Calculate the amount in moles and the mass in grams of KOH needed to convert 1.50 g of aluminum to KAl(OH)4. Balanced equation = 2 Al (s) + 2 KOH (aq) + 6 H2O (l) �¨ 2 KAl(OH)4 (aq) + 3 H2 (g)
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To solve this problem, we need to use stoichiometry. Stoichiometry is a branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. In this case, we are given the mass of aluminum (Al) and want to find the amount in moles and mass in grams of potassium hydroxide (KOH) needed to convert it to KAl(OH)4.
Let's break down the steps to solve the problem:
1. Determine the molar mass of KOH:
The molar mass of potassium (K) is 39.10 g/mol, oxygen (O) is 16.00 g/mol, and hydrogen (H) is 1.01 g/mol. Add up the molar masses of the individual elements to find the molar mass of KOH:
KOH = 39.10 g/mol (K) + 16.00 g/mol (O) + 1.01 g/mol (H) = 56.11 g/mol
2. Calculate the amount in moles of aluminum (Al):
We are given the mass of aluminum, which is 1.50 g. To find the amount in moles, divide the mass by the molar mass of aluminum.
Amount (moles) = Mass (g) / Molar mass (g/mol)
Amount (moles) = 1.50 g / 26.98 g/mol (molar mass of Al) = 0.056 moles
3. Use the balanced equation to determine the stoichiometric ratio between KOH and Al:
The balanced equation indicates that it takes 2 moles of KOH to convert 2 moles of Al to KAl(OH)4.
4. Calculate the amount in moles of KOH:
Since the stoichiometric ratio between KOH and Al is 2:2 (according to the balanced equation), the amount in moles of KOH will be the same as the amount in moles of Al. Therefore, the amount in moles of KOH is also 0.056 moles.
5. Calculate the mass in grams of KOH:
To find the mass in grams of KOH, multiply the amount in moles of KOH by the molar mass of KOH.
Mass (g) = Amount (moles) * Molar mass (g/mol)
Mass (g) = 0.056 moles * 56.11 g/mol (molar mass of KOH) = 3.139 g
Therefore, to convert 1.50 g of aluminum to KAl(OH)4, you would need 0.056 moles of KOH, which is equivalent to 3.139 grams.