Assume that 29.7 g of Al react with HCl
according to the equation
Al(s) + HCl(aq) −→ AlCl3(aq) + H2(g)
at STP. How many moles of Al react? Remember to balance the equation first.
Answer in units of mol.
How many moles of H2 are produced?
Answer in units of mol.
How much H2 at STP is produced?
Answer in units of L.
After working those other problems, what about this do you not understand. Explain in detail. And while you're at it, balanced the equation.
My balanced eq is
2Al + 6HCl - 2AlCl3 +3H2
so moles of H2 at STP will be 3x22.4 right?
I don't think so. mols Al = grams/atomic mass = ?
To answer these questions, we need to follow a few steps:
1. Balance the equation:
The given equation is:
Al(s) + HCl(aq) -> AlCl3(aq) + H2(g)
To balance it, we count the number of atoms of each element on both sides of the equation and adjust the coefficients until they are equal. In this case, we need two moles of HCl to react with one mole of Al, so the balanced equation is:
2Al(s) + 6HCl(aq) -> 2AlCl3(aq) + 3H2(g)
2. Convert grams of Al to moles:
We are given that 29.7 g of Al react. To find the number of moles, we can use the molar mass of Al which is approximately 26.98 g/mol. We divide the mass of Al by its molar mass to get the number of moles:
moles of Al = 29.7 g / 26.98 g/mol = 1.100 mol (rounded to three decimal places)
So, 1.100 moles of Al react.
3. Determine the moles of H2 produced:
According to the balanced equation, for every 2 moles of Al that react, 3 moles of H2 are produced. Since we have 1.100 moles of Al, we can use the ratio to calculate the moles of H2:
moles of H2 = (1.100 mol Al) * (3 mol H2 / 2 mol Al) = 1.650 mol (rounded to three decimal places)
Therefore, 1.650 moles of H2 are produced.
4. Calculate the volume of H2 at STP:
STP (Standard Temperature and Pressure) is defined as 0 degrees Celsius (273.15 K) and 1 atmosphere of pressure (1 atm). At STP, one mole of any ideal gas occupies 22.4 liters.
Since we have 1.650 moles of H2, we can calculate the volume of H2 gas produced at STP:
Volume of H2 = (1.650 mol) * (22.4 L/mol) = 36.96 L (rounded to two decimal places)
So, 36.96 liters of H2 gas are produced at STP.