How many grams of zinc metal are required to produce 2.00 L of hydrogen gas at STP
according to the chemical equation shown below?
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
The answer is 5.83g
22.4 Mol/L at STP means 44.8 moles of H2
Each mole of Zn produces one mole of H2, so you need 44.8 moles of Zn.
How many grams is that?
Do you mean 44.8L of Zn?
when I do m=M*n
I get a really high Number which I don't think is right.
It isn't. That's 22.4 L/mol and not 22.4 mols/L. So you want 2/22.4 = ? mols H2 produced.
1 mol of any gas occupies 22.4L of space at STP.
2L of H2 spread in 22.4L of space =2/22= .089molH2
According to the equation, 1 mol H2 is produced from 1 mol of Zn. .089molH2 * 65.38gZn = 5.8gZn
To determine the number of grams of zinc metal required to produce 2.00 L of hydrogen gas at STP, we need to use the balanced chemical equation given.
The balanced equation is:
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
From the equation, we can see that one mole of zinc reacts to produce one mole of hydrogen gas.
Now, we need to determine the number of moles of hydrogen gas that will be produced when 2.00 L is formed at STP.
We can use the ideal gas law to calculate the number of moles:
PV = nRT
Where:
P = pressure (STP is 1 atm)
V = volume (2.00 L)
n = number of moles (to be determined)
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (STP is 273 K)
Rearranging the equation to solve for n, we get:
n = PV / RT
Substituting the values into the equation:
n = (1 atm)(2.00 L) / (0.0821 L·atm/mol·K)(273 K)
Calculating the right-hand side of the equation:
n ≈ 0.0877 moles
From the balanced equation, we know that for every 1 mole of hydrogen gas produced, we need 1 mole of zinc.
Therefore, the number of moles of zinc required will be the same as the number of moles of hydrogen gas, which is approximately 0.0877 moles.
Now, we need to calculate the mass of zinc in grams.
To do this, we need to use the molar mass of zinc, which is found on the periodic table. The molar mass of zinc is approximately 65.38 g/mol.
Finally, we can calculate the mass of zinc:
Mass = Moles × Molar Mass
Mass = 0.0877 moles × 65.38 g/mol
Calculating the right-hand side of the equation:
Mass ≈ 5.73 grams
Therefore, approximately 5.73 grams of zinc metal are required to produce 2.00 L of hydrogen gas at STP according to the given chemical equation.