A student reacts 0.506 grams of aluminum with excess KOH and H2O according to reaction one from the lab manual.
2Al + 2KOH +6H2O ---> 2K[Al(OH)4]+3H2
Enter your answers in numerical format.
How many moles of aluminum was reacted?
How many moles of K[Al(OH)4] will theoretically be produced?
molar mass of Al is 27 g/mol
we used .506 g/27 g/mol
= .0187 mols of Al
for every mol of Al we get a mol of K[Al(OH)4]
so .0187
To find the number of moles of aluminum reacted, we need to use the given mass of aluminum and convert it to moles using the molar mass.
1. Determine the molar mass of aluminum (Al). The atomic mass of aluminum is 26.98 g/mol.
2. Convert the given mass of aluminum (0.506 grams) to moles using the following equation:
Number of moles = Given mass / Molar mass
Number of moles = 0.506 g / 26.98 g/mol
Calculate the above equation to find the number of moles of aluminum.
To find the number of moles of K[Al(OH)4] theoretically produced, we need to use the stoichiometry of the reaction, which indicates the mole ratio between aluminum and K[Al(OH)4].
From the balanced equation: 2Al + 2KOH + 6H2O ---> 2K[Al(OH)4] + 3H2
We can see that for every 2 moles of aluminum reacted, 2 moles of K[Al(OH)4] will be produced.
3. Use this mole ratio to find the moles of K[Al(OH)4]. Since we know the moles of aluminum reacted from the previous step:
Number of moles of K[Al(OH)4] = (Number of moles of aluminum) * (Mole ratio between aluminum and K[Al(OH)4])
Calculate the above equation to find the number of moles of K[Al(OH)4].
Now you can perform the necessary calculations to find the answers to the questions: the number of moles of aluminum reacted and the number of moles of K[Al(OH)4] that will theoretically be produced.