- 11 3269 G 10 5689 G 0 7580 G 13 1451 Mass Of Sulphamic Acid Beaker Mass Of Empty Beaker Mass Of Sulphamic Acid Mass Of 1 (27.52 KiB) Viewed 54 times
Pcol (kPa) the pressure exerted by the
water in the column.
2.At what temperature, in Kelvin, was the experiment
conducted?
3.Using the equation in the lab manual, calculate
PN2 (kPa), the
pressure of the nitrogen gas produced.
4.How many moles of sulphamic acid were used in the
test?
5.How many moles of sodium nitrite were used in the
test?
6.How many moles of nitrogen gas were produced during the
reaction?
7.Calculate the universal gas constant R (kPa L / mol K) from
the information collected and your calculated valuesthe value
determined will not match the actual value due to experimental
error
8.Calculate R in the SI units of J/(mol K)
Hint: the conversion from kPa L to J is given in the lab
manual.
11.3269 g 10.5689 g 0.7580 g 13.1451 Mass of sulphamic acid & beaker Mass of empty beaker Mass of sulphamic acid Mass of sodium nitrite & beaker Mass of empty beaker Mass of sodium nitrite Final water level in burette (mL) Initial water level in burette (mL) Total volume of N2 gas collected ( mL) Distance between level in burette & water level in beaker (cm) 12.3562 g 0.7889 g 18.45 mL 3.41 mL 13.1 cm 22.0 OC Room Temperature (°C) Atmospheric Pressure 100.4 kPa 2.643 kPa Vapour Pressure of water at 22°C obtained from the CRC Handbook of Chemistry and Physics 62nd Edition