12.976 g of lead combines with 2.004 g of oxygen to form PbO2 . PbO2 can also be produced by heating lead nitrate and it was found that the percentage of oxygen present in PbO2 is 13.38%. With the help of given information,illustrate the law of constant composition?
In first experiment
Total mass of compound =12.976+2.004=14.98g
%oygen =2.004/12.976*100
=13.38%
In 2nd experiment %oygen is given that is 13.38%
So it illustrates law of definite proportions
find the percent of Oxygen in Lead(IV) oxide.
percent: 2.004/(12.976+2.004)= 0.133778371 or 13.38Percent.
Of course, your mentioning of lead nitrate is silly.
The decomposition of PbO2 and the combination of Pb and O2 reflect the same percentage.
Solve kr ke photo nhi dal skte?
In first experiment
Total mass of compound =12.976+2.004=14.98g
%oygen =2.004/12.976*100
=13.38%
In 2nd experiment %oygen is given that is 13.38%
In first experiment
Total mass of compound =12.976+2.004=14.98g
%oxygen =2.004/12.976*100
=13.38%
In 2nd experiment %oygen is given that is 13.38%
The law of constant composition, also known as the law of definite proportions, states that a given compound is always composed of the same elements in the same proportion by mass.
Let's illustrate this law using the information provided:
1. The mass of lead (Pb) is 12.976 g.
2. The mass of oxygen (O) is 2.004 g.
3. The formula for lead dioxide (PbO2) tells us that it contains one lead atom and two oxygen atoms.
To determine if the law of constant composition holds true, we need to calculate the mass ratio of Pb to O in both cases:
For the first case:
- Mass of Pb = 12.976 g
- Mass of O = 2.004 g
Pb:O mass ratio = 12.976 g / 2.004 g = 6.471
For the second case:
- Given that PbO2 contains 13.38% oxygen.
Since we know that oxygen is 2.004 g, we can calculate the mass of PbO2 as follows:
Mass of PbO2 = 100% - 13.38% (oxygen) = 86.62% (lead)
Mass of PbO2 = 86.62% x 2.004 g = 1.736 g
Now let's calculate the mass ratio of Pb to O in the second case:
Mass of Pb = 1.736 g (from the mass of PbO2)
Mass of O = 2.004 g
Pb:O mass ratio = 1.736 g / 2.004 g = 0.867
Comparing the mass ratios for both cases:
- In the first case, the mass ratio of Pb to O is 6.471.
- In the second case, the mass ratio of Pb to O is 0.867.
Since the two mass ratios obtained for the different reactions are not equal, we can conclude that the law of constant composition is not satisfied in this specific example.
Therefore, the given information does not illustrate the law of constant composition.