PROBLEM 4: A gas at 300.0 K and 6.00 atm has a molar volume 9.00% larger than that calculated from the ideal gas law. Calculate: (a) the compressibility (i.e. compression) factor under these conditions; (b) the molar volume of the gas, Vm. Also, answer this question: (c) which dominate in this system, attractive or repulsive forces?

perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.

Scottish physicist W. J. M. Rankine proposed an absolute temperature scale based on the Fahrenheit degree, now called degree Rankine abbreviated R and used by some engineering fields. If a degree Rankine is 5/9 of a degree Kelvin, what is the value of the ideal gas law constant in L. atm/mol. R?

5-107 If 60.0 g of NH3 occupies 35.1 L under a pressure of 77.2 in. Hg, what is the temperature of the gas, in °C?

Calculate U when 1.00 mol of H2 goes from 1.00 atm, 10.0 L, and 295 K to 0.793 atm, 15.0 L, and 350 K.

The compression ratio in an automobile engine is the ratio of the gas pressure at the end of the compression stroke to the pressure in the beginning. Assume that compression occurs at constant temperature. The total volume of the cylinder in an automobile is 350 cm3, and the displacement the reduction in volume during the compression stroke is 309 cm3. What is the compression ratio in that engine?

5-54 Automobile air bags are inflated by nitrogen gas. When a significant collision occurs, an electronic sensor triggers the decomposition of sodium azide to form nitrogen gas and sodium metal. The nitrogen gas then inflates nylon bags, which protect the driver and front-seat passenger from impact with the dashboard and windshield. What volume of nitrogen gas measured at 1 atm and 27°C is formed by the decomposition of 100. g of sodium azide?

Suppose a uniform ideal gas of total mass M, temperature T and N particles. What is the (²) of each molecule when the gas is: (a) monatomic? (b) diatomic? (The molecules rotate but do not oscillate.)

Please answer completely. Thank youu!

6. a) What would be the expected temperature of a .75mg sample of H2 gas compressed to real gas conditions at 4.0 atm in a 50ml airtight volumetric flask? b) What fraction of the total 50mL volume is occupied by the gas particles? Hint: consider the corrective term for the volume of the gas particles with respect to container volume.