How to calculate the blank which I don\'t fill. I need the details and steps how

Question

How to calculate the blank which I don't fill. I need the details and steps how to calculate them. of the (and The procedure involves heating NaHCO, to produce COs gas. Measurements mass number of moles) of the gas, its volume, and the temperature and pressure will permit inspection of the desired relationships. Most of these measurements must be made indirectly, since it is difficult to do so water vapor as described below. otherwise. In particular, the experimental gas pressure must be corrected for the effect of EXPERIMENTAL PROCEDURES Prepare the apparatus as illustrated in Figure 1. The pyrex test tube must be clean and thoroughly dry. Fill the 500 mL flask with water, and have about 100 ml of water in the 600 mL beaker. Fill the rubber tube B with water by blowing into rubber tube A. Syphon water back and forth through tube B, by raising and lowering the beaker, to expel all air bubbles. Finally, with the flask nearly VII-1

Explanation / Answer

I am going to show you how to do the calculations for trial 1

I. (a) Mass loss = 0.6189 g

(b) water vapor pressure at 22 oC (from graph) = 19.763 mmHg

II. calculations

(a) Mass of CO2 collected

mass loss = 95.08 - 04.4611 = 0.6189 g

moles of NaHCO3 = mass/molar mass = 0.6189/84.007 = 7.37 x 10^-3 mols

So, moles of CO2 = 7.37 x 10^-3/2 = 3.68 x 10^-3 mols

moles of CO2 = mass/molar mass = 0.6189/44.01 = 0.0141 mols

(b) system Temperature (K) = 22 oC + 273 = 295 K

(c) Pressure of CO2 = 29.88 - 19.763 = 10.117 mmHg = 0.0133 atm

(d) Experimental R = pV/nT = 0.0133 atm x 0.242 L/3.68 x 10^-3 mols x 295 K = 2.96 x 10^-3 L.atm/K.mol

(e) Molar volume (Vm) = 0.242/3.68 x 10^-3 = 65.76 L.mol-1

(f) standard molar volume at STP = 0.242 x 273 x 0.0133/3.68 x 10^-3 x 295 x 1 = 0.81 L.mol-1

Similarly the calcualtions for trial 2 and 3 can be done

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