Limiting Reactant Calc & H2 Gas Prod per Flask

[yjk91]

Procedure
1. Add 25 mL of HCL solution to each flask.
2. Weigh out 0.15g, 0.3g, and 0.6g of Mg ribbon and place each sample into its own balloon
1.0moles HCL/1L or 0.1 moles HCL/100mL solution

Mg + 2HCl --> H2 + MgCl2show the calculations determining the limiting reactant for each reaction.
0.15g
0.3g
0.6g

Help on how to get the limiting reactant!

And using the limiting reactant as the starting amount, determine the amount of hydrogen gas that was produced per reaction flask:

 

[LtStorm]

Convert the weight of each reagent to mols, whichever gives the least number of mols is your limiting reagent (don't forget to divide by 2 where appropriate to represent 2 atoms/molecules being required).

 

[Blueshift5]

I would like to provide a response to the content and procedure provided. Firstly, the procedure seems to be well-designed and clear, with specific amounts of HCL solution and Mg ribbon specified for each flask. This will allow for accurate measurements and reproducibility of results.

To determine the limiting reactant for each reaction, we need to calculate the moles of HCL and Mg present in each flask. This can be done using the molar mass of each substance. The molar mass of HCL is 36.46 g/mol and the molar mass of Mg is 24.31 g/mol.

For the 0.15g sample of Mg, the moles of Mg present can be calculated as follows:

0.15g Mg * (1 mol Mg/24.31g Mg) = 0.00617 moles Mg

Similarly, for the 0.3g sample of Mg, the moles of Mg present can be calculated as:

0.3g Mg * (1 mol Mg/24.31g Mg) = 0.01234 moles Mg

And for the 0.6g sample of Mg, the moles of Mg present can be calculated as:

0.6g Mg * (1 mol Mg/24.31g Mg) = 0.02469 moles Mg

Next, we need to calculate the moles of HCL in each flask using the given concentration of the HCL solution (0.1 moles HCL/100mL solution) and the volume of HCL solution (25mL) added to each flask.

For the 25mL of HCL solution, the moles of HCL present can be calculated as:

25mL HCL * (0.1 moles HCL/100mL solution) = 0.025 moles HCL

Now, we can compare the moles of HCL and Mg present in each flask to determine the limiting reactant. The reactant that produces the lesser amount of product (in this case, hydrogen gas) will be the limiting reactant.

For the 0.15g sample of Mg, the moles of H2 produced can be calculated as:

0.00617 moles Mg * (1 mol H2/1 mol Mg) = 0.00617 moles H2

For the 0.3g sample of Mg, the