Two samples of nitrogen dioxide are decomposed into their constituent elements.

Question

Two samples of nitrogen dioxide are decomposed into their constituent elements. One sample 19.2 of oxygen and 8.40 g of nitrogen, and the other sample produces 12.0 g of oxygen and 5.25 g of nitrogen. Which pair of ratios accurately demonstrates that the results are consistent with the law of definite proportions? mass of oxygen/mass or nitrogen (1st sample) = 8.40 g/19.2 g = 0.438:mass of oxygen/mass of nitrogen (2nd sample) = 5.25 g/12.0 g = 0.438 mass of oxygen/mass or nitrogen (1st sample) = 19.2 g/8.40 g = 2.29:mass of oxygen/mass of nitrogen (2nd sample) = 1.20 g/5.25 g = 2.29 mass of oxygen/mass or nitrogen (1st sample) = 1.20 g/19.2 g = 0.625:mass of oxygen/mass of nitrogen (2nd sample) = 5.25 g/8.40 g = 0.625 mass of oxygen/mass or nitrogen (1st sample) = 19.2 g/12.0 g = 1.60:mass of oxygen/mass of nitrogen (2nd sample) = 8.40 g/5.25 g = 1.60

Explanation / Answer

Ans . Option B is correct

According to the law of definite proportions , the given compound must contain the same elements in the same proportion , irrespective of the source.

So here mass of oxygen / mass of nitrogen is 2.29 in both the samples , which is correctly represented in option b

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