Question

A sample of h2so4 contains 2.02 g of hydrogen, 32.07 g of sulfur, and 64.00 g of oxygen. how many grams of sulfur and grams of oxygen are present in a second sample of h2so4 containing 7.27 g of hydrogen?

Answer 1

Answer : The mass of sulfur and oxygen are present in second sample is, 115.44 and 212.72 grams respectively.

Solution :

As we know that the component of elements are in fixed proportions in the compound.

First we have to calculate the total mass of first sample.

Total mass of first sample = 2.02 + 32.07 + 64 = 98.04 g

Now we have to calculate the % of hydrogen, sulfur and oxygen.

$\% \text{ of H}=\frac{\text{Mass of H}}{\text{Total mass of sample}}\times 100=\frac{2.02g}{98.04g}\times 100=2.06\%$

$\% \text{ of S}=\frac{\text{Mass of S}}{\text{Total mass of sample}}\times 100=\frac{32.07g}{98.04g}\times 100=32.71\%$

$\% \text{ of O}=\frac{\text{Mass of O}}{\text{Total mass of sample}}\times 100=\frac{64g}{98.04g}\times 100=65.27\%$

Now we have to calculate the total mass of second sample.

$\% \text{ of H}=\frac{\text{Mass of H}}{\text{Total mass of second sample}}\times 100\\\\2.06\%=\frac{7.27g}{\text{Total mass of second sample}}\times 100\\\\\text{Total mass of second sample}=352.91g$

Now we have to calculate the mass of sulfur and oxygen.

$\% \text{ of S}=\frac{\text{Mass of S}}{\text{Total mass of second sample}}\times 100\\\\\text{Mass of S}=32.71\times \frac{352.91}{100}=115.44g$

$\% \text{ of O}=\frac{\text{Mass of O}}{\text{Total mass of second sample}}\times 100\\\\\text{Mass of O}=65.27\times \frac{352.91}{100}=212.72g$

Therefore, the mass of sulfur and oxygen are present in second sample is, 115.44 and 212.72 grams respectively.

Answer 2

115,420 grams  of sulfur and 230, 336 grams  of oxygen are present in a second sample of h2so4 containing 7.27 g of hydrogen

Further explanation

Proust stated the Comparative Law that compounds are formed from elements with the same Mass Comparison so that the compound has a fixed composition of elements

In the same compound, although from different sources and formed by different processes, it will still have the same composition/comparison

With this law, we can calculate how many grams an element is needed to make a compound with a certain mass, as desired

The mass of compounding compounds can also be calculated.

For example, the mass ratio of oxygen (O) and hydrogen (H) elements in H₂O remains at 8: 1. So if you know the amount of mass of oxygen you can know the amount of hydrogen and water mass.

It is known that the mass ratio of H₂SO₄ compounds is:

H = 2.02 grams

S = 32.07 grams

O = 64 grams

So that the mass ratio of the three elements is: (we divide by the smallest mass of element H by 2.02 g)

H: S: O = 1: 15,876: 31,68

From the second H₂SO₄ sample it is known that the mass H is 7.27 grams, then the mass of the other elements:

S = 15,876 x 7.27 = 115,420 grams

O = 31.68 x 7.27 = 230, 336 grams

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Keywords: H₂SO₄, The mass of compounding compounds, Proust, Comparative Law