Chemistry, 15.07.2019 17:30 Nanamoney5385

Achemist finds that 30.82 g of nitrogen will react with 17.60 g, 35.20 g, 70.40 g, or 88.00 g of oxygen to form four different compounds. calculate the mass of oxygen per gram of nitrogen in each compound.

Achemist finds that 30.82 g of nitrogen will react with 17.60 g, 35.20 g, 70.40 g, or 88.00 g of oxy

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Answer from: Webber07

Answer : The mass of oxygen per gram of nitrogen for four different oxygen are, 0.57, 1.14, 2.28 and 2.85 grams respectively.

Explanation :

First we have to calculate the mass of oxygen per gram of nitrogen for oxygen 1.

As, 30.82 g of nitrogen will react with 17.60 g of oxygen

So, 1 g of nitrogen will react with $\frac{17.60}{30.82}=0.57g$ of oxygen

Now we have to calculate the mass of oxygen per gram of nitrogen for oxygen 2.

As, 30.82 g of nitrogen will react with 35.20 g of oxygen

So, 1 g of nitrogen will react with $\frac{35.20}{30.82}=1.14g$ of oxygen

First we have to calculate the mass of oxygen per gram of nitrogen for oxygen 3.

As, 30.82 g of nitrogen will react with 70.40 g of oxygen

So, 1 g of nitrogen will react with $\frac{70.40}{30.82}=2.28g$ of oxygen

First we have to calculate the mass of oxygen per gram of nitrogen for oxygen 4.

As, 30.82 g of nitrogen will react with 88.00 g of oxygen

So, 1 g of nitrogen will react with $\frac{88.00}{30.82}=2.85g$ of oxygen

Therefore, the mass of oxygen per gram of nitrogen for four different oxygen are, 0.57, 1.14, 2.28 and 2.85 grams respectively.

Answer from: Keekee9847

0.57, 1.14, 2.28, and 2.85 grams respectively.The latter compound does not comply with Dalton's law.Further explanation

Let us calculate the mass of oxygen per gram of nitrogen in each compound.

First compound

$\boxed{ \ \frac{17.60 \ g \ of \ O}{30.82 \ g \ of \ N} = 0.57\ }$

Second compound

$\boxed{ \ \frac{35.20 \ g \ of \ O}{30.82 \ g \ of \ N} = 1.14\ }$

Third compound

$\boxed{ \ \frac{70.40 \ g \ of \ O}{30.82 \ g \ of \ N} = 2.28\ }$

Fourth compound

$\boxed{ \ \frac{88.00 \ g \ of \ O}{30.82 \ g \ of \ N} = 2.85\ }$

How do the numbers above support Dalton's atomic theory?

Let's find out the ratio that connects the results between the first, second, and third compounds above.

Between the first and second compounds: $\boxed{ \ 0.57 \div 1.14 = \boxed{ \ 1 \div 2 \ } \ }$ Between the second and third compounds: $\boxed{ \ 1.14 \div 2.28 = \boxed{ \ 1 \div 2 \ } \ }$ Between the first and third compounds: $\boxed{ \ 0.57 \div 2.28 = \boxed{ \ 1 \div 2 \ } \ }$

It all obeys the law of multiple proportions because the ratio is simple whole numbers.

Notes:

The law of multiple proportions was put forward by John Dalton. This law is one of the basic laws of stoichiometry.The law of multiple proportions states: if two elements can form more than one compound, the ratio of the mass of one element, which is compounded with a certain number of other elements, can be expressed in small whole-number ratios.Learn moreThe chemical formula of a compound Determine the mass of aspirin from the number of molecules The density of platinum

Keywords: A chemist finds that 30.82 g of nitrogen, oxygen, different compounds, calculate the mass of oxygen per gram of nitrogen, Dalton, the law of multiple proportions.

Answer from: Quest

answer: your mm

explanation:

Answer from: Quest

the answer is the first option

explanation:

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