Question

when 1.00g of magnesium is reacted with excess hydrochloric acid, what volume of hydrogen gas will be produced at standard temperature and pressure? statndard temperature and pressure is defined as 0 C and 1 atm. At STP, 1 mole of gas occupies 22.4L.

Answer 1

0.93L

Step-by-step explanation:

Hello,

To solve this question, we need to first of all write down the equation of reaction.

Equation of reaction,

2Mg + 4HCl → 2MgCl₂ + 2H₂

From the equation of reaction, it shows that 2 moles of Mg produces 2 moles of H₂.

Number of moles = mass / molar mass

Mass = number of moles × molar mass

Molar mass of Mg = 24g/mol

Mass = 2 × 24 = 48g

Therefore, 48g of Mg produces (2 × 22.4)L of H₂

48g of Mg = 44.8L of H₂

1g of Mg = xL of H₂

x = (1 × 44.8) / 48

x = 0.93L

1g of Mg will produce 0.93L of H₂