The following reaction represents the decomposition of hydrogen peroxide
2H2O2 -> o2 (g) + 2H2O (l)
How many molecules of water are produced from the decomposition of 3.4g of Hydrogen peroxide, H2O2?
Please walk me through this one, I need more then just the answer, I need to understand how the work was done. I'm very lost at the moment with this question. Thanks in advance for your help.
Two important things about chemistry.
1. ALWAYS write an equation and balance it.
2. Chemistry works with moles. Therefore, change g to moles first thing you do.
You have the equation. Now change the 3.4 g H2 to moles. moles = grams/molar mass
3.4 g/2.016 = 1.686 moles.
Now using the coefficients in the balanced equation, convert moles H2O2 to moles H2O.
1.686 moles H2 x (2 moles H2O/2 moles H2O2) = 1.686 x (2/2) = 1.686 x (1/1) = 1.686 moles H2O.
Now you know that 1 mole of water is composed of 6.022 x 10^23 molecules. So
1.686 moles H2O x (6.022 x 10^23 molecules H2O/1 mole H2O) = ?? molecules.
Here is a sample stoichiometry problem I've posted. Feel free to use it as needed.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine how many molecules of water are produced from the decomposition of 3.4g of hydrogen peroxide (H2O2), we need to follow these steps:
1. Start with the given mass of hydrogen peroxide (H2O2) and convert it to moles using the molar mass.
2. Use the balanced chemical equation to determine the stoichiometric ratio between hydrogen peroxide (H2O2) and water (H2O).
3. Convert the moles of water (H2O) to molecules using Avogadro's number.
Let's calculate the number of molecules of water produced step-by-step:
Step 1: Calculate the number of moles of hydrogen peroxide (H2O2)
The molar mass of hydrogen peroxide (H2O2) is:
2(1.01 g/mol) + 2(16.00 g/mol) = 34.02 g/mol
To calculate the number of moles, use the formula:
moles = mass / molar mass
moles = 3.4 g / 34.02 g/mol = 0.1 mol
Step 2: Use the balanced chemical equation to determine the stoichiometric ratio.
From the balanced equation:
2H2O2 -> O2(g) + 2H2O(l)
For every 2 moles of hydrogen peroxide, 2 moles of water are produced.
Step 3: Convert moles of water to molecules.
We know that 1 mole of any substance contains Avogadro's number of molecules, which is approximately 6.022 × 10^23 molecules.
So, the number of molecules of water produced is:
0.1 mol H2O x (6.022 × 10^23 molecules/mol) = 6.02 × 10^22 molecules of H2O
Therefore, 3.4 grams of hydrogen peroxide will produce approximately 6.02 × 10^22 molecules of water.
To determine the number of water molecules produced from the decomposition of 3.4g of hydrogen peroxide (H2O2), we need to follow a series of steps:
Step 1: Calculate the molar mass of hydrogen peroxide (H2O2).
The molar mass of hydrogen (H) is 1g/mol, and oxygen (O) is 16g/mol. Since there are two hydrogens and two oxygens in hydrogen peroxide, the molar mass of H2O2 is:
Molar mass of H2O2 = (2 * 1g/mol) + (2 * 16g/mol)
= 2g/mol + 32g/mol
= 34g/mol
Step 2: Calculate the number of moles of hydrogen peroxide using its molar mass and its given mass.
We can use the formula:
Number of moles = mass (in grams) / molar mass
Number of moles of H2O2 = 3.4g / 34g/mol
= 0.1 mol
Step 3: Use the balanced chemical equation to determine the mole ratio of water to hydrogen peroxide.
From the balanced equation:
2H2O2 -> O2(g) + 2H2O(l)
The coefficients in front of the reactants and products indicate the ratio of the moles involved in the reaction. In this case, the ratio of water to hydrogen peroxide is 2:2, which simplifies to 1:1.
Step 4: Calculate the number of moles of water produced.
Since the mole ratio of water to hydrogen peroxide is 1:1, the number of moles of water produced will be equal to the number of moles of hydrogen peroxide.
Number of moles of water = 0.1 mol
Step 5: Convert the number of moles of water to the number of water molecules.
We can use Avogadro's number, which states that one mole of any substance contains 6.022 x 10^23 particles (atoms, molecules, or ions).
Number of water molecules = Number of moles of water * Avogadro's number
= 0.1 mol * 6.022 x 10^23 molecules/mol
= 6.022 x 10^22 water molecules
Therefore, the decomposition of 3.4g of hydrogen peroxide will produce approximately 6.022 x 10^22 water molecules.