A metal x with relative atomic mass 56 form an oxide with formula X2 O3 how many grams of metal will combine with 10g of oxygen:?(O=16)
56 *2 112g X will react with 3*16 = 48g O
10g O will react with 10gO / 48gO * 112gX =23.3g X
10 g x (4*atomic mass X/3*molar mass O2) = ?
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To answer this question, we need to determine the molar mass of the metal X and then use the molar ratio between the metal and oxygen to calculate the amount of metal needed.
1. Start by finding the molar mass of the metal X:
The relative atomic mass of X is given as 56. This means that the molar mass of X is 56 g/mol.
2. Calculate the molar mass of oxygen (O):
The molar mass of oxygen is given as 16 g/mol.
3. Determine the molar ratio between metal X and oxygen:
From the formula X2O3, we can see that for every 2 moles of X, we have 3 moles of O.
4. Calculate the amount of moles of oxygen in 10 g of O:
Using the molar mass of O (16 g/mol), we can calculate the number of moles as follows:
moles = mass / molar mass = 10 g / 16 g/mol = 0.625 mol
5. Use the molar ratio to find the amount of moles of metal X:
From the molar ratio, we know that for every 3 moles of O, we have 2 moles of X. So, we can set up a ratio:
3 moles O / 2 moles X = 0.625 mol O / x moles X
We cross multiply:
3 moles O * x moles X = 0.625 mol O * 2 moles X
3x = 1.25
x = 1.25 / 3 = 0.4167 moles
6. Calculate the mass of metal X:
Using the molar mass of X (56 g/mol), we can calculate the mass as follows:
mass = moles * molar mass = 0.4167 mol * 56 g/mol ≈ 23.33 g (rounded to two decimal places)
Therefore, approximately 23.33 grams of the metal X will combine with 10 grams of oxygen.