 83.09 Volume of cyclohexane collected in mL 1.60 Vapor temperature when distillation of toluene started (°C) 110.81 Vapor temperature when distillation of toluene finished (°C) 111.88 Volume of toluene collected in mL 1.55