Calculating partial pressure in a gas mixture A 6.00 L tank at 2.95 °C is filled with 20.0 g of sulfur hexafluoride gas and 5.86 g of boron trifluoride gas. You can assume both gases behave as ideal gases
under these conditions.
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
mole fraction:
DI
sulfur hexafluoride
partial pressure:
atm
Х
5
?
mole fraction:
0
boron trifluoride
partial pressure:
atm
Total pressure in tank:

This is a characteristic of the elements in the periodic table that shows a pattern. it may increase or decrease across or down the table.

Lab reagent, hypothesis test.a reference solution used as a lab reagent is purported to have a concentration of 5 mg/dl. six samples are taken from this solution and the following concentrations are recorded: (5.32, 4.88, 5.10, 4.73, 5.15, 4.75) mg/dl.these six measurements are assumed to be an srs of all possible measurements from solution.they are also assumed to have a standard deviation of 0.2, a normal distributin, and a mean concentration equal to the true concentration of the solution.carry out a significance test to determine whether these six measurements provide reliable evidence that the true concentration of the solution is actually not 5 mg/dl.

Which statement are accurate about snow flakes