1.70 L of 0.550 M H2O2 reacts according to the following reaction.

2H2O2(aq) -> 2H2O(l) + O2(g)
How much H2O is formed? (molar mass of H = 1.00 g/mol O = 16.0 g/mol)

Well, let's get right into it! The balanced equation tells us that for every 2 moles of H2O2, we get 2 moles of H2O.

To find the amount of H2O formed, we need to use stoichiometry. First, let's calculate the number of moles of H2O2 we have:

1.70 L * 0.550 mol/L = 0.935 mol H2O2

Since the ratio of H2O2 to H2O in the balanced equation is 2:2, for every 2 moles of H2O2, we get 2 moles of H2O. Therefore, the amount of H2O formed is also 0.935 mol.

To convert moles into grams, we'll multiply by the molar mass of H2O:

0.935 mol * (2 mol H2O / 2 mol H2O2) * (18.0 g H2O / 1 mol H2O) = 16.83 g

So, approximately 16.83 grams of H2O is formed. Now that's a refreshing result!

To determine the amount of H2O formed, we first need to calculate the number of moles of H2O2 present in the solution.

The molarity (M) of H2O2 is given as 0.550 M, which means that there are 0.550 moles of H2O2 in 1 liter of solution.

Given that the volume of the solution is 1.70 L, we can calculate the number of moles of H2O2 as follows:

moles of H2O2 = molarity of H2O2 * volume of solution
moles of H2O2 = 0.550 M * 1.70 L
moles of H2O2 = 0.935 moles

From the balanced equation, we can see that for every 2 moles of H2O2, 2 moles of H2O are formed.

Therefore, using stoichiometry, we can calculate the number of moles of H2O formed:

moles of H2O = (moles of H2O2 / 2) * 2
moles of H2O = (0.935 moles / 2) * 2
moles of H2O = 0.935 moles

Finally, we can convert the moles of H2O to grams using the molar mass of H2O:

mass of H2O = moles of H2O * molar mass of H2O
mass of H2O = 0.935 moles * (2 * 1.00 g/mol + 16.0 g/mol)
mass of H2O = 0.935 moles * 18.0 g/mol
mass of H2O = 16.23 grams

Therefore, approximately 16.23 grams of H2O is formed.

To determine the amount of H2O formed in the given reaction, we need to consider the stoichiometry of the reaction.

According to the balanced equation:
2 moles of H2O2 produces 2 moles of H2O

We are given the volume and concentration of H2O2. To find the number of moles of H2O2, we can use the formula:

moles = volume (in liters) × concentration

Given:
Volume of H2O2 = 1.70 L
Concentration of H2O2 = 0.550 M

Using the formula:
moles of H2O2 = 1.70 L × 0.550 M = 0.935 mol H2O2

Since the reaction is balanced on a 1:1 ratio between H2O2 and H2O, we can conclude that the moles of H2O formed will be equal to the moles of H2O2.

Therefore, the moles of H2O formed = 0.935 mol.

To find the mass of H2O formed, we can use its molar mass.

Given:
Molar mass of H = 1.00 g/mol
Molar mass of O = 16.0 g/mol

The molar mass of H2O can be calculated as:
2(1.00 g/mol) + 16.0 g/mol = 18.0 g/mol

To find the mass of H2O formed, we can apply the formula:

mass = moles × molar mass

mass of H2O formed = 0.935 mol × 18.0 g/mol ≈ 16.83 g

Therefore, approximately 16.83 grams of H2O would be formed in the reaction.

mols H2O2 = M x L = ?

Convert mols H2O2 to mols H2O with the coefficients in the balanced equation.
Convert mols H2O to g. g = mols x molar mass.