p. Graham's LawLet's say you carried out the following, where you1. Prepare glass tubing to about a one (1) meter long.2. Fit corks on both end of the tube (Figure 3). To both end make a 2-cm mark.NH4OHHCIFigure 33. Prepare two cotton balls. Immerse one cotton ball in a conc. ammonium hydroxidesolution and the other with conc. hydrochloric acid.4. Simultaneously place the 2-soaked cotton balls on both ends of the tube. Now, putthe cork back.5. Observe carefully the formation of a white ring of ammonium chloride. Mark on theglass tubing the spot where the ring is formed. The distance traveled by theammonia gas is from the 2-cm mark to the spot of the ring and that of hydrogenchloride gas is from the other mark on its side to the ring spot. Measure theirdistances.6. Since the rate multiplied by the time equal to the distance and the time is taken to beconstant, the distance traveled may be substituted for rate, R, in the above equation.7. Using the data in your activity, calculate the ratio of the rate of diffusion of ammoniagas to that of hydrogen chloride gas. Compare the result of your calculation with thatobtained from the square root of their molecular weights. C. Graham's LawTable 3. Rate of DiffusionParameterSymbolResultDistance traveled by ammoniagasDistance traveled by HCI gasD12cmD2cmRatioD1: D2Molecular Weight of NH3MW14.12g/moleMolecular Weight of HCIMW26g/mole4.12:6RatioV MW1 : V MW2Write the balanced chemical equation for the reaction.

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Table 3. Rate of Diffusion Symbol D1 Parameter Result 2cm Distance traveled by ammonia gas Distance traveled by HCl gas Ratio D2 D1: D2 cm Molecular Weight of NH3 MW1 4.12g/mole Molecular Weight of HCI MW2 6g/mole 4.12:6 Ratio V MW1 : V MW2 Write the balanced chemical equation for the reaction.

Table 3. Rate of Diffusion Symbol D1 Parameter Result 2cm Distance traveled by ammonia gas Distance traveled by HCl gas Ratio D2 D1: D2 cm Molecular Weight of NH3 MW1 4.12g/mole Molecular Weight of HCI MW2 6g/mole 4.12:6 Ratio V MW1 : V MW2 Write the balanced chemical equation for the reaction.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section8.7: Kinetic-molecular Theory And The Velocities Of Gas Molecules

Problem 8.17E

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