Question: 1 theoretical yield of hydrogen gas for each trial use...
1. Theoretical Yield of Hydrogen Gas. For each trial, use the molar masses of magnesium and hydrogen, and the balanced equation for the reaction you have just observed, to calculate the theoretical mass of hydrogen that could be formed, assuming that the magnesium was pure and was completely consumed by the hydrochloric acid.
2. Actual Yield of Hydrogen Gas. Using your pressure (PH2), temperature, and measured volume data, for each trial, calculate the mass of hydrogen gas formed in the reaction.
3. Determine the % yield of hydrogen gas for each trial.
4. If an undetected bubble of air were trapped inside the graduated cylinder, what would be its effect on the percent yield in your experiment? Would the percent yield be erroneously high, erroneously low, or be unaffected by the bubble of air? Explain with a maximum of 3 sentences.
5. If you hadn’t added quite enough hydrochloric acid to consume all of the magnesium metal, what would bethe effect of this error on the percent yield in your experiment? Would the percent yield be erroneously high, erroneously low, or be unaffected by not adding enough HCl? Explain with a maximum of 3 sentences.
6. In a well-executed experiment like the one you performed, the value of the ideal gas constant can be determined. Use your data (measured volume H2, temperature, PH2, and mol H2) to determine the value of the ideal gas constant, R, in L·kPa/ mol·K for each trial. Then, determine the % error for each trial.