What is the mass (in grams) of 2.00 L of C,H,CI, at STP? R= 0.08314 L· 2' '2 bar/mol·K.

Mass of a vacuumed (empty) vessel of volume 5 L is 640.05 g, and mass of the same vessel filled with this hydrocarbon up to the pressure 2.0 atm at 22oC is 658.23 g. What is the molecular formula of the hydrocarbon?

A flask at room temperature contains equal numbers of di-nitrogen molecules and krypton atoms. (a) Which of the two gases exerts the higher partial pressure? (b) Which gas has a higher kinetic energy per molecule/atom? (c) Which gas has molecules with a higher velocity? Explain your answers.

A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)

A sample of 3.42 mol of xenon is confined at low pressure in a volume at a temperature of 86 °C. Describe quantitatively the effects of each of the following changes on the pressure, the average kinetic energy per molecule in the gas, and the root-mean-square speed. (a) The temperature is increased to 199 °C (b) The volume is tripled. (c) The amount of xenon is decreased to 1.87 mol Give each answer as a decimal factor of the form: new value factor old value. A factor of 1 means no change. ChangeP KEavgms

For the reaction A + B --> 2 C, Kç = 0.16. A 2.00 L flask is filled with 1.00 mol A and 1.00 mol B, and allowed to come to equilibrium. Determine the concentrations, in moles/liter, of A, B and C at equilibrium. (Do not input units, 3 sig figs). A = B = C =

A sample of H2(g) was collected over water in a volume of 12.0 mL at 18 °C under atmospheric pressure of 770. Torr. Partial pressure of water is P(H2O, 18 °C) = 16 Torr. Find the mol’s of H2(g) in the sample

Calculate the total pressure (in atm) of a mixture of 3.00 x 10-2 mol of helium, He, and 7.00 x 10- mol of oxygen, O2, in a 6.00 L flask at 20.°C. Assume ideal gas behavior. Total pressure atm ||

What is the pressure of a mixture of 0.0500 g of H2, 1.00 g of N2, and 1.60 g of Ar in a container with a volume of 4.00 L at 20 °C?

lithium reacts with H2O to produce hydrogen.(a) Write a balanced chemical equation for the reaction, using the smallest integer coefficients possible. Write states in brackets. (Hint: LiOH is the second product.) (b) Calculate the mass of pure Li that will furnish 16.3 L of hydrogen at a pressure of 0.860 atm and a temperature of 30.4°C.