Given You are heating potassium perchlorate and collecting the oxygen gas from the decomposition over water. Write equation. 2 KClO3(s) ----------> 2KCl (s) + 3O2 (g)             Mass of sample: 0.398 g              Ambient pressure: 752.3 mmHg              Volume of gas: 81.4 mL              Room temperature: 18.9 degrees Celsius   Using the mass of your KClO4 sample, and the balanced equation, calculate the theoretical yield of O2 gas in grams. The theoretical yield of O2 gas is 0.155 g. 1. Using the equation from the graph posted on Moodle with vapor pressure of water versus temperature, find the              vapor pressure of water at your temperature:  18.9 degrees celsius (i think this is right.)             Vapor pressure of water at given temperature: 2.  Now using your total pressure, and the vapor pressure of water at your temperature, find the pressure of O2 gas in your sample, in atm.   3.   How many moles of O2 gas were actually produced?  (Assume ideal behavior of the gas).

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Given

You are heating potassium perchlorate and collecting the oxygen gas from the decomposition over water. Write equation.

2 KClO3(s) ----------> 2KCl (s) + 3O2 (g)

            Mass of sample: 0.398 g 

            Ambient pressure: 752.3 mmHg 

            Volume of gas: 81.4 mL 

            Room temperature: 18.9 degrees Celsius  

Using the mass of your KClO4 sample, and the balanced equation, calculate the theoretical yield of O2 gas in grams.

The theoretical yield of O2 gas is 0.155 g.

1.

Using the equation from the graph posted on Moodle with vapor pressure of water versus temperature, find the 

            vapor pressure of water at your temperature:  18.9 degrees celsius (i think this is right.)

            Vapor pressure of water at given temperature:

2.

 Now using your total pressure, and the vapor pressure of water at your temperature, find the pressure of O2 gas in your sample, in atm.

 

3.

  How many moles of O2 gas were actually produced?  (Assume ideal behavior of the gas). 

 

 

Vapor Pressure of Water
8.
7
y = -5206.4x + 20.621
R² = 0.9999
2
0.0025
0.0027
0.0029
0.0031
0.0033
0.0035
0.0037
0.0039
1/T (K4)
Figure 1: Use the above table to determine the vapor pressure of water (partial pressure of water) at room
temperature.
In P (mmHg)
Transcribed Image Text:Vapor Pressure of Water 8. 7 y = -5206.4x + 20.621 R² = 0.9999 2 0.0025 0.0027 0.0029 0.0031 0.0033 0.0035 0.0037 0.0039 1/T (K4) Figure 1: Use the above table to determine the vapor pressure of water (partial pressure of water) at room temperature. In P (mmHg)
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