Question

What volume of hydrogen is formed when 3.00 g of

magnesium react with an excess of dilute sulfuric acid is
carried out under room temperature and pressure at 1 atm.

Answer 1

Volume of hydrogen gas formed = 3.1 L

Step-by-step explanation:

Given data:

Mass of magnesium = 3.00 g

Temperature = room = 27°C (27+273 = 300 K)

Pressure = 1 atm

Volume of hydrogen gas formed = ?

Solution:

Chemical equation:

Mg + H₂SO₄ → MgSO₄ + H₂

Number of moles of Mg:

Number of moles = mass/molar mass

Number of moles = 3.00 g/ 24 g/mol

Number of moles = 0.125 mol

Now we will compare the moles Mg with hydrogen.

Mg : H₂

1 : 1

0.125 : 0.125

Volume of hydrogen:

PV = nRT

1 atm × V = 0.125 mol × 0.0821 atm.L /K.mol × 300 k

V = 3.1atm.L/1 atm

V = 3.1 L