5. How many moles of magnesium were consumed in the reaction? Open the Data window and click on the flask to provide evidence that this answer is correct.

6. Could this experiment be performed in the smaller 50 mL Erlenmeyer flask?

How about letting us in on what you did? My crystal ball isn't working today.

you are in trimms lab class arn't you... I am also taking it you are looking a number... if you look at the equation that you have gotten should have looked something like this

Mg+2HCl---->MgCl2+H2 if you look no Mg was lost nor gained in this equation when you look at the data table it doesn't show a number because Mg was not consumed in this reaction.

Hope this helped

To determine the number of moles of magnesium consumed in the reaction, you'll need some information about the reaction and the amount of magnesium used. The balanced chemical equation for the reaction is needed to establish the stoichiometry of the reaction. Without that information, it is not possible to determine the number of moles of magnesium consumed.

As for the second question, to determine if the experiment can be performed in a smaller 50 mL Erlenmeyer flask, you'll need to consider the reaction conditions and the volume of reactants and products involved in the reaction.

If the reaction conditions remain the same and the reactants and products can fit within the smaller flask while allowing for proper mixing and reaction to occur, then it may be feasible to perform the experiment in the smaller flask. However, if the volume of reactants or products exceeds the capacity of the 50 mL flask, or if the reaction conditions need to be adjusted, then it may not be possible to perform the experiment in the smaller flask.

To make a definitive conclusion, it is important to assess the specific details of the reaction and the experimental setup.