how many grams of oxygen is required to produce 2.0 kg of water??

1. Write and balance the equation.

2H2 + O2 ==> 2H2O

2. Convert what you have (water in this case) to moles. moles = grams/molar mass that's 2000/18.015 = ?? moles.

3. Using the coefficients in the balanced equation, convert moles of what you have (water) to moles of what you want (in this case oxygen).

4. Now convert moles oxygen to grams. g = moles x molar mass.

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To find out how many grams of oxygen are required to produce 2.0 kg of water, we need to apply stoichiometry and use the molar mass of water.

Here's the step-by-step process:

1. Determine the chemical equation for the formation of water. The equation is: 2H₂ + O₂ → 2H₂O. This indicates that for every 1 mole of oxygen (O₂), 2 moles of water (H₂O) are produced.

2. Calculate the molar mass of water (H₂O). The molar mass of hydrogen (H) is approximately 1.008 g/mol, and the molar mass of oxygen (O) is approximately 16.00 g/mol. Thus, the molar mass of water is:
2(1.008 g/mol) + 16.00 g/mol = 18.02 g/mol.

3. Convert the given mass of water to moles. Since the molar mass of water is 18.02 g/mol, we divide the given mass (2.0 kg) by the molar mass to get:
2.0 kg × 1000 g/kg ÷ 18.02 g/mol = 110.54 mol.

4. Apply stoichiometry to find the number of moles of oxygen required. From the balanced equation, we know that for every 2 moles of water produced, 1 mole of oxygen is consumed. Therefore, the number of moles of oxygen can be calculated as:
110.54 mol water × (1 mol O₂ / 2 mol H₂O) = 55.27 mol.

5. Finally, convert the moles of oxygen to grams using its molar mass. The molar mass of oxygen (O₂) is approximately 32.00 g/mol. Thus,
55.27 mol O₂ × 32.00 g/mol = 1768.64 g.

Therefore, approximately 1768.64 grams of oxygen are required to produce 2.0 kg of water.