Description 1. A prevailing pressure of one standard atmosphere will support a column of mercury 76 ...

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Description 1. A prevailing pressure of one standard atmosphere will support a column of mercury 760 mm in height. Liquid carbon tetrachloride has a density of 1.59 g/mL. The height of a column of carbon tetrachloride that one standard atmosphere can support is ______ mm. The density of liquid mercury is 13.6 g/mL. 2. Liquid methylene chloride has a density of 1.33 g/mL. A barometer is constructed using methylene chloride instead of mercury. If the atmospheric pressure is 0.952 atm, what is the height of the methylene chloride column in the barometer in cm? The density of liquid mercury is 13.6 g/mL. 3. A sample of oxygen gas occupies a volume of 9.58 L at 46 °C and 0.638 atm. If it is desired to increase the volume of the gas sample to 12.1 L, while decreasing its pressure to 0.413 atm, the temperature of the gas sample at the new volume and pressure must be  _____  °C. 4. A sample of gas contains 0.1400 mol of H2(g) and 7.000E-2 mol of O2(g) and occupies a volume of 7.05 L. The following reaction takes place: 2H2(g) + O2(g)--->2H2O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. 5. A sample of gas contains 0.1100 mol of CH4(g) and 0.2200 mol of O2(g) and occupies a volume of 11.9 L. The following reaction takes place: CH4(g) + 2O2(g)--->CO2(g) + 2H2O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. 6. A sample of oxygen gas collected at a pressure of 0.851 atm and a temperature of 29.0 °C is found to occupy a volume of 28.1 liters. How many moles of O2 gas are in the sample? _____ mol 7.  A sample of helium gas collected at a pressure of 0.578 atm and a temperature of 297 K is found to occupy a volume of 530. milliliters. How many moles of He gas are in the sample? 8. A sample of helium gas collected at a pressure of 797 mm Hg and a temperature of 277 K has a mass of 2.31 grams. The volume of the sample is  _____ L. 9. According to the ideal gas law, a 0.9150 mol sample of nitrogen gas in a 1.753 L container at 265.8 K should exert a pressure of 11.38 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For N2 gas, a = 1.390 L2atm/mol2 and b = 3.910E-2 L/mol. Hint: % difference = 100 x (P ideal - Pvan der Waals) / P ideal 10. What volume of hydrogen sulfide is required to produce 29.6 liters of sulfur dioxide according to the following reaction? (All gases are at the same temperature and pressure.) hydrogen sulfide (g) + oxygen(g)--->water (l) + sulfur dioxide(g) _____ L Hydrogen Sulfide