equation: 4NH3(g) + 5O2(g) -> 4NO(g) + 6H2O(g)

What mass of O2 is needed to produce 0.563g of NO? I think the answer is 750g but how do I get that answer?

A stoichiometry problem. Here is a solve example. Just follow the steps.

http://www.jiskha.com/science/chemistry/stoichiometry.html

It certainly won't take more than 1000 times as much O2 to make that much NO. Did you omit a decimal point somewhere?

Five moles of O2, with a mass of 160 g, are all that is required to make 4 moles of NO, with a mass of 112 g.

Try applying the 160/112 ratio to the amount of NO you want to produce.

To find the mass of O2 needed to produce 0.563g of NO, we can use the stoichiometry of the balanced equation.

Given:
1 mole of NO has a mass of 30 g.

Step 1: Calculate the moles of NO produced.
Moles of NO = mass of NO / molar mass
Moles of NO = 0.563g / 30 g/mol
Moles of NO = 0.01876 mol

Step 2: Use the stoichiometry of the balanced equation to determine the moles of O2 required.
From the balanced equation:
4 moles of NH3 + 5 moles of O2 -> 4 moles of NO + 6 moles of H2O

From the stoichiometry:
5 moles of O2 are required to produce 4 moles of NO.

Moles of O2 required = (Moles of NO) x (5 moles of O2 / 4 moles of NO)
Moles of O2 required = 0.01876 mol x (5/4)
Moles of O2 required = 0.02345 mol

Step 3: Calculate the mass of O2 required.
Mass of O2 required = (Moles of O2 required) x (molar mass of O2)
Mass of O2 required = 0.02345 mol x 32 g/mol (molar mass of O2)
Mass of O2 required = 0.7504 g

Therefore, the mass of O2 needed to produce 0.563g of NO is approximately 0.7504 g, not 750 g.

To determine the mass of O₂ needed to produce a given amount of NO, we need to use stoichiometry and the balanced chemical equation.

First, let's calculate the molar mass of NO:
- The molar mass of N = 14.01 g/mol, and there are 4 moles of N in 4NO = 56.04 g/mol.
- The molar mass of O = 16.00 g/mol, and there are 1 mole of O in 4NO = 16.00 g/mol.

Therefore, the molar mass of NO is 56.04 g/mol + 16.00 g/mol = 72.04 g/mol.

Next, we need to convert the mass of NO (0.563 g) to moles:
- Moles of NO = mass of NO / molar mass of NO
- Moles of NO = 0.563 g / 72.04 g/mol ≈ 0.0078 mol (rounded to four decimal places).

According to the balanced equation, the stoichiometric ratio between O₂ and NO is 5:4. This means that for every 5 moles of O₂, 4 moles of NO are produced.

Now, use the mole ratio to find the moles of O₂:
- Moles of O₂ = Moles of NO × (5 moles of O₂ / 4 moles of NO)
- Moles of O₂ = 0.0078 mol × (5/4) ≈ 0.0098 mol (rounded to four decimal places).

Finally, convert the moles of O₂ to mass:
- Mass of O₂ = Moles of O₂ × molar mass of O₂
- Mass of O₂ = 0.0098 mol × 32.00 g/mol (rounded to two decimal places) ≈ 0.31 g.

Therefore, the mass of O₂ needed to produce 0.563 g of NO is approximately 0.31 grams, not 750 grams as you mentioned.