Nitrogen forms five compounds with oxygen in which1.0g of nitrogen combines with0.572,1.14,1.73,2.28,2.85 of oxygen respectively. verify law of multiple proportions.

This is a very bad answer

They don't know how to explain
I suggest you should close this thing

I think answer should not only consider result but the process part should also be correct .

Bad answer

Answer process should be showing to understand it.

Answer should be showing to understand it.

It's very bad.

Its superb and logical thnku

To verify the law of multiple proportions, we need to compare the ratios of the masses of oxygen that combine with a fixed mass of nitrogen in different compounds.

Let's list the given data:
Mass of nitrogen = 1.0g
Mass of oxygen in compound 1 = 0.572g
Mass of oxygen in compound 2 = 1.14g
Mass of oxygen in compound 3 = 1.73g
Mass of oxygen in compound 4 = 2.28g
Mass of oxygen in compound 5 = 2.85g

Now, we can calculate the ratios of oxygen to nitrogen for each compound:

Ratio for compound 1 = 0.572g ÷ 1.0g = 0.572
Ratio for compound 2 = 1.14g ÷ 1.0g = 1.14
Ratio for compound 3 = 1.73g ÷ 1.0g = 1.73
Ratio for compound 4 = 2.28g ÷ 1.0g = 2.28
Ratio for compound 5 = 2.85g ÷ 1.0g = 2.85

Now, let's compare these ratios to see if they can be expressed as small whole-number ratios:

Ratios in descending order: 0.572, 1.14, 1.73, 2.28, 2.85

By observing these ratios, we can see that the ratios of oxygen to nitrogen in compounds 2, 3, and 4 are approximately double, triple, and quadruple the ratio in compound 1. Furthermore, the ratio in compound 5 is nearly five times the ratio in compound 1.

Therefore, the ratios follow a simple whole-number multiple relationship, which verifies the law of multiple proportions.

First, the law, which I copied verbatim from Wikipedia.

"If two elements form more than one compound between them, then the ratios of the masses of the second element which combine with a fixed mass of the first element will be ratios of small whole numbers."

Note that the 1.0 g nitrogen is fixed. Now look at the ratios of the others.
0.572; 1.14:1.73; 2.28; 2.85.
0.572/0.572 = 1.00
1.14/0.572 = 1.99 which rounds to 2.00
1.73/0.572 = 3.02 which rounds to 3.00
2.28/0.572 = ?
etc.