If the reaction
2H2O2 →2H2O+O2
has a 45% yield, what is the molarity of the H2O2 solution if 2.5 L of this solution pro- duces 150 g of O2?
Well, if the reaction only has a 45% yield, it means that 55% of the H2O2 is not turning into H2O and O2, and is probably off somewhere enjoying a vacation.
Now, to find the molarity of the H2O2 solution, we need to calculate the number of moles of O2 produced. Given that 150 g of O2 is produced, we can use the molar mass of O2 (32 g/mol) to calculate the number of moles:
150 g O2 * (1 mol O2 / 32 g O2) = 4.6875 mol O2
Since the reaction has a stoichiometry of 2:2 (2 moles of H2O2 produce 2 moles of O2), it means that 4.6875 mol of O2 are produced from 4.6875 mol of H2O2.
Now, we know that there are 2.5 L of the H2O2 solution. To find the molarity, we divide the number of moles by the volume in liters:
4.6875 mol H2O2 / 2.5 L = 1.875 M
So, the molarity of the H2O2 solution is approximately 1.875 M. But remember, 55% of the H2O2 is on vacation, so make sure to throw in some extra jokes to get their attention when you need them!
To find the molarity of the H2O2 solution, we need to know the number of moles of H2O2 and the volume of the solution.
First, let's calculate the number of moles of O2 produced in the reaction.
Given:
Mass of O2 produced = 150 g
The molar mass of O2 = 32 g/mol (as oxygen has an atomic mass of 16 g/mol, and O2 consists of two atoms of oxygen)
Number of moles of O2 = Mass of O2 produced / Molar mass of O2
= 150 g / 32 g/mol
= 4.6875 mol
Since the stoichiometry of the reaction is 2H2O2 → 2H2O + O2, the number of moles of H2O2 would be half the number of moles of O2 produced.
Number of moles of H2O2 = 0.5 * the number of moles of O2
= 0.5 * 4.6875 mol
= 2.3438 mol
Now we need to calculate the volume of the solution.
Given:
Yield = 45%
Volume of the solution = 2.5 L
The yield is the percentage of the actual amount of H2O2 obtained compared to the theoretical amount.
Actual amount of H2O2 = Yield * theoretical amount of H2O2
= 0.45 * 2.3438 mol
= 1.0542 mol
Now we can find the molarity of the H2O2 solution.
Molarity = Number of moles of solute / Volume of solution in liters
= 1.0542 mol / 2.5 L
= 0.4217 M
Therefore, the molarity of the H2O2 solution is approximately 0.4217 M.
well, it would have produced 150/.45 g of O2, which is
moleO2= 150/.45*32
which means twice those moles were used in the peroxide, or
2*150/(.45*32)=2.5*Molarity
solve for molarity
To find the molarity of the H2O2 solution, we need to determine the number of moles of H2O2 and the volume of the solution.
First, we need to find the number of moles of O2 produced. We can use the given mass of O2 (150 g) and its molar mass (32.00 g/mol) to calculate the number of moles using the formula:
moles of O2 = mass of O2 / molar mass of O2
moles of O2 = 150 g / 32.00 g/mol = 4.69 mol
Since the balanced chemical equation shows that 2 moles of H2O2 produce 1 mole of O2, we can determine the number of moles of H2O2:
moles of H2O2 = (moles of O2) / (2 moles of O2 / 2 moles of H2O2)
moles of H2O2 = 4.69 mol / (2 / 2) = 4.69 mol
Next, we need to find the volume of the H2O2 solution. The volume given is 2.5 L.
Now we can calculate the molarity (M):
Molarity (M) = moles of solute / volume of solution (in L)
Molarity = 4.69 mol / 2.5 L = 1.88 M
Therefore, the molarity of the H2O2 solution is 1.88 M.