Course and lab section: Lab instructor\'s name: Raw Data from potassium chlorate

Question

Course and lab section: Lab instructor's name: Raw Data from potassium chlorate decomposition reaction Post-Lab Calculations and Analysis 1. Complete the following, and enter these preliminary results in the Table 3. a. Calculate the mass (grams) of oxygen produced. b. Calculate the number of moles of oxygen gas by using the molar mass of O_2. c. Calculate the volume of oxygen gas, and convert to units of liters (L). d. Calculate the pressure of oxygen gas by using the barometric pressure and pressure from the water vapor. e. Convert the room temperature to degrees Kelvin (K). f. Calculate the idea gas constant R (in units of L-atm/mol-K) from your experimental results by using Equation 2. 2. Complete the following, and enter these final results in the Table 4. a. Enter your experimental value for the ideal gas constant. b. Look up the theoretical value for the ideal gas constant, in units of L-atm/mol-K. c. Calculate the percent error between the experimental and theoretical values.

Explanation / Answer

2KClO3 = 2KCl + 3O2

(a) mass of O2 produced = 0.04 gm

(b) moles of O2 produced = 0.04 gm/32g/mol = 1.25*10^-3 moles

(c) volume of O2 gas = final-initial = 35-2 = 33mL = 0.033 L

(d) Ptotal = P(O2 ) + P(water vapor)

P(water vapor) at 24.2oC =22.4 torr (standerd value) = 1atm *22.4 torr/ 760 torr = 0.029 atm

P(O2) = 0.97 atm - 0.029 atm =0.941 atm

(e) T = 24.2oC = 297.2 K

(f) PV = nRT

     or, R = PV/nT

              = 0.941 * 0.033 L/ 1.25*10^-3 moles *297.2 K = 0.0835 Latm/K/mol

            

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