From earlier parts of the problem: 0.02979 moles Zn, 0.03 moles H 2 , and 22.8 t

Question

From earlier parts of the problem: 0.02979 moles Zn, 0.03 moles H2, and 22.8 torr

22. DISCUSSION Next, using your calculated values for the number of moles, n, the corrected pressure, Pcorr, of H2, and the ideal gas equation, PV=nRT, determine the volume of the pressure vessel (in liters) and enter below. Note 1. Assume that the final system temperature is 22 degree C. Note 2. Remember to convert P and T to units that correspond to those used in the gas constant, R. You may return to the Lab Details page, click REFRESH ALL, and check other students' values for the pressure vessel volume. The low, high and mean reported values will be displayed after you enter your calculated volume.

Explanation / Answer

PV = nRT, and rearranging,

V = nRT / P

Here, in pressure units, R = 0.08314 dm3 bar K-1 mol-1

Since the gas constant unit is there in bar, we will also convert 22.8 torr into bar units below:

bar = torr × 0.00133322368

bar = 22.8 x 0.00133322368 = 0.0304 bar

Temperature also should be taken in Kelvin for the same reason.

T = 273.15 + 22 = 295.15 K

Apply all the values in ideal gas equation,

V = nRT / P

V = [(0.03 mol) x (0.08314 dm3 bar K-1 mol-1) x (295.15 K)] / 0.0304 bar

V = 24.216 dm3

V = 24.216 liters

(Use 295K instead of 295.15K in the calculation, if you are instructed to use just 273K for absolute zero temperature)

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