If 26.5 mL of 0.222 M HCl reacts with excess Mg, how many mL of hydrogen gas are produced at STP?
Well, if you're trying to give me a "stoichiometric" time, I'd say you're on the "right mole-ment"! Let's clown around with the numbers a bit, shall we?
First, we need to determine the number of moles of HCl that reacted. We can get that by using the formula: moles = concentration × volume.
So, moles of HCl = 0.222 M × 26.5 mL.
But wait, you may need to convert milliliters to liters first. Grab your clown noses, folks, because unit conversions are about to get wacky!
26.5 mL is equal to 0.0265 L. So, moles of HCl = 0.222 M × 0.0265 L.
Now, let's put on our stoichiometric shoes (clown shoes, obviously) and use the balanced equation to figure out the ratio of HCl to H2.
The balanced equation is: 2 HCl + Mg -> MgCl2 + H2.
From this equation, we can see that for every 2 moles of HCl, we get 1 mole of H2. So, the moles of H2 produced are half the moles of HCl used.
Therefore, moles of H2 = (0.222 M × 0.0265 L) / 2.
Now, let's convert back to milliliters, because we're all about that clown life!
1 mole of any gas occupies 22.4 L at STP. Since we have moles of H2, we can calculate the volume in liters and convert it back to milliliters.
Volume of H2 = (moles of H2) × (22.4 L/mol).
But wait! We want mL, so convert it again: Volume of H2 = (moles of H2) × (22.4 L/mol) × (1000 mL/L).
Now that you know the calculations to follow, I hope you can find some clown-plicated fun along the way!
To find the volume of hydrogen gas produced at STP, we need to use stoichiometry.
1. Write the balanced chemical equation for the reaction between HCl and Mg:
2 HCl + Mg -> MgCl2 + H2
2. Calculate the number of moles of HCl:
moles of HCl = concentration of HCl (M) * volume of HCl (L)
moles of HCl = 0.222 M * 0.0265 L
3. Use stoichiometry to determine the number of moles of hydrogen gas produced:
1 mole of HCl produces 1 mole of H2 gas
moles of H2 gas = moles of HCl
4. Convert the moles of hydrogen gas to volume at STP using the ideal gas law:
volume of hydrogen gas (L) = moles of H2 gas * 22.4 L/mol
5. Convert the volume of hydrogen gas to milliliters:
volume of hydrogen gas (mL) = volume of hydrogen gas (L) * 1000 mL/L
Now, let's calculate the volume of hydrogen gas produced at STP step-by-step:
moles of HCl = 0.222 M * 0.0265 L = 0.00587 mol
moles of H2 gas = 0.00587 mol
volume of hydrogen gas (L) = 0.00587 mol * 22.4 L/mol = 0.131568 L
volume of hydrogen gas (mL) = 0.131568 L * 1000 mL/L = 131.568 mL
Therefore, approximately 131.568 mL of hydrogen gas are produced at STP.
To determine the volume of hydrogen gas produced at STP, we need to use the stoichiometry of the balanced chemical equation between HCl and Mg. The balanced equation is:
2 HCl + Mg -> MgCl2 + H2
From the equation, we see that 2 moles of HCl react to produce 1 mole of H2. Therefore, we need to convert the given volume of HCl to moles and then convert moles of H2 to volume at STP.
First, let's calculate the number of moles of HCl using the given volume of 26.5 mL and the molarity of 0.222 M:
Number of moles = Volume (in liters) * Molarity
= 26.5 mL * (1 L / 1000 mL) * 0.222 M
= 0.005883 mol
Next, using the stoichiometry of the balanced equation, we know that 2 moles of HCl produce 1 mole of H2. Therefore, the number of moles of H2 produced will be half the number of moles of HCl:
Number of moles of H2 = 0.005883 mol * (1/2)
= 0.002942 mol
Now, we can use the ideal gas law to calculate the volume of H2 at STP. The ideal gas law equation is:
PV = nRT
Where:
P = pressure (STP is 1 atm)
V = volume
n = number of moles
R = ideal gas constant (0.0821 L * atm / (mol * K))
T = temperature in Kelvin (STP is 273.15 K)
Rearranging the equation, we get:
V = (nRT) / P
Substituting the values into the equation, we have:
V = (0.002942 mol * 0.0821 L * atm / (mol * K) * 273.15 K) / 1 atm
= 0.0677 L
= 67.7 mL (rounded to one decimal place)
Therefore, approximately 67.7 mL of hydrogen gas is produced at STP when 26.5 mL of 0.222 M HCl reacts with excess Mg.
Mg + 2HCl ==> MgCl2 + H2
mols HCl = M x L = ?
Convert mols HCl to mols H2. That will be mols H2 = 1/2 mols HCl.
Then convert mols H2 to L at STP knowing that 1 mol H2 will occupy 22.4 L at STP, then convert that to mL.