Nitrogen form five compound with oxygen in which 1.0 g of nitrogen combines with 0.572,1.14,1.73,2.28 and 2.85g of oxygen respectively .show dis figure agree with law of multiple proportion.
Take the first one.
mols N = 1/14 = 0.0714
mols O 1/16 = 0.0357
You can see N is twice that of O sot he formula is N2O. Go through the others in the same fashion to see NO, N2O3 ETC.
1:2:3:4:5
To determine if these figures agree with the law of multiple proportions, we need to compare the ratios of the masses of oxygen to the mass of nitrogen in each compound.
1. Compound 1: Nitrogen (N) combines with 0.572g of Oxygen (O)
The ratio of oxygen to nitrogen is 0.572g O / 1.0g N = 0.572:1
2. Compound 2: Nitrogen (N) combines with 1.14g of Oxygen (O)
The ratio of oxygen to nitrogen is 1.14g O / 1.0g N = 1.14:1
3. Compound 3: Nitrogen (N) combines with 1.73g of Oxygen (O)
The ratio of oxygen to nitrogen is 1.73g O / 1.0g N = 1.73:1
4. Compound 4: Nitrogen (N) combines with 2.28g of Oxygen (O)
The ratio of oxygen to nitrogen is 2.28g O / 1.0g N = 2.28:1
5. Compound 5: Nitrogen (N) combines with 2.85g of Oxygen (O)
The ratio of oxygen to nitrogen is 2.85g O / 1.0g N = 2.85:1
Now, let's simplify the ratios by dividing each value by the lowest value obtained in the above calculations.
1. Compound 1: 0.572:1 simplifies to 0.572:1
2. Compound 2: 1.14:1 simplifies to 1.14:1
3. Compound 3: 1.73:1 simplifies to 1.73:1
4. Compound 4: 2.28:1 simplifies to 2.28:1
5. Compound 5: 2.85:1 simplifies to 2.85:1
From these simplified ratios, we can observe that the ratio of oxygen to nitrogen in each compound is nearly in agreement with small whole numbers (1, 1, 2, 2, 3). This confirms the law of multiple proportions, which states that when two elements combine to form different compounds, the mass ratios are in small whole numbers.
Hence, the figures obtained for the different compounds of nitrogen and oxygen are in accordance with the law of multiple proportions.