in a compound of nitrogen and oxygen, 14.0 grams of nitrogen combines with 32.0 grams of oxygen. How much oxygen is required to combine with a sample of 10.5 grams of nitrogen in producing same compound? How do you do the math?
N.....O
14....32
10.5...x
Just make a ratio/proportion out of it and solve for x.
x = 32*(10.5/14) = ??
To determine the amount of oxygen required to combine with 10.5 grams of nitrogen, we can use the concept of stoichiometry.
1. Start by finding the molar masses of nitrogen (N) and oxygen (O). The molar mass of nitrogen is approximately 14.01 g/mol, and oxygen is approximately 16.00 g/mol.
2. Convert the given masses of nitrogen and oxygen into moles. Divide the mass of nitrogen (10.5g) by its molar mass (14.01 g/mol) to find the number of moles of nitrogen.
Moles of nitrogen = 10.5 g / 14.01 g/mol
3. Use the balanced chemical equation to determine the mole ratio between nitrogen and oxygen. From the given information, we know that 14.0 grams of nitrogen combine with 32.0 grams of oxygen. The balanced equation is required to determine the mole ratio:
N2 + O2 → Compound
4. Calculate the number of moles of oxygen corresponding to the moles of nitrogen by using the mole ratio obtained from the balanced equation. In this case, the mole ratio for nitrogen and oxygen is 1:1.
Moles of oxygen = Moles of nitrogen
5. Finally, convert the moles of oxygen back into grams by multiplying it by the molar mass of oxygen (16.00 g/mol).
Mass of oxygen = Moles of oxygen * Molar mass of oxygen
By following these steps, you can determine the amount of oxygen required to combine with 10.5 grams of nitrogen in producing the same compound.