2. (3) Corey and Nicole performed the same experiment that you did last week. Th

Question

2. (3) Corey and Nicole performed the same experiment that you did last week. They collected the following data. Calculate the value of R from their data. Determine their % error. 1 liter, 1000 ml; MW of O2 = 32.0 Barometric Pressure: 756 torr Temperature: 22°C Vapor Pressure of H2O at 22°C: 20.0 torr mass of tube+KCIOs before heating: 8.3078 g mass of tube +contents after heating: 8.2585 g Initial buret reading: 0.1 ml Final buret reading: 38.7 ml heat Unbalanced Reaction: KCIO3(s)KCl(s) +O2(9) 3. (3) What is Boyle's law (include an equation expressing the relationship between the volume and the pressure of a gas)? What equipment (or apparatus) did you use to verity Boyle's law? How did you verify Boyle's law from last week's experiment?

Explanation / Answer

Q2

balance

KClO3 = KCl + O2

KClO3 = KCl + 3/2O2

Apply Ideal Gas Law,

PV = nRT

where

P = absolute pressure

V = total volume of gas

n = moles of gas

T = absolute Temperature

R = ideal gas constant

PV = nRT

R = PV/(nT)

Pgas = Ptotal - Pvapor = 756-20 = 736

V = Vfinal - vinitial = 38.7-0.1 = 38.6 mL = 38.6*10^-3 L

mass of O2 = 8.3078 - 8.2585 = 0.0493 g

mol = mass/MW = 0.0493/32 = 0.00154

T = 22C° = 22+273 = 295 K

R = (736)( 38.6*10^-3)/(0.00154*295 )

Rcalculated = 62.5349 torrL/molK

now...

Rreal = 62.3637

%error = (62.3637 -62.5349 )/(62.3637 ) * 100 = 0.2745%

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