in the equation mg+2hcl-->mgcl2+h2, what mass of the hcl is consumed by the reaction of 2.50 mol of magnesium

You need to learn to use the caps key when you do chemistry because co, Co and CO and not the same.

Mg + 2HCl ==> MgCl2 + H2
How many mols Mg? That's 2.50 mols in the problem.
Using the coefficients in the balanced equation, convert mols Mg to mol HCl. That will be 2.50 x (2 mol HCl/1 mol Mg) = 2.5 x 2/1 = ? mol HCl.
Now convert mols HCl to grams. g = moles x molar mass.

183

To find the mass of HCl consumed in the reaction, we need to use the stoichiometry of the balanced equation. The balanced equation is:

Mg + 2HCl → MgCl2 + H2

From the equation, we can see that 1 mole of magnesium reacts with 2 moles of HCl. The molar ratio between magnesium and HCl is 1:2.

Given that there are 2.50 moles of magnesium, we can use this ratio to determine the moles of HCl consumed:

2.50 mol Mg × (2 mol HCl / 1 mol Mg) = 5.00 mol HCl

Now, we need to convert the moles of HCl to mass. We can do this by using the molar mass of HCl, which is approximately 36.5 g/mol.

5.00 mol HCl × 36.5 g/mol HCl = 182.5 g HCl

Therefore, the mass of HCl consumed by the reaction of 2.50 mol of magnesium is 182.5 grams.