Question

A 50.51g sample of a compound made from phosphorus and chlorine is decomposed. Analysis of the products showed that 11.39 g of phosphorus atoms were produced. Answer using three significant figures. What is the percent by mass of phosphorus? % What is the percent by mass of chlorine? %

Answer 1

Answer:

Mass percentage of phosphorus is 22.54%and mass percentage of chlorine is 77.46%.

Explanation:

Mass of the compound = 50.51 g

Mass of phosphorus atoms produced = 11.39 g

According to law of conservation of mass.

Mass of phosphorus atoms and chlorine atoms = Mass of the compound

Mass of the phosphorus = 50.51 g

Percentage of Phosphorus:

$\%(Phosphorus)=\frac{11.39 g}{50.51 g}\times 100=22.54\%$

Percentage of Chlorine:

$\%(Chlorine)=100\%-(\%(Phosphorus))=100\%-22.54\%=77.46\%$

Mass percentage of phosphorus is 22.54%and mass percentage of chlorine is 77.46%.

Answer 2

Ans: P = 22.5% and Cl = 77.5%

Given:

Total Mass of sample containing P and Cl = 50.51 g

Mass of P produced = 11.39 g

To determine:

Mass % of P and Cl

Explanation:

Mass % of a given element in a total mass is generally expressed as:

Mass % of element = [mass of element/total mass]*100

Here,

Total mass = mass of P + mass of Cl

mass of Cl = Total - mass of P = 50.51-11.39 = 39.12 g

% P = [11.39/50.51]*100 = 22.5%

%Cl = [39.12/50.51]*100 = 77.5%