Question

How many liters of H2 would be formed at 540 mm Hg and 17°C if 24.5 g of zinc was allowed to react?

(a) 0.22 L
(b) 1.11 L
(c) 2.58 L
(d) 5.43 L

Answer 1

To find the volume of H2 gas produced from the reaction of zinc with hydrochloric acid, we use the ideal gas law equation PV = nRT. We need to find the number of moles of zinc, then calculate the number of moles of hydrogen gas using the stoichiometry of the balanced equation. Finally, we can solve for the volume of hydrogen gas by plugging the values into the ideal gas law equation. The correct answer is 5.43 L.

Step-by-step explanation:

This is a stoichiometry problem involving the reaction of zinc with hydrochloric acid to produce hydrogen gas. The balanced chemical equation is:

Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)

To determine the volume of hydrogen gas produced, we need to use the ideal gas law, PV = nRT. First, we need to find the number of moles of zinc (Zn) using its molar mass. Then, we can calculate the number of moles of hydrogen gas (H2) using the stoichiometry of the balanced equation. Finally, we can plug these values into the ideal gas law equation to find the volume of hydrogen gas.

Converting the given temperature from Celsius to Kelvin, and the pressure from mm Hg to atm, we can solve for the volume of hydrogen gas using the ideal gas law equation.

The correct answer is (d) 5.43 L.