Calculate the volume of gas that will be released when aluminum weighing 2.7 g
Calculate the volume of gas that will be released when aluminum weighing 2.7 g interacts with a 40% potassium hydroxide solution weighing 50 g.
1. Let’s compose the equation of a chemical reaction.
2Al + 2KOH + 6H2O = 2K [Al (OH) 4] + 3H2.
2. Find the amount of aluminum and potassium hydroxide.
n (Al) = m (Al) / M (Al) = 2.7 g / 27 g / mol = 0.1 mol.
m (KOH) = m (solution) * ω (KOH) / 100% = 50 g * 40% / 100% = 20 g.
n (KOH) = m (KOH) / M (KOH) = 20 g / 56 g / mol = 0.357 mol.
Aluminum is in short supply, therefore we will decide based on its quantity.
3. Using the reaction equation, we find the amount and then the volume of hydrogen.
n (H2) = n (Al) * 1.5 = 0.1 mol * 1.5 = 0.15 mol.
V (H2) = n (H2) * Vm = 0.15 mol * 22.4 L / mol = 3.36 L.
Answer: V (H2) = 3.36 liters.