In the balanced redox reaction 2 al(s) + 6 hcl(aq) → 2 alcl3(aq) + 3 h2(g) 80.0 ml of 2.0 m hcl would (theoretically) react with how many grams of al(s)? assume that the reaction is quantitative.
a. 1.44 g
b. 4.32 g
c. 1,440 g
d. 2,030 g
e. none of the above

The chemical reaction is written as:

 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g)

We use the volume and the concentration of the acid to determine the number of moles HCl used. Then, we use relation from the reaction to determine the moles Al used. Finally, we convert it to grams by the molar mass.

(2.0 mol HCl / L) (.080 L) ( 2 mol Al / 6 mol HCl ) ( 26.98 g / mol ) = 1.44 g Al is used.

The answer is accuracy