# Question 51377

Apr 27, 2017

This will require 2.067 litres of the acid solution.

#### Explanation:

In the equation, we see that 3 moles of ${H}_{2}$ are produced when 3 moles of ${H}_{2} S {O}_{4}$ are reacted. (This is seen from the coefficients placed before these formulas.)

To simply the relation, we can say that the ratio between ${H}_{2} S {O}_{4}$ used and ${H}_{2}$ produced is 1-to-1.

Now, we must convert the mass of ${H}_{2}$ into moles:

$25.0 g \div 2.01588 \frac{g}{\text{mol" = 12.40 "mol}}$

Since the ratio is 1-to-1, this means we will require 12.40 mol of ${H}_{2} S {O}_{4}$ to produce this hydrogen gas.

To determine the volume of the solution required, we start with the definition of molarity:

"Molarity" = ("moles of solute")/("litres of solution")

So,

"litres of solution" = ("moles of solute")/("molarity") = (12.4 "mol")/(6.00 "mol"/L) = 2.067 L#