hydrogen gas can be produced by reacting aluminum with sulfuric acid .How many L hydrogen gas are produced by reacting 15.0 mol of sulfuric acid with 15.0 mol of aluminum at STP?

Answer 1

This is a limiting reagent problem. I now that because amounts are given for BOTH reactants. Write a balanced equation.

2Al + 3H2SO4 ==> Al2(SO4)3 + 3H2

Convert mols of each reactant to mols H2.
Al first.
15.0 mols Al x [3 mols H2/2 mols Al) = 15.0 x 3/2 = 22.5 mols H2 gas.
Next H2SO4:
15.0 mols H2SO4 x (3 mols H2/3 mols H2SO4) = 15.0 x 1/1 = 15.0 mol H2 produced.
The two answers are different; therefore, one of them must be incorrect. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that number is the limiting reagent. H2SO4 is the LR.
1 mol gas at STP occupies a volume of 22.4L; therefore, 15.0 mols x 22.4L = ? L H2 gas from this reaction if you have 100% yield.

Answer 2

what would the volume of the gas produced be at a pressure of 700mmHg and a temperature of 30degrees of C

Answer 3

Use PV = nRT
You have n.Substitute the new T and P. Remember T must be in kelvin and P in atmospheres.
P of 700 mm = 700/760 atm