Evaluation of a Gas Constant (Experiment 3)
Experiment 3: Evaluation of Gas Constant
Purpose:
The purpose of this lab is to demonstrate the ideal gas law under ordinary conditions. In this lab, the variables in the ideal gas law are known or can be found aside from the constant R. Thus, the R values can be found and relatively determine the relevancy of the ideal gas law to the lab conditions. The ideal gas law was tested using the reaction:
Mg (s) + 2HCl2 (aq) H2 (g)
Procedure:
1. Ribbons of magnesium (5) were cut to the approximate length of the instructor’s example and were weighed separately on scale #1. 2. HCl provided by the instructor was added to a eudiometer tube (8mL). The rest of the tube was filled with water. One of the magnesium tapes was wrapped around a piece of copper wire in the opening of the tube. 3. The eudiometer tube was then inverted over and into a 450 mL beaker with water. The initial volume was recorded. 4. While the reaction occurred, the temperature was taken at 1 minute intervals for 3 minutes. 5. After the reaction occurred, the height difference from the solution within the eudiometer tube and the top of the liquid volume in the beaker was recorded. The final volume was also recorded.
Summary Table:
Mean of R= .0737
Standard Deviation= .0298
Relative Standard Deviation= 40.46%
Summary Table:
Mean of R= .0737
Standard Deviation= .0298
Relative Standard Deviation= 40.46%
Discussion:
This lab was supposed to generate numbers close to the R constant by plugging in the values acquired in reaction Magnesium and Hydrochloric acid reaction. (The reaction results in H2 gas.) The mean acquired from our data set was .0737 L-ATM/mol-K as opposed to the actual constant .08206 L-ATM/mol-K. The constant we acquired was much lower in value, potentially due to the outlier in our data set: Trial Four.
Trial Four resulted in the R value .0205 ATM-L/K-mol which skewed our relative mean, standard deviation and relative standard
Purpose:
The purpose of this lab is to demonstrate the ideal gas law under ordinary conditions. In this lab, the variables in the ideal gas law are known or can be found aside from the constant R. Thus, the R values can be found and relatively determine the relevancy of the ideal gas law to the lab conditions. The ideal gas law was tested using the reaction:
Mg (s) + 2HCl2 (aq) H2 (g)
Procedure:
1. Ribbons of magnesium (5) were cut to the approximate length of the instructor’s example and were weighed separately on scale #1. 2. HCl provided by the instructor was added to a eudiometer tube (8mL). The rest of the tube was filled with water. One of the magnesium tapes was wrapped around a piece of copper wire in the opening of the tube. 3. The eudiometer tube was then inverted over and into a 450 mL beaker with water. The initial volume was recorded. 4. While the reaction occurred, the temperature was taken at 1 minute intervals for 3 minutes. 5. After the reaction occurred, the height difference from the solution within the eudiometer tube and the top of the liquid volume in the beaker was recorded. The final volume was also recorded.
Summary Table:
Mean of R= .0737
Standard Deviation= .0298
Relative Standard Deviation= 40.46%
Summary Table:
Mean of R= .0737
Standard Deviation= .0298
Relative Standard Deviation= 40.46%
Discussion:
This lab was supposed to generate numbers close to the R constant by plugging in the values acquired in reaction Magnesium and Hydrochloric acid reaction. (The reaction results in H2 gas.) The mean acquired from our data set was .0737 L-ATM/mol-K as opposed to the actual constant .08206 L-ATM/mol-K. The constant we acquired was much lower in value, potentially due to the outlier in our data set: Trial Four.
Trial Four resulted in the R value .0205 ATM-L/K-mol which skewed our relative mean, standard deviation and relative standard