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# Graham's law. In this experiment the relationship between the molar mass of a gas and the speed with which it diffuses was to be assessed.

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Introduction

Abstract In this experiment the relationship between the molar mass of a gas and the speed with which it diffuses was to be assessed. The idea we had behind finding this relationship was to first form a participate and measure the distance from this participate ring. In Graham's Law a gas's rate of effusion is inversely proportional to the square root of its molecular weight. Because of this, by finding the molar mass and distance from the participate ring the relationship can be experimentally analyzed. ...read more.

Middle

Next, in the fume hood, an end of the cotton swab was soaked into the 12 M HCl and another in the 17 M NH3. After being soaked for a brief period of time each were inserted simultaneously into opposite ends of one of tubes and covered with paper towels to prevent excess air flow. This was repeated twice and a white ring participate was formed. The distance of this ring to both ends is then measured and recorded. Data Table 1: Raw Data Trial Number 1 2 3 Diameter of tube (cm +/- 0.01) ...read more.

Conclusion

In terms of validating Graham's Law our experiment did in that because we demonstrated that the NH3 diffused faster. This coincides with Graham's Law because the lighter the gas the faster it diffuses. Further Questions a) If the temperature was changed then nothing will occur because according to Graham's law temperature is not a factor. However, if the molar masses were changed then the rate will changed in an inversely proportional matter. b) oxygen r1 = 1.03r2 1.03r2/r2 = sq. root (m2/32) 1.03 = sq. root (m2/32) 1.06 = m2/32 33.95 = Unknown gas Cartagena 3 Table #N/A Graham's Law #6 ...read more.

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