a)What is the mass of heavy water D2O produced when 5.20g of O2 reacts with excess D2?

b)What is the mass of water H2O,produced when 5.20g of O2 reacts with excess H2

Consider the reaction 2D2+O2->2D2O

Can someone step me through this?

Of course! I can help you step-by-step with these problems.

a) To determine the mass of heavy water (D2O) produced when 5.20g of O2 reacts with excess D2, we need to calculate the molar mass of D2O and use stoichiometry.

Step 1: Calculate the molar mass of D2O.
The molar mass of D2O can be calculated by adding the molar masses of two deuterium atoms (D) and one oxygen atom (O).

Molar mass of deuterium (D)= 2.01 g/mol
Molar mass of oxygen (O) = 16.00 g/mol

Molar mass of D2O = (2 x 2.01 g/mol) + (1 x 16.00 g/mol)
= 4.02 g/mol + 16.00 g/mol
= 20.02 g/mol

Step 2: Determine the moles of O2.
Given mass of O2 = 5.20 g
Molar mass of O2 = 32.00 g/mol

Moles of O2 = given mass / molar mass
= 5.20 g / 32.00 g/mol
= 0.1625 mol

Step 3: Apply stoichiometry.
From the balanced equation, we can see that 2 moles of D2O are produced for every 1 mole of O2 consumed.

Moles of D2O = (0.1625 mol O2) x (2 mol D2O / 1 mol O2)
= 0.325 mol D2O

Step 4: Convert moles to grams.
Now we can convert moles of D2O to grams using its molar mass.

Mass of D2O = moles of D2O x molar mass of D2O
= 0.325 mol x 20.02 g/mol
= 6.505 g

Therefore, the mass of heavy water (D2O) produced when 5.20 g of O2 reacts with excess D2 is 6.505 g.

b) To determine the mass of water (H2O) produced when 5.20 g of O2 reacts with excess H2, we can follow similar steps with a different molar mass calculation.

Step 1: Calculate the molar mass of H2O.
The molar mass of H2O can be calculated by adding the molar masses of two hydrogen atoms (H) and one oxygen atom (O).

Molar mass of hydrogen (H) = 1.01 g/mol
Molar mass of oxygen (O) = 16.00 g/mol

Molar mass of H2O = (2 x 1.01 g/mol) + (1 x 16.00 g/mol)
= 2.02 g/mol + 16.00 g/mol
= 18.02 g/mol

Step 2: Determine the moles of O2.
Given mass of O2 = 5.20 g
Molar mass of O2 = 32.00 g/mol

Moles of O2 = given mass / molar mass
= 5.20 g / 32.00 g/mol
= 0.1625 mol

Step 3: Apply stoichiometry.
From the balanced equation, we can see that 2 moles of H2O are produced for every 1 mole of O2 consumed.

Moles of H2O = (0.1625 mol O2) x (2 mol H2O / 1 mol O2)
= 0.325 mol H2O

Step 4: Convert moles to grams.
Now we can convert moles of H2O to grams using its molar mass.

Mass of H2O = moles of H2O x molar mass of H2O
= 0.325 mol x 18.02 g/mol
= 5.8535 g

Therefore, the mass of water (H2O) produced when 5.20 g of O2 reacts with excess H2 is 5.8535 g.

Sure! I can walk you through the steps to find the mass of heavy water (D2O) and water (H2O) produced when 5.20g of O2 reacts with excess D2 and H2 respectively.

a) Mass of heavy water (D2O) produced when 5.20g of O2 reacts with excess D2:
1. Start with the balanced chemical equation: 2D2 + O2 -> 2D2O
2. Determine the molar mass of O2 and D2O.
- The molar mass of O2 is 32 g/mol (16 g/mol for each oxygen atom).
- The molar mass of D2O is 20 g/mol (2 g/mol for each deuterium atom + 16 g/mol for each oxygen atom).
3. Convert the given mass of O2 to moles using the molar mass of O2.
- Moles = Mass / Molar mass = 5.20 g / 32 g/mol = 0.1625 mol
4. Use the stoichiometry of the balanced equation to find moles of D2O.
- According to the equation, 1 mole of O2 reacts with 2 moles of D2O.
- Moles of D2O = 2 × Moles of O2 = 2 × 0.1625 mol = 0.325 mol
5. Finally, calculate the mass of D2O using the moles of D2O and its molar mass.
- Mass of D2O = Moles × Molar mass = 0.325 mol × 20 g/mol = 6.50 g

Therefore, the mass of heavy water (D2O) produced is 6.50 g.

b) Mass of water (H2O) produced when 5.20g of O2 reacts with excess H2:
1. Start with the balanced chemical equation: 2D2 + O2 -> 2D2O
2. Determine the molar mass of O2 and H2O.
- The molar mass of O2 is 32 g/mol.
- The molar mass of H2O is 18 g/mol (2 g/mol for each hydrogen atom + 16 g/mol for each oxygen atom).
3. Follow the same steps as in part (a), replacing the molar mass and stoichiometry values.
- Convert the given mass of O2 to moles.
- Moles of O2 = 5.20 g / 32 g/mol = 0.1625 mol
- Moles of H2O = 2 × Moles of O2 = 2 × 0.1625 mol = 0.325 mol
- Mass of H2O = Moles of H2O × Molar mass of H2O = 0.325 mol × 18 g/mol = 5.85 g

Therefore, the mass of water (H2O) produced is 5.85 g.

Look at it from moles only.

how many moles of O2 is in 5.2grams?
mole=5.2/32 work this precisely.
YOU will get twice this moles of product. What is the mass?
Moles product: 5.2/32 * 2

so what is the mass of the product:
massD2O= 5/32 *2*molmassD2O
massH2O=5/32 * 2 * molmassH2O