A 2.56-g sample of a colorless liquid was vaporized in an evacuated 250.-mL flask at 121°C to give a pressure of 786 mmHg. What is the molecular weight of this substance? Molecular weight = amu

When 0.1 mol of HCl gas is placed in a 10 liter box at 25 degree C, the pressure is about the same as that observed when 0.1 mol of NH3 is placed in an identical box at the same temperature. However, when 0.05 mol of HCl and 0.05 mol of NH3 are mixed in a 10 Liter box at 25 degree C, a noticeable lower pressure is observed. Explain this behavior.

8) Consider the apparatus pictured below, which consists of two containers separated by a valve. CH;N(g) 285 mL O2(g) 419 mL 591 torr 1766 torr The valve is opened and the gases react as follows (note that the temperature is high enough that the water is produced as a gas): 4 C2H;N(g) + 15 O2(g) → 8 CO2(g) + 14 H2O(g) + 2 N2(g) What will be the total pressure in the apparatus when the reaction has gone to completion? Assume that the temperature does not change.

After 0.600 L of Ar at 1.19 atm and 240.0 °C is mixed with 0.200 L of O₂ at 428. torr and 110.0 °C in a 400.- mL flask at 28.0 °C, what is the pressure in the flask? Be sure your answer has the correct number of significant figures. Note: Reference the Conversion factors for non-SI units, Fundamental constants and SI prefixes tables for additional information. atm

4.)  (a)  0.375 g of CO2 gas is held in a 520.-mL container at 24. oC.  What is its pressurre?                                                                                                                                    atm (b) 0.375 g of N2 are held in an identical container at the same temperature.  What is its pressure?                                                                                                                           atm (c) Are the pressures the same or different?  Why?                                                                                         (d) If both these samples were contained in the same 520.-mL container, what would the partial pressure of each gas be?  What would the total pressure be? (FYI, these gases do not react.)       PCO2=                          atm                                                                                                                                     PN2=                            atm…

11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b)  The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.

A 22.5 mL sample of liquid ethanol (C₂H₅OH, density = 0.789 g/mL) was injected into a 10.0 L cylinder containing O₂ at a pressure of 4.50 atm and a temperature of 25°C. The cylinder was heated to 125°C and a spark was used to ignite the ethanol, which was completely combusted. What was the final total pressure in the cylinder (in atm) after the reaction, while it was still at 125°C?

Gaseous CO exerts pressure of 45.6 mmHg in a 56.0 L tank at 22°C was released to a room with a volume of 2.70 x 104L. The room has another two gaseous that are 5.50 g of NO2 and 8.034 x 1022 atoms of SO2 at 22°C. Calculate the partial pressure of CO in the room at 22°C. •Ans : P = 0.09458 mmHg Calculate the total pressure in the room and the molarity of CO gas in the room. •Ans: 5.14 x 10-6 M, Total pressure 2,7 x 10-4 atm Calculate the density of the mixture in the room and the mass percentage of SO2 gas in the room. 6.00027

Oxygen gas can be prepared by heating potassium chlorate according to the following equation: 2KCIO3(s)2KCI(s) + 302(g) The product gas, O2, is collected over water at a temperature of 25 °C and a pressure of 758 mm Hg. If the wet O2 gas formed occupies a volume of 8.11 L, the number of grams of O, formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C.

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