Question

1.00 g of magnesium ribbon reacted with 25.0 cm3 of 1.00 mol dm–3 hydrochloric acid. Determine the volume, in cm3, of a balloon filled with the hydrogen gas produced at SATP (25°C and 100 kPa).Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

Answer 1

To determine the volume of hydrogen gas produced at SATP, we need to calculate the moles of magnesium reacted and use stoichiometry and the ideal gas law.

Step-by-step explanation:

In this reaction, 1.00 g of magnesium reacts with 25.0 cm3 of 1.00 mol dm–3 hydrochloric acid to produce hydrogen gas. To find the volume of hydrogen gas produced at SATP (25°C and 100 kPa), we need to use the ideal gas law.

We can start by calculating the moles of magnesium reacted using its molar mass, then use stoichiometry to find the moles of hydrogen gas produced. Finally, we can use the ideal gas law, PV = nRT, where P = 100 kPa, V is the volume in liters, n is the moles of hydrogen gas, R is the ideal gas constant, and T = 25°C (which needs to be converted to Kelvin).

Using these calculations, the volume of the balloon filled with the hydrogen gas produced can be determined.