Suppose some property q of a gas is proportional to (0.326 s m-u? + (7 s° m-v?. What is the average value of q? 1.3

How many moles of an ideal gas occupy 14.2L at 298K and 1.00atm (1.01bar) pressure?

53. Consider the initial. and final data for an ideal gas: Which expression gives the final volume, V2, in liters? Initial Final 3 atm 2L Temperature 300 K Pressure Volume 5 atm ?L 400 K (A) 2x 중x0 400 300 (B) 2× x 400 300 400 300 (D) 2x 를x200

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At what temperature does sulfur tetrafluoride have a density of 0.290 g/L at 0.0721 atm? Tap here or pull up for additional resources Question 6 of 33 C > 4-A b 1 4 7 +/- 2 5 8 27.5 K 3 6 9 O ||| 0 Submit C x 100 <

Calculate the volume of O2 gas in liters needed to metabolize (i.e., "combust") 1.00 gram of aqueous glucose (C6H12O6) under physiological conditions (at 37 degrees C and 0.200 atm). (correct sig. figs; no units included) The unbalanced chemical equation is: __C6H12O6 (aq) + __O2 (g) --> __CO2 (g) + __H2O (l)

The average kinetic energy of the molecules a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT rms speed = where R= 8.314 J/(mol-K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-m/s3). What is the rms speed of N, molecules at 365 K? rms speed: m/s What is the rms speed of He atoms at 365 K? rms speed: m/s

Hot gaes Expanding A mixture hot gases expands, changing volume from 2.45 L to 6.82 L, against a constant pressure of 3.22 atm. The P-Vwork involved is Latm .

The fermentation of glucose (wine making) reaction is shown below. During this process 780 mL of CO2 gas was produced at 37 oC and 1.00 atm. (R= 0.0821 LatmK-1mol-1)                                   C6H12O6(s)  +     6O2(g)      à      6CO2 (g)     +    6H2O (l)   a. Calculate the number of moles of CO2 produced in the above reaction?   b.What is the final volume, in liters, of the CO2 gas when measured at 22 oC and 675 mm Hg. ( 1 atm = 760 mm Hg)

Use the van der Waals equation of state to calculate the pressure of 3.30 mol of HI at 483 K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = atm Use the ideal gas equation to calculate the pressure under the same conditions. P = atm Under these conditions, would you expect HI or CCl, to deviate more from ideal behavior? Why? CCl because it occupies a larger volume and it has smaller dispersion forces between molecules. HI because it occupies a smaller volume and it has smaller dispersion forces between molecules. HI because it occupies a larger volume and it has smaller dispersion forces between molecules. CCI, because it occupies a larger volume and it has greater dispersion forces between molecules. HI because it occupies a smaller volume and it has greater dispersion forces between molecules. CCI, because it occupies a smaller volume and it has greater dispersion forces between molecules.