The density of an unknown gas is found to be 2.82 g/L at standard temperature and pressure (STP). What is the molar mass of this gas?

A sample of gas at 298 Kelvin and 0.98 atmospheres has a density of 1.45 g/L. What is the molar mass of this gas? Show all of the work used to solve this problem.

A 14.5-gram sample of gas is found to have a volume of 1.1 liters at 275 K and 1.3 atm. What is the molar mass of this gas? Show all of the work used to solve this problem.

Explain Dalton's law of partial pressures and how it relates to the collection of gas by water displacement.

Which of the following aqueous solutions will have the lowest vapor pressure at 25 degrees Celsius?

1.0 M CH_{4}

1.0 M NaCl

1.0 M AlCl_{3}

1.0 M BaCl_{2}

A solution is made by dissolving 19.5 grams of glucose (C_{6}H_{12}O_{6}) in 0.245 kilograms of water. If the molal freezing point constant for water (K_{f}) is -1.86 °C/*m*, what is the resulting Δ_{f} of the solution? Show all he steps taken to solve this problem. (4 points)

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#### Top Answer

1)The molar mass of unknown gas = 63.24 g/mol 2) The molar mass of this gas= 36.2 g/mol 3) Molar... View the full answer