Alaboratory experiment requires 4.8 l of a 2.5 m solution of sulfuric acid (h2so4), but the only available h2so4 is a 6.0 m stock solution. how could you prepare the solution needed for the lab experiment? show all the work used to find your answer.

Take 2.0 L of the H2SO4 stock solution of 6.0 M and dilute it to 4.8 L

Explanation:

For The exercise we are going to need the next equation:

(Final concentration)(final volume) = (initial concentration)(initial volume) or CfVf=CiVi

The final solution is the one required to the experiment, the one with a concentration of 2.5 M and a volume of 4.8 L, and the initial solution is the one available of concentration 6.0 M. So, we need to know the volume of the initial solution we need to take to prepare the require solution. For the equation above we have:

Replacing the values:

Then, to prepare the solution needed for the experiment we must take 2.0 L of the H2SO4 stock solution of 6.0 M and dilute it to 4.8 L of solution, that is to say, add 2.8 L of water, so to get a 2.5 M H2SO4 solution.

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.