Kinetic Molecular Theory Gas Laws - Oakland Schools
Kinetic Molecular Theory Gas Laws - Oakland Schools
Kinetic Molecular Theory Gas Laws - Oakland Schools
You also want an ePaper? Increase the reach of your titles
YUMPU automatically turns print PDFs into web optimized ePapers that Google loves.
Answer Key:<br />
Calculations:<br />
Calculation 1: mass of Mg x (1 mole Mg/molar mass Mg) x (coeff of H2/ coeff of Mg) =<br />
moles of H2<br />
Calculation 2: atmospheric pressure – water vapor pressure = pressure of H2;<br />
If these pressures are in mmHg, convert to atm with the unit equality 1 atm = 760.<br />
mmHg<br />
Calculation 3: Remember the graduated cylinder was inverted! Convert to Liters using<br />
1000 mL = 1 Liter<br />
Calculation 4: if the temperature obtained from the thermometer is in Celsius, convert<br />
to Kelvin using K = degree Celsius + 273<br />
Calculation 5: It is recommended that students first rearrange the variables of the ideal<br />
gas equation to solve for R before plugging in values [R = (PV)/(nT)] Their units<br />
should be (atm x Liters) / (mol x K)<br />
Analysis and Conclusion Questions<br />
Question 1: bubbles appeared near the magnesium, heat was generated, Mg<br />
disappeared<br />
Question 2: copper wire appeared unchanged. It did not take part in the reaction.<br />
Copper does not react w/ HCl b/c Cu is below H on the activity series<br />
Question 3:<br />
Question 4: sources of error include the following: experimental error in the<br />
measurements of the volume, temperature, and pressure of the gas; small sample of<br />
gas generated; escaped pieces of Mg that did no react<br />
Question 5: The value of R would not change. It is dependent on the values of the<br />
pressure, temperature, volume, and number of moles of the gas. Under the same<br />
conditions, these variables would be the same for any gas.<br />
35
Change language